# Equilibrium Questions

We provide equilibrium practice exercises, instructions, and a learning material that allows learners to study outside of the classroom. We focus on equilibrium skills mastery so, below you will get all questions that are also asking in the competition exam beside that classroom. #### List of equilibrium Questions

Question NoQuestionsClass
1The solubility product of ( M g F_{2} ) is ( 7.4 x )
( 10^{-11} . ) Calculate the solubility of ( M g F_{2} ) in ( 0.1 mathrm{M} ) NaF solution.
A ( .7 .4 times 10^{-9} )
В. ( 3.7 times 10^{-9} )
c. ( 3.7 times 10^{-11} )
D. ( 7.4 times 10^{-11} )
11
2Equilibrium constants for four different
reactions are given as:
( boldsymbol{K}_{mathbf{1}}=mathbf{1 0}^{mathbf{6}}, boldsymbol{K}_{mathbf{2}}=mathbf{1 0}^{-mathbf{4}}, boldsymbol{K}_{mathbf{3}}=mathbf{1 0}, boldsymbol{K}_{mathbf{4}}= )
1. Which reaction will take maximum
time to attain equilibrium?
A ( cdot K_{1}=10^{6} )
B ( cdot K_{2}=10^{-4} )
( mathbf{c} cdot K_{3}=10 )
D. can’t predict
11
3A solution contaming ( N H_{4} C l ) and ( N H_{4} O H ) has ( [stackrel{ominus}{O} H]=10^{-6} m o l L^{-1} )
which of the following hydroxides would be precipitated when this solution in added in equal volume to a solution containing ( 0.1 mathrm{M} ) of metal ions?
A ( cdot M g(O H)_{2},left(K_{s p}=3 times 10^{-11}right) )
B. ( F e(O H)_{2}left(K_{s p}=8 times 10^{-16}right) )
c. ( C d(O H)_{2}left(K_{s p}=8 times 10^{-6}right) )
D. ( operatorname{AgOH}left(K_{s p}=5 times 10^{-3}right) )
11
4Q14. H, (g) + 1,(g) + 2HI ()
What is the relationship between K, and K?
11
514. The value of log K for a reaction
A B is:
(Given: AH,09 x = -54.07 kJ mol!, A.S… x = + 10 J mof,
and R= 8.31 JK-mol-1; 2.3030 ~ 8.314 x 298 = 5705)
(a) 5
(b) 10
(c) 95
(d) 100
11
6Give the molecular formula for
bleaching powder.
11
7Calculate ( K_{C} ) for the reaction:
( 2 H_{2}(g)+S_{2}(g) rightleftharpoons 2 H_{2} S(g) ) if ( 1.58 mathrm{mol} )
( boldsymbol{H}_{2} boldsymbol{S}, 1.27 mathrm{mol} boldsymbol{H}_{2}, ) and ( mathbf{2 . 7 8} times mathbf{1 0}^{-mathbf{6}} ) mol
of ( S_{2} ) are in equilibrium in a flask of capacity ( 180 mathrm{L} ) at ( 750 mathrm{C} )
A ( cdot K_{C}=124 times 10^{8} L ) mol ( ^{-1} )
B. ( K_{C}=1 times 10^{8} L ) mol( ^{-1} )
c. ( K_{C}=1 times 10^{-8} L mathrm{mol}^{-1} )
D. ( K_{C}=1 times 10^{7} L mathrm{mol}^{-1} )
11
8In some solutions, the concentration of
( H_{3} O^{+} ) remains constant even when
small amounts of strong acid or strong base are added to them. These solutions
are known as:
A. colloidal solutions
B. buffer solutions
c. true solutions
D. ideal solutions
11
9How many moles of acetic acid and
sodium acetate each should be
dissolved to prepare one litre of 0.063 molar buffer solution of pH ( 4.5 ? )
( left(K_{a} text { for } C H_{3} C O O H=1.8 times 10^{-5}right) )
11
10An increase in pressure will change the equilibrium by:
A. shifting to the side where a smaller volume results
B. shifting to the side where a larger volume results
C. favoring the endothermic reaction
D. favoring the exothermic reaction
E. none of the above
11
11Solubility of Potassium nitrate:
A. increases with temperature
B. decreases with temperature
C. remains constant with temperature
D. is not related to the temperature fluctuations
11
12Consider the reaction equilibrium Ice( rightleftharpoons_{text {Lesservier}}-boldsymbol{X k c a l} )
Greatervolume
The favourable condition for forward
reaction are:
A. low temperature, high pressure and excess of ice
B. low temperature, low pressure and excess of ice
c. high temperature, low pressure and excess of ice
D. high temperature, high pressure and excess of ice
11
13At ( 373 mathrm{K} ), steam and water are in
equilibrium and ( Delta H=40.98 mathrm{kJ} ) mol( ^{-1} )
What will be ( Delta S ) fro conversion of
water into steam?
( boldsymbol{H}_{2} boldsymbol{O}_{(l)} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(g)} )
A ( cdot 109.8 ) J ( K^{-1} m o l^{-1} )
B . 31 J ( K^{-1} ) mol ( ^{-1} )
c. 21.98 J ( K^{-1} m o l^{-1} )
D. 326 J ( K^{-1} ) mol ( ^{-1} )
11
14Which of the following mixtures in aqueous solution of equimolar concentration acts as a buffer solution?
A. ( H N O_{3}+N a O H )
в. ( H_{2} S O_{4}+K O H )
c. ( N H_{4} O H(text {excess})+H C l )
D. ( C H_{3} C O O H+N a O H(e x c e s s) )
11
15Which of the following represents a conjugate acid/base pair?
A. ( N a^{+} / C l^{-} )
в. ( H C l / H^{+} )
c. ( H_{2} C O_{3} / C O_{3}^{2} )
D. ( N H_{3} / N H_{4}^{+} )
E . ( K^{+} / O H^{-} )
11
16When equilibrium is attained, the concentration of each of the reactants
and products become equal.
A. True
B. False
c. Ambiguous
D. None of these
11
17Q. 25 Ionisation constant of a weak base MOH, is given expression
[M”] [OH-]
[MOH]
Values of ionisation constant of some weak bases at a particular
temperature are given below
Base Dimethylamine Urea Pyridine Ammonia
no 5.4 x 10-
4 1 .3 x 10 * 1.77 x 10-9 1.77 x 10-5
Arrange the bases in decreasing order of the extent of their jonisation at
equilibrium. Which of the above base is the strongest?
11
18If ( K_{a 1} ) and ( K_{a 2} ) are the ionization constants of ( boldsymbol{H}_{3} stackrel{+}{boldsymbol{N}} boldsymbol{C} boldsymbol{H} boldsymbol{R} boldsymbol{C O O} boldsymbol{H} ) and
( boldsymbol{H}_{3}^{+} boldsymbol{N} boldsymbol{C} boldsymbol{H} boldsymbol{R} boldsymbol{C O O}^{-}, ) respectively, the ( boldsymbol{p} boldsymbol{H} )
of the solution at the isoelectric point
is:
A ( cdot p H=p K_{a 1}^{circ}+p K_{a 2}^{circ} )
в.
[
p H=left(p K_{a 1}^{circ} p K_{a 2}^{circ}right)^{frac{1}{2}}
]
c.
[
p H=left(p K_{a_{1}}^{circ}+p K_{a 2}^{circ}right)^{frac{1}{2}}
]
D. ( _{p H}=frac{left(p K_{a 1}^{circ}+p K_{a 2}^{circ}right)}{2} )
11
19saturated solution of ( A g C l ) then which
of the following plot is correct?
( A )
B.
( c )
( D )
11
20On passing ( boldsymbol{H}_{2} boldsymbol{S} ) into a solution
containing both ( Z n^{2-} ) and ( C u^{2-} ) in
acidic medium, only CuS gets precipitated. This is because:
( mathbf{A} cdot K_{s p} ) of ( C u SK_{s p} ) of ZnS
D. cus is more stable then zns
11
21People use bases called antacids due
to:
A. get rid of stomach pain
B. irritation
c. both ( (A) ) and ( (B) )
D. none of the above
11
22The equilibrium constant of a reaction is 300 , if the volume of the reaction
flask is tripled, the equilibrium constant will be:
A . 100
B. 300
( c .250 )
D. 150
11
236. Consider the following equilibrium in a closed
container:
N204(8) 2NO2(g)
At a fixed temperature, the volume of the reaction
container is halved. For this change, which of the given
statements holds true regarding the equilibrium constant
(KD) and degree of dissociation (a)?
(a) Neither K, nor a changes
(b) Both Ko and a change
(c) K, changes, but a does not change
(d) K, does not change, but a changes
11
24Maximum change in ( p H ) is observed
when 50 of ( 1 M K O H ) solution is
A . 25 ml. of ( 2.5 N ) HCl
B. ( 50 mathrm{ml} ) of ( 1 mathrm{N} ) HCl
c. ( 30 mathrm{ml} ) of ( 2 mathrm{N} ) HCl
D. ( 50 mathrm{ml} ) distilled water
11
25The label of a bottle containing a dilute aqueous solution of an acid become damage Only its concentration was
readable ( A ) pH meter was nearby, and a quick measurement showed that the
hydrogen ion concentration is equal to the value on the label. Which of the
following four acids that could have been the solution if the pH changed one unit after a tenfold dilution?
This question has multiple correct options
( mathbf{A} cdot H C l O_{4} )
B. ( H_{3} B O_{3} )
с. ( C H_{3} ) СООН
D. ( H N O_{3} )
11
26In aqueous solution, the proton exists
as a (acid/base)
11
27For the reaction, ( boldsymbol{S n O}_{2}(boldsymbol{s})+boldsymbol{2} boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons )
( boldsymbol{S} boldsymbol{n}(l)+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) the equilibrium
mixture of steam and hydrogen
contained ( 45 % ) and ( 24 % H_{2} ) at ( 900 mathrm{K} )
and ( 1100 mathrm{K} ) respectively. Calculate ( boldsymbol{K}_{boldsymbol{P}} )
at both the temperatures. Generally should it be higher or lower temperatures for better reduction of
( boldsymbol{S} boldsymbol{n} boldsymbol{O}_{2} ? )
( mathbf{A} cdot therefore K_{C_{2}}=1.03 )
( mathbf{B} cdot therefore K_{C_{2}}=5.02 )
( mathbf{c} cdot therefore K_{C_{2}}=15.01 )
( mathbf{D} cdot therefore K_{C_{2}}=10.03 )
11
28( C O_{2} ) gas along with solid (Y) is obtained when sodium salt (X) is
heated. ( (X) ) is again obtained when ( C O_{2} )
gas is passed into aqueous solution of
(Y). Identify ( (X) ) and ( (Y) ) respectively.
A. ( N a_{2} C O_{3}, N a_{2} O )
в. ( N a_{2} C O_{3}, ) NaOH
с. ( N a H C O_{3}, N a_{2} C O_{3} )
D. ( N a_{2} C O_{3}, N a H C O_{3} )
11
29In the reaction ( C(s)+C O_{2}(g) rightleftharpoons )
( 2 C O(g), ) the equilibrium pressure is
12 atm. If ( 50 % ) of ( C O_{2} ) reacts till
equilibrium then ( boldsymbol{K}_{boldsymbol{p}} ) will be :
A . 12 atm
B. 6 atm
( c .20 ) atm
D. 24 atm
11
30State True or False.
Almost every liquid is either an acid or a base.
A. True
B. False
11
31If the equilibrium constant of the reaction of weak acid ( boldsymbol{H} boldsymbol{A} ) with strong
base is ( 10^{9} ), then ( mathrm{pH} ) in ( 0.1 M ) NaA is:
A . 5
B. 9
( c cdot 7 )
D.
11
32For the reaction
( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons )
( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) )
which one is correct representation:
A ( cdot K_{P}=left(P_{H_{2}} partialright)^{2} )
в. ( K_{C}=left[H_{2} Oright]^{2} )
( mathbf{c} cdot K_{p}=K_{c}(R T)^{2} )
D. all of these
11
33( A t 817, K_{p} ) for the reaction between
( C O_{2}(g) ) and excess hot graphite ( (s) ) is
10 atm.
(a) The sum of equilibrium
concentration of the gases at ( 817^{circ} mathrm{C} ) is
( X M ) and a total pressure of 5 atm.
(b) At ( Y ) atm total pressure, the gas
contains ( 5 % C O_{2} ) by volume.
The value of ( 1000(X+Y) ) is
11
34Which of the following compounds can be called as non-electrolytes?
A. ( C_{6} H_{12} O_{6} )
в. ( C_{2} H_{5} O H )
( mathbf{c} cdot C_{2} H_{6} )
D. All of the above
11
35The progress of reaction ( boldsymbol{A}(boldsymbol{g}) rightleftharpoons )
( boldsymbol{x} boldsymbol{B}(boldsymbol{g})+boldsymbol{y} boldsymbol{C}(boldsymbol{g}) ) with time is presented
in figure. What is the value of ( boldsymbol{K}_{c}^{0} ) at
( mathbf{3 0 0 K} ? )
( A )
B.
( c .3 )
( D )
11
36Many lead salts are often used as pigments. If ( boldsymbol{P b S O}_{4}left(boldsymbol{K}_{s p}=mathbf{1 . 6} times mathbf{1 0}^{-8}right) )
were used in an unglazed ceramic bowl
how many milligrams of lead (II) could dissolve per liter of water?
( A cdot 43 )
B. 35
( c cdot 11 )
D. 38
11
37How many mole of ( boldsymbol{H} boldsymbol{C} boldsymbol{N} ) will be required to prepare one litre buffer solution of ( boldsymbol{p} boldsymbol{H}=mathbf{1 0 . 4} ) using ( mathbf{0 . 0 1} ) mol
NaC N?
(Given: ( left.boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{C N})=boldsymbol{4} times mathbf{1 0}^{-10}right) )
( mathbf{A} cdot 2 times 10^{-2} mathbf{M} )
В. ( 9 times 10^{-4} ) М
( mathbf{c} cdot 4 times 10^{-4} mathrm{M} )
D. ( 9 times 10^{-3} mathrm{M} )
11
38The solubility product of ( B a S O_{4} ) is
( 1.5 times 10^{-9} . ) The precipitation in a
( 0.01 M B a^{2+} ) solution will start on
adding ( H_{2} S O_{4} ) of concentration:
A ( cdot 1 times 10^{-9} M )
в. ( 1.5 times 10^{-7} M )
c. ( 2 times 10^{-7} M )
D. ( 1 times 10^{-6} M )
11
39The number of ( boldsymbol{H}^{+} ) ions in ( 1 mathrm{cc} ) of ( mathrm{a} )
solution of ( p H=13 ) is:
A. ( 6.023 times 10^{7} )
B. ( 1 times 10^{-13} )
c. ( 6.023 times 10^{13} )
D. ( 1 times 10^{16} )
11
40The ( p H ) of an acid buffer can be raised
by 2 units by
A. Increaseing the concentration of both weak acid and salt by two moles
B. Increasing the concentration of both the acid and salt by 10 times
c. Diluting the solution by 10 times
D. Increasing the concentration of the salt by 10times and decreasing concentration of the acid by 10 times
11
41To a solution of acetic acid, solid
sodium acetate is added gradually. When ( x ) mole of salt is added, the pH has
a certain value. If y mole of salt is
added, the pH change by 0.6 units to the previous pH. What is the ratio of ( x ) and
y?
11
42Which of the following reactions have
( boldsymbol{K}_{boldsymbol{p}}<boldsymbol{K}_{boldsymbol{c}} )
This question has multiple correct options
A ( cdot H_{2}(g)+I_{2}(g) rightleftharpoons 2 H I(g) )
в. ( C O(g)+C l_{2}(g) rightleftharpoons C O C l_{2}(g) )
c. ( 2 B r C l(g) rightleftharpoons B r_{2}(g)+C l_{2}(g) )
D. ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) )
11
43Polar covalent compounds are
in gaseous state, but ionizes in aqueous solution state.
A. electrolytes
B. non-electrolytes
c. soluble
D. none of the above
11
44When we add a pinch of sodium hydrogen carbonate in a flask containing ethanoic acid a reaction
takes place. What will be the observation when we carry out the
reaction?
A. Milky solution
B. Bubble formation
c. Solution turns red
D. Brisk effervescence
11
45The species among the following, which can act as acid as well as base is?
A ( . H S O_{4}^{-} )
B. ( S O_{4}^{2} )
c. ( H_{3} O^{+} )
D. ( C l )
11
46An equilibrium constant of ( 10^{-4} ) for a
reaction means, the equilibrium is
A. largely towards backward direction
B. largely towards forward direction
c. equally poised
D. never established
11
47The pH of 0.001M HCN is:
( A cdot 3 )
в. 1
c. between 3 & 7
D. 7
11
48Q6. Define solubility product.11
49For the reaction
( mathbf{2} boldsymbol{A}+boldsymbol{B} rightleftharpoons mathbf{3} boldsymbol{C} ) at ( mathbf{2} mathbf{9 8} boldsymbol{K}, boldsymbol{K}_{boldsymbol{c}}=mathbf{4 9} )
A ( 3 L ) vessel contains 2,1 and 3 moles of
( A, B ) and ( C ) respectively. The reaction at
the same temperature:
A. must proceed in forward direction
B. must proceed in backward direction
c. must be in equilibrium
D. cannot be predicted
11
501.0 ( mathrm{ml} ) of a solution of ( mathrm{H} C l ) with a ( p H ) of
4.0 is added it to ( 9.0 mathrm{ml} ) of distilled
water, the ( p H ) of the final solution will
be:
A. The pH would remain unchanged.
B. The pH would rise to 5.5
c. The pH would rise to 5.0
D. The pH would be unmeasurable due to the amount of dilution
E. The pH would rise to 7.0
11
51If volume ratio of ( 0.02 M H C l ) and
( 0.02 M B O H ) (a weak base) mixed to
make ( 200 mathrm{mL} ) of buffer of ( p H=7 ) is
( 2.23: X . ) The value of ( X ) is:
( boldsymbol{K}_{b} ) for ( boldsymbol{B O H}=mathbf{8 . 1} times mathbf{1 0}^{-mathbf{8}} )
( A )
B. 5
( c cdot 0.2 )
D. 2.5
11
52Assertion
( H C l rightarrow H^{+}+C l^{-} ) is an ionization
Reason
The electron is initially shared between both atoms, thus the dissociation event
into ions involves the transfer of an
electron from one atom to the other.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
53lonic solutions are good conductors
of Electricity.
A. True
B. False
11
54Buffer solution is prepared by mixing:
A. Strong acid + its salt of strong base
B. Weak acid + its salt of strong base.
c. Strong acid + its salt of weak base
D. None of the above
11
55Five solutions ( A, B, C, D, E ) when
tested with universal indicator showed
( p H ) as 4,1,11,7 and 9 respectively. Which solution is weakly acidic?
( A cdot A )
B. B
( c cdot c )
( D . ) D
11
56The solubility of ( A_{2} X_{5} ) is ( x ) mol ( d m^{-3} )
Its solubility product is:
A ( cdot 36 x^{6} )
В. ( 64 times 10^{4} x^{7} )
c. ( 126 x^{7} )
D. ( 1.25 times 10^{4} x^{7} )
11
57Q9. Give two characteristics of a buffer solution.
Ana
L.
IT
11
58For which of the following reactions will the equilibrium mixture contain an
appreciable concentration of both reactants and products?
A ( cdot C l_{2}(g) rightleftharpoons 2 C l(g) ; K_{c}=6.4 times 10^{-39} )
B. ( C l_{2}(g)+2 N O(g) rightleftharpoons 2 N O C l(g) ; K_{c}=3.7 times 10^{8} )
c. ( C l_{2}(g)+2 N O(g) rightleftharpoons 2 N O_{2} C l(g) ; K_{c}=1.8 )
D. ( H_{2}(g)+I_{2}(g) rightleftharpoons 2 H I(g) . K_{c}=49 )
11
59For the reaction ( 2 H I(g) Leftrightarrow H_{2}(g)+ )
( I_{2}(g), ) the degree of dissociation ( (alpha) ) of
( H I(g) ) is related to the equilibrium
constant, ( boldsymbol{K}_{boldsymbol{p}} ) by the expression:
( ^{mathrm{A}} cdot frac{1+2 sqrt{K_{p}}}{2 sqrt{K_{p}}} )
B. ( sqrt{frac{1+2 K_{p}}{2}} )
( ^{mathrm{c}} cdot sqrt{frac{2 K_{p}}{1+2 K_{p}}} )
D. ( frac{2 sqrt{K_{p}}}{1+2 sqrt{K_{p}}} )
11
60The standard reduction potential of two reactions are given. ( boldsymbol{A} boldsymbol{g} boldsymbol{C l}_{(s)}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g}_{(s)}+boldsymbol{C l}_{(a q)}^{-} ; boldsymbol{E}^{ominus}= )
( mathbf{0 . 2 2 V} )
(i)
( boldsymbol{A} boldsymbol{g}_{(a q)}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g}_{(s)} ; boldsymbol{E}^{ominus}=mathbf{0 . 8 0 V} )
The solubility product of ( A g C l ) under standard conditions of temperature is:
A ( .1 .6 times 10^{-5} )
В. ( 1.5 times 10^{-8} )
c. ( 3.2 times 10^{-10} )
D. ( 1.5 times 10^{-10} )
11
61What weight of sodium nitrate will
separate when a saturated solution
containing 50 gram of water is cooled
from ( 50^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ) ? The solubility of
( N a N O_{3} ) at ( 50^{circ} C ) and ( 30^{circ} C ) is 114 g and 86 g respectively.
11
62lonization of phosphoric acid gives:
A ( cdot H_{2} P O_{4}^{-} )
в. ( H P O_{4}^{-2} )
( mathrm{c} cdot P O_{4}^{-3} )
D. all of these
11
63Assertion ( : H C O_{3}^{-} ) can act as a Bronsted acid or a Bronsted base.
Reason ( : H C O_{3}^{-} ) can donate a proton to
form ( C O_{3}^{2-} ) or accept a proton to form
( boldsymbol{H}_{2} boldsymbol{C} boldsymbol{O}_{3} )
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct and Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
E. Both Assertion and Reason are incorrect
11
64Calculate the degree of ionization and ( left[boldsymbol{H}_{3} boldsymbol{O}^{+}right] ) of ( mathbf{0 . 0 1} boldsymbol{M} boldsymbol{C H}_{3} boldsymbol{C O O H} )
solution. The equilibrium constant of acetic acid is ( 1.8 times 10^{-5} )
11
65Which among the following resists a rapid change of pH?
A. Buffer
B. Indicator
C. Arrhenius acid
D. Arrhenius base
E. Neutral condition
11
66100ml of a solution of HCl with pH value 3 is diluted with ( 400 mathrm{ml} ) of water. The
new pH of the solution is?
A. 3.7
B. 5.3
c. 4.2
D. 5.6
11
67Calculate the ratio of ( H C O O^{-} ) and ( F^{-} )
in a mixture of ( 0.2 M ) HCOOH ( left(K_{a}=right. )
( left.2 times 10^{-4}right) ) and ( 0.1 M H Fleft(K_{a}=6.6 timesright. )
( left.10^{-4}right) )
A .1: 6.6
B. 1: 3.3
c. 2: 3.3
D. 3.3 : 2
11
68How much ( N a F ) should be added to 100
mL of solution having ( 0.016 M ) in ( S r^{2}+ )
ions to reduce its concentration to
( 2.5 times 10^{-3} M ?left(K_{s p} S r F_{2}=8 times 10^{-10}right) )
A. 0.098 g
ggg ( . . .998 )
B. 0.168 g
c. 0.177 g
D. 0.118 g
11
69For the reaction, ( 2 N O(g)+2 H_{2}(g) rightarrow )
( N_{2}(g)+2 H_{2} O(g) ) the rate expression
can be written in the following ways:
( left{boldsymbol{d t}left[boldsymbol{N}_{2}right] / boldsymbol{d} tright}= )
( boldsymbol{k}_{1}[boldsymbol{N} boldsymbol{O}]left[boldsymbol{H}_{2}right] ;left{boldsymbol{d}left[boldsymbol{H}_{2} boldsymbol{O}right] / boldsymbol{d} boldsymbol{t}right)= )
( boldsymbol{k}[boldsymbol{N} boldsymbol{O}]left[boldsymbol{H}_{2}right] )
( {-boldsymbol{d}[boldsymbol{N} boldsymbol{O}] / boldsymbol{d} boldsymbol{t}}= )
( boldsymbol{k}_{mathbf{1}}^{prime}[boldsymbol{N} boldsymbol{O}]left[boldsymbol{H}_{2}right] ;left{-boldsymbol{d}left[boldsymbol{H}_{2}right] / boldsymbol{d} tright}= )
( k_{1}^{prime prime}[N O]left[H_{2}right] )
The relation ship between ( k, k_{1}, k_{1}^{prime} ) and
( k_{1}^{prime prime} ) is:
11
70Which one of the following is not a
Lewis Acid?
( mathbf{A} cdot B F_{3} )
в. ( A l C l_{3} )
c. ( B e C l_{2} )
D. ( operatorname{SnCl}_{2} )
11
71The term ( p H ) comes from:
A. hydrogen purity
B. pure Hydrogen
c. hydrogen power
D. purity of Hydrogen
11
72In a reaction, ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C}, mathbf{2 . 0} ) mole of
( A 3.0 ) mole of ( B ) and 2.0 mole of ( C ) are
placed in a ( 2.0 L ) flask and the
equilibrium concentration of ( boldsymbol{C} ) is 0.5 mole ( / L . ) The equilibrium constant
( K ) for the reaction is
( mathbf{A} cdot 0.073 )
B. 0.147
( c .0 .05 )
D. 0.026
11
73The dissociation constant of uric acid is
( boldsymbol{K}_{boldsymbol{a}}=mathbf{4 . 0} times mathbf{1 0}^{-mathbf{6}} boldsymbol{M} . ) The ( boldsymbol{p} boldsymbol{H} ) of a
sample is ( 6.0 . ) What is the ratio of urate
ion to uric acid in the urine??
11
74The specific conductance at ( 298 mathrm{K} ) of AgCl solution In water was determined
to be ( 1.826 times 10^{-6} ) ohm ( ^{-1} mathrm{cm}^{-1} . ) The ionic
conductances ( A g^{+} ) and ( C l^{-} ) are 61.92 and 76.34 respectively. What is the solubility of AgCl in water?
A ( cdot 2.1 times 10^{-4} mathrm{gL}^{-1} )
B . ( 1.32 times 10^{-5} mathrm{gL}^{-1} )
c. ( 1.9 times 10^{-3} mathrm{gL}^{-1} )
D. 2.1 ( times 10^{-6} mathrm{gL}^{-1} )
11
75One mole of ( boldsymbol{H}_{2}, boldsymbol{2} ) moles of ( boldsymbol{I}_{2} ) and ( boldsymbol{3} )
moles of ( H I ) are injected in a one litre flask. What will be the concentration of
( boldsymbol{H}_{2}, boldsymbol{I}_{2} ) and ( boldsymbol{H} boldsymbol{I} ) at equilibrium when ( boldsymbol{K}_{boldsymbol{c}} )
is ( 45.9 ? )
11
76An equilibrium mixture in a vessel of
capacity 100 litre contain 1 mol ( N_{2}, 2 ) mol
( O_{2} ) and 3 mol ( N O . ) Number of moles of
( O_{2} ) to be added so that at new
equilibrium the conc. of ( N O ) is found to be 0.04 mol/lit is:
A . ( 101 / 18 )
в. ( 101 / 9 )
c. ( 202 / 9 )
D. none of these
11
77A reaction system in equilibrium
according to the equation ( 2 S O_{2}+ )
( O_{2} rightleftharpoons 2 S O_{3} ) in 1 litre reaction vessel at
a given temperature was found to
contain 0.11 mol of ( S O_{2}, 0.12 ) of ( S O_{3} ) and
0.05 mol of ( O_{2 .} ) Another 1 litre reaction
vessel contains 64 g of ( S O_{2} ) at the
same temperature. What mass of ( boldsymbol{O}_{2} )
must be added to this vessel in order
that at equilibrium half of ( S O_{2} ) is
oxidised to ( boldsymbol{S O}_{3} ) ?
A. 9.34 g
в. 10.87
c. ( 21.3 mathrm{g} )
D. 32.4 g
11
78Calculate : ( K_{a} ) for ( H C N ) given
( boldsymbol{K}_{b}left(boldsymbol{C N}^{-}right)=mathbf{2 . 5} times mathbf{1 0}^{-mathbf{5}} )
A ( cdot 10^{-5} )
В. ( 2 times 10^{-7} )
c. ( 4 times 10^{-10} )
D. None of these
11
79A monoprotic acid in ( 100 M ) solution is ( 0.001 % ) ionized. The dissociation
constant of this acid is:
A ( cdot 1.0 times 10^{-3} )
B. ( 1.0 times 10^{3} )
c. ( 1.0 times 10^{-8} )
D. ( 1.0 times 10^{-10} )
11
80Select the correct statements:
This question has multiple correct options
A. The value of ( Q_{c} ) for a given reaction is constant.
B. A change in the physical state of a gaseous product shows a change in the value of equilibrium constant of that reaction.
C the value of ratio ( frac{Q_{c}}{K_{c}} ) can be used to predict the direction in which a system will proceed spontaneously towards equilibrium.
D. The rate constants for forward and backward reaction
for a reversible reaction always increases with temperature but their ratio ( left(i . e ., frac{K_{f}}{K_{b}}right) ) may increase or decrease with temperature.
11
81In order to prepare a buffer of ( P^{H} 8.26 )
the amount of ( left(N H_{4}right)_{2} S O_{4} ) required to
be mixed with 1L of 0.1 M ( boldsymbol{N} boldsymbol{H}_{mathbf{3}}left(boldsymbol{p} boldsymbol{K}_{boldsymbol{b}}=right. )
4.74) is:
A . 5 mol
B. 0.5 mol
c. 10 mol
D. 1 mol
11
82A solution contains ( 0.4 M C H_{3} C O O H )
and ( 0.2 M C H_{3} C O O N a . ) Calculate the
concentration of ( boldsymbol{H}^{+} ) ions. The
ionisation constant of acetic acid is
( 1.8 times 10^{-5} )
11
83Which among the following represent the conjugate acid/base pairs? This question has multiple correct options
A ( cdot H_{3} O^{+} / H_{2} O )
в. ( H_{2} S O_{4} / S O_{4}^{2} )
c. ( H C O_{3}^{-} / C O_{3}^{2} )
D. All are conjugate acid/ base pairs
11
84Assertion
Assertion: Higher order ionization constants ( left(boldsymbol{K}_{a_{2}}, boldsymbol{K}_{a_{3}}right) ) are smaller than
the lower order ionization constant ( boldsymbol{K}_{boldsymbol{a}_{mathbf{1}}} ) of polyprotic acid.
Reason
Reason: Polyprotic acid solutions contain a mixture of acids.
A. If both the assertion and reason are true and reason is the correct explanation of assertion
B. If both the assertion and reason are true but reason is not the correct explanation of assertion.
c. If assertion is true but reason is false
D. If both assertion and reason are false
11
85Calculate the degree of ionization of
( 0.05 mathrm{M} ) acetic acid of its ( _{p} boldsymbol{K}_{a} ) value is 4.74. How is the degree of dissociation affected when its solution is also (a)
( 0.01 mathrm{M} ) and
(b) ( 0.1 mathrm{M} ) in hydrochloric acid?
11
86Which of the following expressions
is/are not true?
( mathbf{A} cdotleft[H^{+}right]=left[O H^{-}right]=sqrt{K_{w}} ) for a neutral solution at al
temperatures
B ( cdotleft[H^{+}right]>sqrt{K_{w}} &left[O H^{-}right]<sqrt{K_{w}} ) for an acidic solution
( mathbf{C} cdotleft[H^{+}right]sqrt{K_{w}} ) for an alkaline solution
D ( cdotleft[H^{+}right]=left[O H^{-}right]=10^{-7} M ) for a neutral solution at all
temperatures
11
87Calculate the dissociation constant of
( N H_{4} O H ) at ( 298 mathrm{K}, ) if ( triangle H^{ominus} ) and ( Delta S^{ominus} ) for
the given changes are as follows:
( boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{H}^{oplus} rightleftharpoons stackrel{oplus}{boldsymbol{N}} boldsymbol{H}_{4} )
( Delta H^{ominus}=-52.2 k J m o l^{-1}, Delta S^{ominus}= )
( mathbf{1 . 6 7} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} )
( boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{H}^{oplus}+stackrel{ominus}{boldsymbol{O}} boldsymbol{H} ; boldsymbol{Delta} boldsymbol{H}^{ominus}= )
( mathbf{5 6 . 6} k J mathbf{m o l}^{-1} )
( Delta S^{ominus}=-76.53 J K^{-1} m o l^{-1} )
begin{tabular}{l}
A. ( K_{b}=1.7 times 10^{-5} ) \
hline
end{tabular}
в. ( K_{b}=1.7 times 10^{-3} )
c. ( K_{b}=1.7 times 10^{-1} )
D. ( K_{b}=3.4 times 10^{-5} )
11
88LIO 5 D.LT
025. Does the number of moles of reaction products increase, decrease or remain same when each of
the following equilibria is subjected to a decrease in pressure by increasing the volume?
(i) PC (g) = PCI,() + C1 (8)
(ii) CaO(s) + CO.(g) – CaCO3(s)
(iii) 3Fe(s) + 4H2O(g) = Fe, (s) + 4H2 (8)
11
89( 20 mathrm{ml} ) of ( 0.2 mathrm{M} H C N ) mix with ( 10 mathrm{ml} ) of
0.2 M ( N a O H, ) then calculate ( p H ) of resulting mixture, ( p K a ) value of ( H C N )
is ( 5:- )
A . 6
B. 7.5
( c .5 )
D. 11
11
90Conjugate base of a weak acid has ( boldsymbol{K}_{b}=mathbf{1 0}^{-9} . ) The equilibrium constant
for the reaction of acid with strong base is:
( mathbf{A} cdot 10^{-19} )
B . ( 10^{-3} )
( c cdot 10^{9} )
D. ( 10^{5} )
11
91Calcium lactate is a salt of weal organic acid and strong base represented as ( boldsymbol{C} boldsymbol{a}(boldsymbol{L} boldsymbol{a} boldsymbol{C})_{2} cdot boldsymbol{A} ) saturated solution of
( boldsymbol{C} boldsymbol{a}(boldsymbol{L} boldsymbol{a} boldsymbol{C})_{2} ) contains ( boldsymbol{0} . boldsymbol{6} ) mole in ( boldsymbol{2} ) litre
solution. ( p O H ) of solution is ( 5.60 . ) If ( 90 % ) dissociation of the salt takes place then
what is ( p K_{a} ) of lactic acid?
A. ( 2.8-log (0.54) )
B. ( 2.8+log (0.54) )
c. ( 2.8+log (0.27) )
D. None of these
11
92The equilibrium expression, ( boldsymbol{K}=left[boldsymbol{C O}_{2}right] )
represents the reaction:
A. ( C(s)+O_{2}(g) rightleftharpoons C O_{2}(g) )
B. ( C O(g)+frac{1}{2} O_{2}(g) rightleftharpoons C O_{2}(g) )
c. ( operatorname{CaCO}_{3}(s) rightleftharpoons C a O(s)+C O_{2}(g) )
D. ( C O_{2}(g) rightleftharpoons C(s)+O_{2}(g) )
E ( cdot operatorname{CaO}(s)+C O_{2}(g) rightleftharpoons operatorname{CaCO}_{3}(s) )
11
93toppr
to the processes that occur in living organisms. This primarily because the functioning of enzymes-catalysts for these processes – is sharply pH dependent. The normal pH value of blood plasma is ( 7.4 . ) Severe illness or death
can result from sustained variations of
a few tenths of pH unit.
Among the factors that lead to a condition of acidosis, in which there is a
decrease in the pH of blood are heart failure, kidney failure diabetes mellitus
persistent diarrhoea or a long term high protein diet.A temporary condition of acidosis may result from prolonged, intensive exercise. Alkalosis, which
causes increase in pH of blood may occur as a result of severe vomiting over breathing or exposure to high altitudes.

Several factors are involved in the
control of the pH of blood. A particularly important one is the ratio of dissolved ( H C O_{3}^{-} ) to ( H_{2} C O_{3} . C O_{2}(g) ) is
moderately soluble in water and in aqueous solution reacts only to a
limited extent to produce ( boldsymbol{H}_{2} boldsymbol{C} boldsymbol{O}_{3} )
( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{H}_{2} boldsymbol{C} boldsymbol{O}_{3}(boldsymbol{a} boldsymbol{q}) )
( boldsymbol{H}_{2} boldsymbol{C} boldsymbol{O}_{3}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{H} boldsymbol{C} boldsymbol{O}_{3}^{-}+boldsymbol{H}_{3} boldsymbol{O}^{+} )
( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}_{1}}=mathbf{6 . 1 1} )
( boldsymbol{H} boldsymbol{C O}_{3}^{-}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{C} boldsymbol{O}_{3}^{2-}+boldsymbol{H}_{3} boldsymbol{O}^{+} )
( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}_{2}}=mathbf{1 0 . 2 5} )
In the ( H_{2} C O_{3}, H C O_{3}^{-} ) buffer system, we deal only with the first ionization
( operatorname{step}left(boldsymbol{K}_{a_{1}}right): boldsymbol{H}_{2} boldsymbol{C} boldsymbol{O}_{3} ) is a weak acid and
( H C O_{3}^{-} ) is the conjugate base (salt)
( C O_{2} ) enters the blood from tissues as
the by -product of a metabolic reaction.
In the lungs, ( C O_{2}(g) ) is exchanged for ( O_{2}(g), ) which is transported throughout the body by the blood.Important diagnostic analysis in the blood is :
A ( cdotleft[H_{2} P O_{4}^{-}right] /left[H P O_{4}^{-}right. )
в ( cdotleft[H C O_{3}^{-}right] /left[C O_{2}right] )
c. ( left[C O_{3}^{2-}right] /left[H C O_{3}^{2-}right] )
D cdot ( left[P O_{4}^{3-}right] /left[H P O_{4}^{2-}right] )

11
94Which of the following mixtures in aqueous solution acts as a buffer?
A. ( H N O_{3}+K N O_{3} )
в. ( H_{2} S O_{4}+K_{2} S O_{4} )
c. ( N H_{4} O H+N H_{4} C l )
D. ( C H_{3} ) СООН ( + ) NaCl
11
95Calculate the percent of hydrolysis in a ( mathbf{0 . 0 6} M ) solution of ( boldsymbol{K} boldsymbol{C} boldsymbol{N} )
Use ( :left[boldsymbol{K}_{a(boldsymbol{H} C N)}=boldsymbol{6} times mathbf{1 0}^{-mathbf{1 0}}right] )
A . ( 1.667 % )
B . ( 7.45 % )
c. ( 34.67 % )
D. None of these
11
96Q55. Calculate the hydrogen ion concentration in the following biological fluids whose pH are given
below:
(a) Human muscle-fluid, 6.83 (6) Human stomach fluid, 1.2
(c) Human blood, 7.38
(6) Human saliva, 6.4
11
97Assertion
On passing ( boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) ) through a
saturated solution of ( B a C l_{2}, ) a white
turbidity appears
Reason
The common ion effect is responsible for white turbidity
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
98Identify the correct statement(s) for the
given reaction.
( boldsymbol{H} boldsymbol{C l}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{H}_{3} boldsymbol{O}^{+}+boldsymbol{C l}^{-} )
a) Conjugate base of ( boldsymbol{H} boldsymbol{C l} ) is ( boldsymbol{C l}^{-} )
b) Conjugate acid-base pair is ( boldsymbol{H}_{3} boldsymbol{O}^{+} )
and ( boldsymbol{H}_{2} boldsymbol{O} )
c) Conjugate base of ( boldsymbol{H}_{2} boldsymbol{O} ) is ( boldsymbol{H}_{3} boldsymbol{O}^{+} )
d) Conjugate acid-base pair is ( boldsymbol{H} boldsymbol{C l} ) and
( boldsymbol{H}_{3} boldsymbol{O}^{+} )
( A cdot a ) and ( b ) are correct
B. a and c are correct
c. ( c ) and ( d ) are correct
D. a and d are correct
11
99A ( 0.1 ~ M ) aqueous solution of a weak
acid is ( 2 % ) ionized. If the ionic product
of water is ( 1 times 10^{-14}, ) the ( left[O H^{-}right] ) is:
A ( cdot 5 times 10^{-12} mathrm{M} )
В. ( 2 times 10^{-3} ) М
c. ( 1 times 0^{-14} mathrm{M} )
D. none of these
11
1000.43 Match the Column I with Column II.
RO
Column II
1. AG>0,
K1
Column
A. Equilibrium
B. Spontaneous reaction
C. Non-spontaneous reaction
2. AG=0
3. AGⓇ = 0
4. AG 1
11
101Question 27. If the solubility product of CuS is 6 *10-6, calculate the
maximum molarity of CuS in aqueous solution.
the Write the reaction for dissociation of Cus. Find the concentration
(molarity) according to it.
(See Chap. equilibrium of XI part 1)
11
102( 40 mathrm{mL} ) of ( 0.1 mathrm{M} ) ammonia solution is
mixed with ( 20 mathrm{mL} ) of ( 0.1 mathrm{M} ) HCl
What is the ( p H ) of the mixture?
A . 5.74
B. 9.26
c. 4.56
D. 7.06
11
103For making cake, baking powder is taken. If at home your mother uses baking soda instead of baking powder in cake, what is the role of tartaric acid
A. Make it more acidic
B. Make it more basic
c. Neutralise it
D. None of these
11
104The colour of bleaching powder is :
A. green
B. pale yellow
c. blue
D. white
11
105Calculate the ( p H ) of a ( 0.033 mathrm{M} )
ammonia solution, if ( 0.033 mathrm{M} N H_{4} C l ) is introduced in this solution at the same
temperature. ( left(k_{b} text { for } N H_{3}=1.77 timesright. )
( left.10^{-5}right) )
11
106What is pH formula?
A. ( -log _{e}left[H^{+}right] )
B. ( -log _{10}left[H^{-}right] )
c. ( -log _{10}left[O H^{-}right] )
D. ( -log _{10}left[H^{+}right] )
11
107The degree of dissociation of ( N_{2} O_{4} ) into
( N O_{2} ) at 1 atmosphere and ( 40^{circ} C ) is 0.25
Calculate its ( boldsymbol{K}_{boldsymbol{p}} ) at ( boldsymbol{4} boldsymbol{0}^{circ} boldsymbol{C} )
11
108( mathrm{NH}_{3}+mathrm{HCl} rightarrow )11
109Calculate the solubility of ( A g C N ) in a
buffer solution of ( boldsymbol{p} boldsymbol{H}=mathbf{3 . 0} )
( boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{C} boldsymbol{N})=mathbf{1 . 2} times )
( mathbf{1 0}^{-16}, boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{C N})=mathbf{4 . 8} times mathbf{1 0}^{-mathbf{1 0}} . ) There
is no ( C N^{-} ) or ( A g^{+} ) ion in the buffer
previously.
11
110The expression for equilibrium
constant, ( K_{c} ) for the following reaction
is :
( left.boldsymbol{F} boldsymbol{e}_{(}^{boldsymbol{3}+} boldsymbol{a} boldsymbol{q}right)+boldsymbol{3} boldsymbol{O} boldsymbol{H}_{(boldsymbol{a} boldsymbol{q})}^{-} rightleftharpoons boldsymbol{F} boldsymbol{e}(boldsymbol{O} boldsymbol{H})_{boldsymbol{3}(boldsymbol{s})} )
A ( cdot K_{c}=frac{left[F eleft(O H_{3}right)right]}{left[F e^{3+} mid D P Hright]^{5}} )
C . ( K_{c}=frac{1}{left[F e^{s+1}right]left(0 H^{-}right]^{s}} )
D. ( K_{c}=left[mathrm{Fe}left(mathrm{OH}_{3}right)right] )
11
1116. In a closed system
A(S) – 4 B(g) + 3 C(g)
If partial pressure of Cis doubled, then partial pressure of B will be
(@) 202 times the original value (b) times the original value
(©) 2 times of the original value
(d)
times of the original value
11
112The volume of the reaction vessel
containing an equilibrium mixture in the reaction is increased, when
equilibrium is re-established:
( boldsymbol{S} boldsymbol{O}_{2} boldsymbol{C l}_{2}(boldsymbol{g}) leftrightharpoons boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) )
A. the amount of ( S O_{2} ) will have decreased
B. the amount of ( S O_{2} C l_{2} ) will have increased
c. the amount of ( C l_{2} ) will have increased
D. the amount of ( C l_{2} ) will have remained unchanged
11
113Amphetamine ( left(C_{3} H_{13} Nright) ) is a weak
base with ( p K_{b} ) of ( 4.2 . ) Calculate the ( p H ) of a solution containing an amphetamine concentration of ( 220 m g / L )
A . 3.49
B. 5.21
c. 10.5
D. 13.7
11
114In a closed container rates of
evaporation and condensation are
same. What this statement indicate?
A. A general rule for predicting solubility
B. Conversion of solid phase to the liquid phase
C. It represents relationship between absolute temperature and the kinetic energy of particles
D. It represents relationship between volume and temperature at constant pressure
E. A state in which the liquid and gas phases are in equilibrium
11
115For water at ( 25^{circ} mathrm{C}, 2 times 10^{-7} ) moles per
litre is the correct answer for which one
of the following?
( mathbf{A} cdotleft[H^{+}right]+left[O H^{-}right] )
B . ( left[H^{+}right]^{2} )
c. ( left[O H^{-}right]^{2} )
( mathbf{D} cdotleft[H^{+}right]-left[O H^{-}right] )
11
116mole of gas ( A B ) dissociates to an
extent of ( 10 % ) at ( 127^{0} C ) according to
( A B rightleftharpoons A+B ) occupies a volume of
( 4 times 10^{4} ) ml. Find the total pressure at
this temp, assuming ideal gas behaviour.
11
117Which reaction below demonstrates the
lewis definition of acids and bases?
( mathbf{A} cdot H C l+N a O H rightarrow H O H+N a C l )
B. ( H_{2} O+N H_{3} rightarrow O H^{-}+N H_{4}^{+} )
( mathbf{C} cdot N H_{3}+B F_{3} rightarrow N H_{3} B F_{3} )
D. ( H I+K O H rightarrow H_{2} O+K I )
E ( cdot H^{+} O H^{-} rightarrow H_{2} O )
11
118Calculate pH of a solution whose ( 100 mathrm{m} )
contains ( 0.2 mathrm{g} ) NaOH dissolved in it?
A . 10.699
в. 11.699
c. 12.699
D. 13.699
11
119The pH of pure water at ( 25^{circ} mathrm{C} ) is close to:
( A cdot O )
B. 7
( c cdot 2 )
D. 9
11
120The ionic product of a saturated solution is ( _{-}-_{-}-_{-} ) the solubility product constant of its solute.
A. lesser than
B. greater than
c. equal to
D. not related to
11
121Acid buffer can be prepared by mixing solutions of:
A ( . quad N a C l+N a O H )
в. ( H_{2} S O_{4}+N a_{2} S O_{4} )
c. ( N H_{4} O H+N H_{4} C l )
D. ( C H_{3} C O O N a+C H_{3} C O O H )
11
122The pH of an aqueous solution of
( boldsymbol{C H}_{3} boldsymbol{C O O N} boldsymbol{a} ) of concentration ( boldsymbol{C}(boldsymbol{M}) ) if
given by
A ( cdot quad 7-frac{1}{2} p K_{a}-frac{1}{2} log C )
B. ( frac{1}{2}^{p K_{w}}+frac{1}{2} p K_{b}+frac{1}{2} log C )
( ^{mathrm{c}} cdot frac{1}{2}^{p} K_{w}-frac{1}{2} p K_{b}-frac{1}{2} log C )
( ^{mathrm{D} cdot frac{1}{2} p K_{w}+frac{1}{2} p K_{a}+frac{1}{2} log C} )
11
123Give chemical name, formula, and uses
of Washing soda.
11
124State True or False.
According to Bronsted-Lowry theory, neutralization reaction is the formation
of a conjugate acid base pair.
A. True
B. False
11
125Assertion
The value of equilibrium constant depends on the stoichiometry of the equation. BECAUSE
Reason
The value of equilibrium constant does not change when the equation is multiplied or divided by a number.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
126The solubility of ( N a C l ) in water is ( 38 g )
in ( 100 m L ) at ( 50^{circ} C )
I. If ( 50 g ) of salt is added to water, a
dynamic equilibrium will be reached. II. A dissociation equilibrium will
result in ( 50 % ) of the solute being in the aqueous state and ( 50 % ) being in the
solid state.
A. Statement ( I ) is true, Statement ( I I ) is true
B. Statement I is true, Statement II is false
c. statement ( I ) is false, statement ( I I ) is true
D. Statement I is false, Statement II is false
11
127In which of the following reaction, the
value of ( boldsymbol{K}_{boldsymbol{p}} ) will be equal to ( boldsymbol{K}_{c} ) ?
A ( cdot H_{2}+I_{2} rightleftharpoons 2 H I )
в. ( P C l_{5} rightleftharpoons P C l_{3}+C l_{2} )
( mathrm{c} cdot 2 N H_{3} rightleftharpoons N_{2}+3 H_{2} )
D. ( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3} )
11
128The bleaching action of bleaching
powder is due to:
A . oxidation
B. reduction
c. both A and B
D. none of these
11
129For the reaction ( 2 A rightarrow B+3 C ); if
( -frac{boldsymbol{d}[boldsymbol{A}]}{boldsymbol{d} t}=boldsymbol{k}_{1}[boldsymbol{A}]^{2} ; frac{boldsymbol{d}[boldsymbol{B}]}{boldsymbol{d} t}= )
( boldsymbol{k}_{2}[boldsymbol{A}]^{2} ; frac{boldsymbol{d}[boldsymbol{C}]}{boldsymbol{d} boldsymbol{t}}=boldsymbol{k}_{3}[boldsymbol{A}]^{2} ) the correct
relation between ( k_{1}, k_{2} ) and ( k_{2} ) is:
A ( cdot k_{1}=k_{2}=k_{2} )
B. ( 2 k_{1}=k_{2}=3 k_{2} )
( mathbf{c} cdot 4 k_{1}=k_{2}=3 k_{2} )
D. ( frac{k_{1}}{2}=k_{2}=frac{k_{3}}{3} )
11
130The main product obtained when a solution of sodium carbonate reacts
with mercuric chloride is :
( mathbf{A} cdot H g(O H)_{2} )
в. ( H g C O_{3} . H g O )
( mathrm{c} . mathrm{Hg} mathrm{CO}_{3} )
D. ( H g C O_{3} . H g(O H)_{2} )
11
131The molecular formula of acetic acid is
A. ( H C O O H )
в. ( C H_{3}-C H_{3} )
( mathbf{c} cdot C_{6} H_{6} )
D. ( C_{2} H_{4} O 2 )
11
132pH of ( 1 mathrm{M} ) HA (weak acid) is 2 . Hence,
vant Hoff factor is
A . 1.2
B. 1.02
c. ( 1 . )
D. 1.01
11
133( O H^{-} ) lon concentration in a acidic
buffer solution is:
( ^{text {A } cdot} frac{K w[A]}{K a[S]} )
в. ( frac{K a[A]}{K w[S]} )
c. ( frac{K w[S]}{K a[A]} )
D. ( frac{K a[S]}{K w[A]} )
11
134A solution is made of ( 0.1 ~ M C l^{-} ) and
( mathbf{1 0}^{-4} mathbf{M} mathbf{C r} mathbf{O}_{mathbf{4}}^{mathbf{2 -}} . ) If solid ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) is
then what will be the concentration of
( C l^{-} ) when ( A g_{2} C r O_{4} ) begins to
precipitate? ( left[boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{C l})=right. )
( mathbf{1 0}^{-mathbf{1 0}} boldsymbol{M}^{mathbf{2}} ; boldsymbol{K}_{boldsymbol{s p}}left(boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4}right)= )
( left.mathbf{1 0}^{-mathbf{1 2}} mathbf{M}^{mathbf{3}}right] )
В. ( 10^{-4} ) М
( mathbf{c} cdot 10^{-5} M )
D. ( 10^{-9} M )
11
135( left[B a^{2+}right] ) when ( C a S O_{4} ) starts just precipitation will be:
( mathbf{A} cdotleft[B a^{2+}right]=4.58 times 10^{-7} M )
B . ( left[B a^{2+}right]=5.58 times 10^{-7} M )
C ( cdotleft[B a^{2+}right]=4.85 times 10^{-7} M )
D. None of these
11
136( 28 g ) of ( N_{2} ) and ( 6 g ) of ( H_{2} ) were kept at
( 400^{circ} mathrm{C} ) in 1 litre vessel, the equilibrium
mixture contained ( 27.54 g ) of ( N H_{3} . ) The
appropriate value of ( boldsymbol{K}_{c} ) for the above reaction can be (in mole( ^{-2} ) litre( ^{2} ) )
( mathbf{A} cdot 75 )
B. 50
c. 25
D. 100
11
137Neutral litmus solution have
A. no effect of acidic solution
B. no effect of alkaline solution
C. both ( A ) and ( B )
D. none of these
11
138The two equilibrium ( boldsymbol{A B} leftrightharpoons boldsymbol{A}^{+}+boldsymbol{B}^{-} )
and ( A B+B^{-} leftrightharpoons A B_{2}^{-} ) are
simultaneously maintained in a
solution with equilibrium constant ( boldsymbol{K}_{mathbf{1}} )
and ( K_{2} ) respectively. The ratio of ( left[A^{+}right] ) to
( left[A B_{2}^{-}right] ) in the solution is:
A. directly proportional to the concentration of ( B )
B . inversely proportional to the concentration of ( B )
c. directly proportional to the square of the concentration of ( B )
D. inversely proportional to the square of the concentration of ( B )
11
139When chlorine is passed over dry slaked
lime at room temperature, the main reaction product is:
A ( cdot C aleft(C l O_{2}right)_{2} )
в. ( C a C l_{2} )
c. ( C a O C l )
D. ( operatorname{Ca}left(O C l_{2}right)_{2} )
11
140Q28. Hydrogen gas is obtained from the natural gas by partial oxidation with steam as per following
endothermic reaction:
| CH, (g) + H20g) + COg) + 3H, (g)
Write the expression for K, for the above reaction
How will the value of K, and composition of equilibrium mixture be affected by:
(i) increasing the pressure. (ii) increasing the temperature, (iii) using a catalyst?
11
141Backward reaction is favoured by
increase in the pressure of which of the following equilibrium?
A ( cdot 2 S O_{2}+O_{2} leftrightharpoons 2 S O_{3} )
в. ( N_{2}+O_{2} leftrightharpoons 2 N O )
c. ( N_{2}+3 H_{2} leftrightharpoons 2 N H_{3} )
D. ( P C l_{5} leftrightharpoons P C l_{3}+C l )
11
142The precipitate of
( boldsymbol{C a} boldsymbol{F}_{2}left(boldsymbol{K}_{s p}=1.7 times 10^{-10}right) ) is obtained
when equal volumes of the following are ( operatorname{mixed} )
( begin{array}{lll}text { A. } 10^{-4} M & C a^{2-}+10^{-4} M & F^{-}end{array} )
( begin{array}{lll}text { В. } 10^{-2} M & C a^{2-}+10^{-3} M & F^{-} \ & end{array} )
11
1431. The equilibrium expression, K = [CO] represents the reaction.
(a) C(s) + O2(8) = CO2(8)
(b) CaCO3(s) = Cao(s) + CO2(8)
(C) CO(g) + 026) = 00,(8) (a) CaC(s) + CO2(g) = CaCO3(6)
11
144( H_{2} O_{2} ) is decomposed to ( H_{2} O ) and ( O, ) in
the following sequence of reactions:
( mathbf{I} boldsymbol{H}_{2} boldsymbol{O}_{2(boldsymbol{a q})}+boldsymbol{I}_{(boldsymbol{a} q)}^{-} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(l)}+boldsymbol{I} boldsymbol{O}_{(boldsymbol{a} boldsymbol{q})}^{-} )
ii) ( boldsymbol{H}_{2} boldsymbol{O}_{2(a q)}+boldsymbol{I}_{(a q)}^{-} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(l)}+ )
( boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{I} boldsymbol{O}_{(boldsymbol{a} boldsymbol{q})}^{-} )
(a) Write the chemical equation for the overall reaction.
(b) Identify the species that acts as a
catalyst.
(c) Identify the intermediate.
11
145Assertion
An aqueous solution of ammonium
acetate can act as a buffer.
Reason
Acetic acid is a weak acid and
( N H_{4} O H ) is a weak base.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
146The ( K_{s p} ) for ( A g C l ) is ( 2.8 times 10^{-10} ) at a
given temperature. The solubility of ( A g C l ) in 0.01 molar ( H C l ) solution at
this temperature will be:
A. ( 2.8 times 10^{-12} ) mol ( L^{-1} )

B . ( 2.8 times 10^{-8} mathrm{mol} mathrm{L}^{-1} )
c. ( 5.6 times 10^{-8} ) mol ( L^{-1} )
D. 2.8 ( times 10^{-4} mathrm{mol} mathrm{L}^{-1} )
11
147Which one of the following solutions will have the highest pH value?
A. ( 0.01 M ) NaOH
в. ( 0.02 M ) СН( _{3} ) СОО Na .
c. ( 0.01 M ) NaHCO( _{3} )
D. ( 0.01 M H_{2} S O_{4} )
11
148The van’t Hoff factor (i) for a dilute
aqueous solution of the strong electrolyte barium hydroxide is :
( A cdot 2 )
B. 3
( c cdot 0 )
D.
11
149The pH of an ( H C l ) solution is 2
Sufficient water is added to make the pH of new solutions. The hydrogen ion concentration is reduced:
A. ten fold
B. seven fold
c. thousand fold
D. hundred fold
11
150Which of the following expressions is
correct?
( boldsymbol{A} cdot ldots_{p}=K_{c}left(frac{R T}{sum n}right)^{Delta n} )
( mathrm{B} cdot quad K_{p}=K_{x}left(frac{P}{sum n}right)^{Delta n} )
( mathrm{C} cdot_{p}=K_{n}left(frac{P}{sum n}right)^{Delta n-1} )
( mathrm{D} cdot_{p}=K_{c}left(frac{P}{sum n}right)^{-Delta n+1} )
11
151Which one of the following statements
is not correct?
A. The pH of ( 1.0 times 10^{-8} mathrm{M} mathrm{HCl} ) is less than 7
B. The ionic product of water at ( 25^{0} C ) is ( 1.0 times ) ( 10^{-14} mathrm{mol}^{2} L^{-2} )
C ( cdot C l^{-} ) is a Lewis acid
D. Bronsted-Lowry theory cannot explain the acidic character of ( A l C l_{3} )
11
152If ( K_{p} ) for a reaction is ( frac{1}{9} times 10^{-2} a t m^{-2} ) at
500K. Magnitude of ( K_{c} ) will be [Take ( R= ) 0.08]
A. ( 3 times 10^{-1} )
В . ( frac{1}{9} times 10^{-2} )
( c cdot frac{16}{9} )
D. Data insufficient
11
153In manufacture of sodium carbonate
from Solvay (or ammonia soda) process
the raw material used is:
A . ( N a O H )
в. ( N a_{2} S O_{4} )
c. ( N a C l )
D. ( operatorname{NaH} mathrm{CO}_{3} )
11
154Q58. The solubility of Sr (OH), at 298 K is 19.239/L of solution. Calculate the concentrations of
strontium and hydroxyl ions and the pH of the solution. (Atomic mass of Sr = 87.6)
6
Chemistry. YI
11
155Assertion
The melting point of ice decreases with
increase of pressure.
Reason
Ice contracts on melting.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is
not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
15643. The degree of dissociation of an
electrolyte depends on
(1) dilution
(2) impurities
(3) atmospheric pressure
(4) method of dissolution
11
157Consider the following salts:
( N a C l, H g C l_{2}, H g_{2} C l_{2}, C u C l_{2}, C u C l )
and ( A g C l ). Identify the correct set of insoluble salts in water.
A. ( H g_{2} C l_{2}, C u C l, A g C l )
в. ( H g C l_{2}, C u C l, A g C l )
c. ( H g_{2} C l_{2}, C u C l_{2}, A g C l )
D. ( H g_{2} C l_{2}, C u C l, N a C l )
11
158In a 20 litre vessel initially 1,1,1 mole
of ( C O, H_{2} O, C O_{2} ) are present, then for
the equilibrium of ( boldsymbol{C O}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons )
( C O_{2}+H_{2} . ) Which of the following is
true?
A. ( H_{2} ) more then 1 mole
B. ( C O, H_{2} O, H_{2} ) less then 1 mole
c. ( C O_{2} ) and ( H_{2} O ) both more than 1 mole
D. All of these
11
159In the hydrolytic equilibrium;
( boldsymbol{B}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{B} boldsymbol{O} boldsymbol{H}+boldsymbol{H}^{+} )
( K_{b}=1 times 10^{-5} . ) The hydrolysis constant
is:
A ( cdot 10^{-5} )
( ^{5} )
B . ( 10^{-19} )
c. ( 10^{-10} )
D. ( 10^{-9} )
11
160Consider the following solubility data
for various chromates at ( 25^{circ} mathrm{C} )
[
begin{array}{cc}
boldsymbol{K}_{boldsymbol{s} boldsymbol{p}} \
boldsymbol{A} boldsymbol{g}_{boldsymbol{2}} boldsymbol{C r} boldsymbol{O}_{boldsymbol{4}} & boldsymbol{9 . 0} times mathbf{1 0}^{-mathbf{1 2}} \
boldsymbol{B a C r} boldsymbol{O}_{boldsymbol{4}} & boldsymbol{2 . 0} times mathbf{1 0}^{-mathbf{1 0}} \
boldsymbol{P b C r O}_{boldsymbol{4}} & boldsymbol{1 . 8} times mathbf{1 0}^{-mathbf{1 4}}
end{array}
]
The chromate that is the most soluble
in water at ( 25^{circ} mathrm{C} ) on a molar basis is
( mathbf{A} cdot A g_{2} C r O_{4} )
B ( . ) BaCr ( mathrm{O}_{4} )
( mathbf{c} cdot P b C r O_{4} )
D. impossible to determine
E. none of these
11
161In the reaction, ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C}, ) if ( mathbf{2} )
moles of ( A, 3.0 ) moles of ( B ) and 2.0 moles of ( C ) are placed in a ( 2 L ) flask and the
equilibrium concentration of ( mathrm{C} ) is 0.5 mol ( / L . ) The equilibrium constant
( left(K_{c}right) ) for the reaction is:
( mathbf{A} cdot 0.073 )
B. 0.1470
c. 0.0500
D. 0.0080
11
162For reactions involving gaseous reactants and products, the
equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) is written
in terms of:
A. the pressure of the gases
B. the molar volumes of the gases
c. the partial pressures of the gases
D. the mole fraction of the gases
11
163Two flasks ( A ) and ( B ) of an equal volume
containing 1 mole and 2 moles of ( 0_{3} )
respectively are heated to the same
temperature. When the reaction ( 2 O_{3} rightleftharpoons )
( 30_{2} ) practically stops, then both the
A ( . ) the same ratio: ( left[O_{2}right] /left[O_{3}right] )
B. the same ratio: ( left[O_{2}right]^{3 / 2} /left[O_{3}right] )
c. only ( O_{2} )
D. the same time to reach equilibrium
11
164If first dissociation of ( boldsymbol{X}(boldsymbol{O} boldsymbol{H})_{3} ) is ( mathbf{1 0 0 %} )
whereas second dissociation is ( 50 % )
and third dissociation is negligible then the ( p H ) of ( 4 times 10^{-3} M X(O H)_{3} ) is :
A. 11.78
B. 10.78
c. 2.5
D. 2.22
11
165If the equilibrium constant of the reaction of weak acid ( boldsymbol{H} boldsymbol{A} ) with a strong
base is ( 10^{9} ), then the ( p H ) of ( 0.1 M N a A )
solution will be:
11
166The solubility of ( A g C l ) is ( 1 times )
( 10^{-5} ) mol ( / L . ) Its solubility in 0.1 molar
sodium chloride solution is:
A ( cdot 1 times 10^{-10} )
В. ( 1 times 10^{-5} )
c. ( 1 times 10^{-9} )
D. ( 1 times 10^{-4} )
11
167The equilibrium constant for the reaction
( boldsymbol{C H}_{3} boldsymbol{C O O H}(boldsymbol{a q})+boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{O H}(boldsymbol{a q}) Leftrightarrow )
( boldsymbol{C H}_{3} boldsymbol{C O O C}_{2} boldsymbol{H}_{5}(boldsymbol{a q})+boldsymbol{H}_{2} boldsymbol{O}(l) ) is 16
The initial concentration of each of
( C H_{3} C O O H ) and ( C_{2} H_{5} O H ) is two (mole/lit). What is the concentration of
( C H_{3} C O O C_{2} H_{5} ) at equilibrium in moles / lit?
A. 0.9
B. 0.6
( c cdot 1.6 )
D. 0.7
11
168Q. 10 Acidity of BF, can be explained on the basis of which of the following
concepts?
(a) Arrhenius concept
a
(a) Arrhenius concept
n d Us OTTO
(b) Bronsted Lowry concept
(c) Lewis concept
(d) Bronsted Lowry as well as Lewis concept o n to prison
11
169The reaction quotient ( (Q) ) at
equilibrium is:
( A cdot=1 )
в. ( =K )
( c cdot>K )
( mathrm{D} cdot<K )
11
170Which of the following properties of a solution of ( N a C l ) will not vary as the concentration of salt is increased?
A ( . p H )
B. Density
c. Refractive index
D. Electrical conductivity
11
171Ammonium hydrogen sulphide dissociates as follows
( N H_{4} H S(s) rightleftharpoons N H_{3}(g)+H_{2} S(g) )
If solid ( N H_{4} H S ) is placed in an evacuated flask at certain temperature it will dissociate until the total pressure
is 600 torr.
a) Calculate the value of equillibrium constant for the dissociation reaction
b) Addional ( N H_{3} ) is introduced into the equillibrium mixture without changing the temperature until partial pressure
of ( N H_{3} ) is 750 torr, what is the partial
pressure of ( boldsymbol{H}_{2} boldsymbol{S} ) under these conditions? What is the total pressure in the flask?
11
172For the reaction, ( boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}) rightarrow )
( C(g)+D(g) )
( Delta H^{0} ) and ( Delta S^{0} ) are,respectively ( -29.8 k J m o l^{-1} ) and ( -0.100 k J K^{-1} )
( operatorname{mol}-1 ) at ( 298 mathrm{K} )
The equilibrium constant for the
reaction at ( 298 K ) is :
11
173Consider the following gas phase
reaction:
( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{B r}_{2}(boldsymbol{g}) rightleftharpoons 2 boldsymbol{H} boldsymbol{B} boldsymbol{r}(boldsymbol{g}) )
The concentrations of ( boldsymbol{H}_{2}, boldsymbol{B} boldsymbol{r}_{2}, ) and
HBr are ( 0.05 M, 0.03 M, ) and ( 500.0 M )
respectively. The concentration equilibrium constant for this reaction
( operatorname{at} 400^{circ} mathrm{C} ) is ( 2.5 times 10^{3} . ) Is this system at
equilibrium?
A. Yes, the system is at equilibrium.
B. No, the reaction must shift to the right in order to reach equilibrium.
c. No, the reaction must shift to the left in order to reach equilibrium.
D. It cannot be determined
11
174What is ( left[boldsymbol{H}^{+}right] ) in mol/L of a solution that
is ( 0.20 mathrm{M} ) in ( C H_{3} C O O N a ) and ( 0.10 mathrm{M} ) in
( boldsymbol{C H}_{3} boldsymbol{C O O H} ? )
( boldsymbol{K}_{a} ) for ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}} )
A ( .3 .5 times 10^{-4} )
В. ( 1.1 times 10^{-5} )
c. ( 1.8 times 10^{-5} )
D. ( 9.0 times 10^{-6} )
11
175Assertion
( N H_{3} ) is a Lewis base.
Reason
Ammonia can accept a proton.
A. Both Assertion and Reason are correct and the Reason is the correct explanation of the Assertion
B. Both Assertion and Reason are correct but the Reason
is not the correct explanation of the Assertion
C. The Assertion is correct but the Reason is incorrect
D. The Assertion is incorrect and the Reason is correct
11
176For the reaction, ( boldsymbol{C O}_{(boldsymbol{g})}+boldsymbol{C l}_{2(boldsymbol{g})} rightleftharpoons )
( C O C l_{2(g)}, ) the value of ( K_{p} / K_{c} ) is equal
to?
A . 1.0
в. RT
c. ( sqrt{R T} )
D. ( frac{1}{R T} )
11
177Calculate the ( p H ) after the addition of
( 90 m l ) and ( 100 m l ) respectively of
( mathbf{0 . 1} N ) NaOH to
( 100 m l 0.1 N C H_{3} C O O H )
(Given ( left.p K_{a} text { for } C H_{3} C O O H=4.74right) )
11
178A mixture of three gases P (density
0.90)( , Q(text { density } 0.178) ) and ( R( ) density
0.42) is enclosed in a vessel at the
constant temperature. When the equilibrium is established:
A. the gas P will be at the top of the vessel
B. the gas Q will be at the top of the vessel
c. the gas ( R ) will be at the top of the vessel
D. the gases will mix homogeneously throughout the vessel
11
179The pH of a tomato juice is:
A .
B. 4
( c cdot 7 )
D. 14
11
180If the ( K_{b} ) value in the hydrolysis
reaction, ( boldsymbol{B}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{B O H}+boldsymbol{H}^{+} ) is
( 1.0 times 10^{-6}, ) then the hydrolysis constant
of the salt would be:
A ( .1 .0 times 10^{-6} )
В. ( 1.0 times 10^{-7} )
c. ( 1.0 times 10^{-8} )
D . ( 1.0 times 10^{-9} )
11
181Equilibrium constant for an equilibrium reaction is ( 100 . ) Its forward reaction rate constant ( boldsymbol{K}_{boldsymbol{f}}=mathbf{1 0}^{mathbf{5}} . ) Its
backward reaction rate constant ( boldsymbol{K}_{boldsymbol{b}} ) is;
A ( cdot 10^{2} )
B. 10
( c cdot 10^{4} )
D. ( 10^{3} )
11
182( M Y ) and ( N Y_{3}, ) two nearly insoluble
salts, have the same ( boldsymbol{K}_{s p} ) values of
( 6.2 times 10^{-13} ) at room temperature
Which statement would be true in
regards to ( M Y ) and ( N Y_{3} ? )
A. The molar solubilities of ( M Y ) and ( N Y_{3} ) in water are identical.
B. The molar solubility of ( M Y ) in water is less than that of ( N Y_{3} )
C. The salts ( M Y ) and ( N Y_{3} ) are more soluble in ( 0.5 M K Y ) than in pure water.
D. The addition of the salt of KY to solution of ( M Y ) and
( N Y_{3} ) will have no effect on their solubilities
11
183A strong electrolyte in aqueous solution exhibit:
This question has multiple correct options
A. almost completely dissociated
B. hydration
c. partial dissociation
D. none of the above
11
184Carbonic acid generally displaces another acid when the acid is heated
with a salt.
A. True
B. False
11
185( K_{a} ) for acetic acid in water is ( 1.7 times )
( 10^{-5} ) at ( 25^{circ} mathrm{C} . ) The ( mathrm{pH} ) of a mixture of 25
( mathrm{ml} ) of ( 0.02 mathrm{N} ) acetic acid and ( 2.5 mathrm{ml} ) of
0.1N NaOH (neglecting volume change) will be ( (log 1.7=0.23) )
A . 2.
B. 4.8
( c .7 .5 )
D. 1.0.
11
186In general, as the temperature increases, the solubility of gases in water ( _{text {十一一一一一一一一一 }} ) and the solubility of most solids in water
A. decreases, decreases
B. decreases, increases
c. increases, decreases
D. increases, increases
11
187Write the application of sodium
bicarbonate (baking soda)?
11
188What is the ( K_{c} ) for the reaction:
( boldsymbol{M} boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2(s)}+boldsymbol{2} boldsymbol{N} boldsymbol{H}_{4(a q)}^{+} rightleftharpoons )
( mathbf{2} boldsymbol{N} boldsymbol{H}_{3(boldsymbol{g})}+mathbf{2 H}_{mathbf{2}} boldsymbol{O}_{(boldsymbol{a q})}+boldsymbol{M} boldsymbol{g}_{(boldsymbol{a q})}^{mathbf{2 +}} )
(Given that the solubility product for ( M g(O H)_{2}, K_{s p} ) is ( 6 times 10^{-12} ) mol ( ^{3} L^{-3} )
and
the base dissociation constant for
( N H_{4} O H, K_{b} ) is ( 1.8 times 10^{-5} m o l L^{-1} )
A ( cdot 2.05 times 10^{-2} )
В. ( 1.65 times 10^{-2} )
c. ( 1.85 times 10^{-2} )
D. None of these
11
189The total number of basic groups in the following form of lysine is:
( A )
B.
( c cdot 2 )
( D )
( E cdot 4 )
( F .5 )
( G cdot 6 )
H.
8
11
190Predict which of the following reaction will have appreciable concentration of reactants and products:
a) ( C l_{2}(g) rightleftharpoons 2 C l(g) ; K_{c}=5 times 10^{-39} )
b) ( C l_{2}(g)+2 N O(g) rightleftharpoons )
( mathbf{2} boldsymbol{N} boldsymbol{O} boldsymbol{C l}(boldsymbol{g}) ; boldsymbol{K}_{c}=mathbf{3 . 7} times mathbf{1 0}^{mathbf{8}} )
c) ( C l_{2}(g)+2 N O_{2}(g) rightleftharpoons )
( mathbf{2} boldsymbol{N} boldsymbol{O}_{2} boldsymbol{C l}(boldsymbol{g}) ; boldsymbol{K}_{c}=mathbf{1 . 8} )
11
191Which of the following will occur if a 1.0 M solution of a weak acid is diluted to
( 0.01 mathrm{M} ) at constant temperature:
A. Percentage ionisation will increase
B. [H+] will decrease to 0.01 M
c. ( K_{a} ) will increase
D. pH will decrease by 2 units
11
192The state of equilibrium refers to:
A. State of rest
B. Dynamic state
c. Stationary state
D. State of inertness
11
193In aqueous solution, the following mixture acts as buffer:
A. ( H N O_{3}+K N O_{3} )
в. ( H_{2} S O_{4}+K_{2} S O_{4} )
c. ( N H_{4} O H+N H_{4} C l )
D. ( C H_{3} C O O H+N a C l )
11
194An equilibrium mixture for the reaction
( mathbf{2} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{S}_{2}(boldsymbol{g}) ) has
1 mole of ( H_{2} S, 0.2 ) mole of ( H_{2} ) and
0.8 mole of ( S_{2} ) in a 2 litre flask. The
value of ( boldsymbol{K}_{c} ) in mol ( boldsymbol{L}^{-1} ) is
( mathbf{A} cdot 0.004 )
B. 0.08
c. 0.016
D. 0.160
11
195Calculate the amount of ammonium
chloride required to dissolve in ( 500 m L )
water to have ( boldsymbol{p} boldsymbol{H}=mathbf{4 . 5}left(boldsymbol{K}_{boldsymbol{b}} ) for right.
( left.N H_{4} O H text { is } 1.8 times 10^{-5}right) )
11
196Which of the following solutions will be acidic?
(1) ( 0.1 M F e S O_{4} )
(2) ( 0.1 Mleft(N H_{4}right)_{2} S O_{4} )
(3) ( 0.1 M C H_{3} C O O N a )
(4) ( 0.1 M N H_{4} O H )
A ( cdot 1,2 ) and 3 are correct
B. 1 and 2 are correct
( c cdot 2 ) and 4 are correct
D. 1 and 3 are correct
11
197The molar concentrations of ( A, B ) and ( C ) at equilibrium for the reaction ( boldsymbol{A}+ ) ( 2 B Leftrightarrow 3 C ) are 2,3 and 4 moles/lit
respectively. Its ( boldsymbol{K}_{c} ) is:
( A cdot 2 )
в. 3.56
( c cdot 0.2 )
D. 0.026
11
198A weak acid HA after treatment with 12
mL of 0.1 M strong base has a pH of ( 5 . ) At the end point, the volume of same base
required is ( 26.6 mathrm{mL} ). The value of ( K_{a} ) is:
A ( .8 .2 times 10^{-6} )
B . ( 6.4 times 10^{-6} )
( mathbf{c} cdot 5.3 times 10^{-5} )
D. ( 2.4 times 10^{-6} )
11
1991 mole of ( C H_{3} C O O H ) and 1 mole of
( C H_{3} C O O N a ) are dissolved in water to
form 1 litre aqueous solution. The pH of the resulting solution will be:
A . 9.2553
в. 4.7447
c. 14
D.
11
200The concentration of a solution is
( mathbf{1 0}^{-4} boldsymbol{M} ) for ( boldsymbol{C l}^{-}, mathbf{1 0}^{-mathbf{5}} boldsymbol{M} ) for ( boldsymbol{B r}^{-} ) and
( 10^{-3} mathrm{M} ) for ( I^{-} . A g N O_{3}(s) ) is added slowly to the solution. If the minimum
concentration of ( boldsymbol{A} boldsymbol{g}^{+} ) required to start
precipitation of all three ions is ( 10^{-x} )
then the value of ( x ) is
( left[text { Given, } boldsymbol{K}_{s p(A g C l)}=mathbf{1 0}^{-mathbf{1 0}}, boldsymbol{K}_{s p(A g B r)}=right. )
( left.mathbf{1 0}^{-mathbf{1 3}}, boldsymbol{K}_{boldsymbol{s p}(boldsymbol{A g I})}=mathbf{1 0}^{-mathbf{1 7}}right] )
11
201A vessel of 250 litre was filled with 0.01
mole of ( S b_{2} S_{3} ) and 0.01 mole of ( H_{2} ) to
attain the equilibrium at ( 440^{circ} mathrm{C} ) as :
[
begin{array}{r}
boldsymbol{S b}_{2} boldsymbol{S}_{3}(boldsymbol{s})+mathbf{3} boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{S} boldsymbol{b}(boldsymbol{s})+ \
mathbf{3} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})
end{array}
]
After equilibrium, the ( H_{2} S ) formed was analysed by dissolved it in water and treating with excess of ( P b^{2+} ) to give
1.19g of ( P b S ) as precipitate. What is the
value of ( boldsymbol{K}_{c} ) at ( mathbf{4 4 0}^{circ} boldsymbol{C} )
A .
B. 2
( c cdot 4 )
D.
11
202Arrange the following acids in increasing order of their acid strength:
I. ( boldsymbol{H} boldsymbol{C l O}_{mathbf{4}} )
II. ( quad H_{2} S O_{4} )
III ( . )
A. ( I I I<I I<I )
B. ( I<I I<I I I )
c. ( I I<I I I<I )
D. III ( <I<I I )
11
203The solubility ( A g C l ) is maximum in:
A. acidic buffer solution
B. basic buffer solution
c. In pure water
D. equal in all solutions
11
204If ( K_{a} ) is more (or) ( p k_{a} ) is less then more
stronger is the acid.
lonic order: ( boldsymbol{H} boldsymbol{C O O H}>boldsymbol{C}_{mathbf{6}} boldsymbol{H}_{mathbf{5}} boldsymbol{C O O H} )
11
205Anhydrous sodium carbonate is commonly known as:
A. baking soda
B. washing soda
c. chalk
D. paris white
11
206Which of the following salt undergoes
hydrolysis?
A. ( C H_{3} ) СООК
в. ( operatorname{NaNO}_{3} )
c. ( K C l )
D. ( K_{2} S O_{4} )
11
207At equilibrium,in solution a certain
( operatorname{acid}, boldsymbol{H} boldsymbol{A}, ) yields ( [boldsymbol{H} boldsymbol{A}]=mathbf{0 . 9 4} boldsymbol{M} ) and
( left[A^{-}right]=0.060 M . ) On the basis of the
above data given
(A) Calculate ( K_{a} )
(B) Is this acid stronger or weaker than
sulfurous acid ( left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1 . 7} times mathbf{1 0}^{-mathbf{2}}right) ? )
(C) Calculate ( K_{b} )
(D) Calculate pH
11
208The amount of ( left(N H_{4}right)_{2} S O_{4} ) having degree of dissocation ( 75 % ) which should
be dissolved in ( 1500 mathrm{ml} ) of ( 1 mathrm{M} N H_{4} mathrm{OH} )
to decrease its degree of dissociation
by 200 times, is ( left[k_{b} text { of } N H_{4} O H=1.8right. )
( left.times 10^{-5}right]: )
A . ( 112.1 mathrm{gm} )
B. 224.2 gm
c. ( 56.0 mathrm{gm} )
D. 65.4gm
11
209A two litre vessel contains 0.48 mole of
( C O_{2}, 0.48 ) mole of ( H_{2}, 0.96 ) mole of ( C O ) at equilibrium
[
boldsymbol{C O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})+
]
( boldsymbol{C O}(boldsymbol{g}) )
How many ( g m ) (only integer part) of ( boldsymbol{H}_{2} ) must be added to bring the concentration of ( C O ) to ( 0.6 M ? )
11
210At a particular temperature and atmospheric pressure, the solid and
liquid phases of a pure substance can exist in equilibrium. Which of the
following term defines this temperature?
(a) Normal melting point
(b) Equilibrium temperature
(c) Boiling point
(d) Freezing point
11
211Predict if there will be any precipitate by mixing ( 50 mathrm{mL} ) of ( 0.01 mathrm{M} ) NaCl and 50
mL of ( 0.01 mathrm{M} A g N O_{3} ) solution. The
solubility product of ( A g C l ) is ( 1.5 times )
( 10^{-10} )
A. since ionic product is greater than solubility product no precipitate will be formed
B. since ionic product is lesser than solubility product. precipitation will occur
c. since ionic product is greater than solubility product. precipitation will occur.
D. since ionic product and solubility product are same, precipitation will not occur
11
212The ionisation of strong electrolytes in acetic acid compared to that in water is
A. weak
B. Strong
c. Medium
D. No ionisation
11
213A weak acid ( boldsymbol{H} boldsymbol{X}left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1} times mathbf{1 0}^{-mathbf{5}}right) ) on
reaction with NaOH gives NaX. For ( 0.1 mathrm{M} ) aqueous solution of NaX, the % hydrolysis is:
A . 0.001%
B . 0.01%
c. ( 0.15 % )
D. 1%
11
214A sulphate salt of group 2 element of the periodic table is a white, soft substance, which can be moulded into
different shapes by making its dough.
When this compound is left in open for some time, it becomes a solid mass and cannot be used for
moulding purposes. Identify the sulphate salt.
A. White paris
B. Plaster of paris
c. Calcium hydroxide
D. Calcium carbonate
11
215Initially the reactions in the containers a and b are at equilibrium when the products and reactants are put together in a container ( c ) than at the equilibrium the total number of different chemical
compounds are?
A. 5
B. 7
( c cdot 6 )
( D )
11
216Predict the direction of the reaction
from the comparison of ( Q_{c}, K_{c} . ) Mark the
incorrect statement.
A ( cdot ) If ( Q_{c}K_{c} ), net reaction goes from right to left
D. If ( Q_{c}=K_{c} ), reactants and products are at equilibrium.
11
217( P C l_{5} ) dissociates according to the
reaction ( boldsymbol{P} boldsymbol{C l}_{5} rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) cdot mathbf{A t} )
( mathbf{5} mathbf{2 3} boldsymbol{K}, boldsymbol{K}_{boldsymbol{p}}=mathbf{1 . 7 8} boldsymbol{a t m} . ) Find the
density of the equilibrium mixture at a total pressure of 1 atm.
A. 2.96 g/ml
B. 4.51 ( g / m ) ।
c. 6.73 g/ml
D. 3.44 g/ml
11
218At ( 80^{circ} C, ) distilled water has hydronium
( operatorname{ion}left(H_{3} O^{+}right) ) concentration equal to ( 1 times )
( 10^{-6} ) mol ( / l . ) The value of ( K_{w} ) at this
temperature would be:
A ( cdot 1 times 10^{-6} )
В. ( 1 times 10^{-12} )
c. ( 1 times 10^{-9} )
D. ( 1 times 10^{-14} )
11
219Addition of ( H C l ) will not suppress the ionization of:
A . acetic acid
B. benzoic acid
( mathrm{c} cdot mathrm{H}_{2} )
D. sulphuric acid
11
220For a reversible equilibrium reaction
( K_{C}>K_{P} ) at ( 298 K ) and ( Delta H=+200 )
( K J, ) the forward reaction is favoured if:
(i) Pressure is increased
(ii) Temperature is increased
(iii) Temperature is decreased
(iv) Increasing the concnetration of reactants
A . i, i i, iv
B. i, ii
c. ii, iv
D. i, iii, iv
11
221The equilibrium constant ( K_{C} ) for the reaction,
( A(g)+2 B(g) rightleftharpoons 3 C(g) ) is ( 2 times 10^{-3} )
What would be the equilibrium partial
pressure of gas ( C ) if initial pressure of ( operatorname{gas} A ) and ( B ) are 1 and 2
11
222The equilibrium concentration of ( C_{2} H_{4} )
in the following gas phase reaction can be increased by:
( boldsymbol{C}_{2} boldsymbol{H}_{4}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons )
( boldsymbol{C}_{2} boldsymbol{H}_{6}(boldsymbol{g}), quad boldsymbol{Delta} boldsymbol{H}=-mathbf{3 2 . 7} boldsymbol{k} boldsymbol{c a l} )
A ( cdot ) removal of ( C_{2} H_{6} )
B. removing ( H_{2} )
c. decrease in temperature
D. increase in pressure
11
223Which are general property of Bronsted
acids?
This question has multiple correct options
A. They turn litmus red
B. They react with alkalies
c. They burn the skin
D. They contain ( H ) -atom replaceable with metal
11
224One litre solution contains ( 1 M ) HOCl
( left[boldsymbol{K}_{a}=mathbf{1 0}^{-8}right] ) and ( 1 M ) NaOH.What is
the ( p H ) of the solution?
A. 8
B. 1
( c cdot 5 )
D. 2
11
225The ( p K_{a} ) of acetic acid and ( p K_{b} ) of
( N H_{4} O H ) are 4.76 and ( 4.75 . ) Calculate
the ( p H ) of ammonium acetate ions.
11
226About buffer solution which is correct?
This question has multiple correct options
A. It contains a weak acid and its conjugate base
B. It contains a weak base and its conjugate acid
C. It shows change in ( mathrm{pH} ) on adding small amount of acid or base
D. All of the above
11
227At ( 800 mathrm{K} ) a reaction mixture contained
0.5 mole of ( S O_{2} .0 .12 ) mole of ( O_{2} ) and 5
mole of ( S O_{3} ) at equilibrium. ( K_{c} ) for the
equilibrium ( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3} ) is 833
lit/ mole. If the voiume of the container
is 1 litre, calculate how much ( O_{2} ) is to be added at this equilibrium in order to get
5.2 moles of ( S O_{3} ) at the same temperature.
A. 2.34 mole
B. 0.34 mole
c. 1.43 mole
D. 3.23 mole
11
228On the addition of a solution containing ( C r O_{4}^{2-} ) ions to the solution of ( B a^{2+}, S r^{2+}, C a^{2+} ) ions, the precipitate
obtained first will be of:
A. ( C a C r O_{4} )
B ( . ) SrCrO ( _{4} )
( mathrm{c} cdot B a C r O_{4} )
D. A mixture of all the three
11
229Which of the following reactions proceed in forward direction with an
increase in temperature?
( mathbf{A} cdot H_{2}(g)+I_{2}(g) rightleftharpoons 2 H I(g)+3000 c a l )
B ( cdot N_{2}(g)+O_{2}(g) rightleftharpoons 2 N O(g)-43200 c a l )
( mathbf{c} cdot N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g)+22400 c a l )
( mathbf{D} cdot C(g)+O_{2}(g) rightleftharpoons C O_{2}(g)+94300 c a l )
11
230For which one of the following reactions
will ( boldsymbol{K}_{boldsymbol{C}}=boldsymbol{K}_{boldsymbol{P}} )
A ( cdot C O(g)+2 H_{2}(g) rightleftharpoons C H_{3} O H(g) )
в. ( Z n O(s)+C O(g) rightleftharpoons Z n(s)+C O_{2}(g) )
( mathrm{c} cdot 2 mathrm{O}_{3}(g) rightleftharpoons 3 mathrm{O}_{2}(g) )
D. ( operatorname{COCl}_{2}(g) rightleftharpoons operatorname{CO}(g)+C l_{2}(g) )
11
231Drive the following relation:
( boldsymbol{K} boldsymbol{p}=boldsymbol{K} boldsymbol{c}(boldsymbol{R} boldsymbol{T})^{n} )
11
232A solution has ( p H ) 2. It contains:
A. ( C H_{3} ) СООН
в. ( H_{2} C O_{3} )
c. ( H N O_{3} )
( mathrm{D} cdot mathrm{H}_{2} mathrm{C}_{2} mathrm{O}_{4} )
11
233Study the figure given below and mark
the correct statement about ( K_{c} ) and
dependence of extent of reaction on it.
A. ( x ) – Reaction does not occur
Y – Reaction proceeds to completion; Z – Reaction does not occur
B. X- Reaction completes; Y – Reaction does not occur; Z Reactants and products are at equilibrium
c. ( x ) – Reaction hardly occurs;
Y – Reactants and products are at equilibrium; Z – Reaction proceeds completion
D. ( x ) – Reaction proceeds completion; ( Y ) – Reactants and products are at equilibrium; Z – Reaction hardly occurs
11
234A monoprotic acid in ( 1.00 M ) solution is
( 0.001 % ) ionised. The dissociation
constant of acid is:
A. ( 1 times 10^{-3} )
В. ( 1 times 10^{-6} )
c. ( 1 times 10^{-8} )
D. ( 1 times 10^{-10} )
11
235Fresh milk has a pH of 6. Explain why the pH changes as it turns into curd?11
236The reaction is of first order in each
diagram, with an equilibrium constant of ( 10^{4} . ) For the conversion of chair form
to boat form ( e^{-E a / R T}=4.35 times 10^{-8} mathrm{at} )
( 298 K ) with pre-exponential factor of
( 10^{12} s^{-1} . ) Apparent rate constant ( left(=k_{A}right) )
at ( 298 K ) is:
A. ( 4.35 times 10^{4} s^{-1} )
в. ( 4.35 times 10^{8} s^{-1} )
c. ( 4.35 times 10^{-8} s^{-1} )
D. ( 4.35 times 10^{12} s^{-1} )
11
237The solubility product expression for silver (I) sulfide, using x to represent the molar concentration of silver (I) and y to represent the molar concentration of sulfide, is formulated as
A ( . x y )
B . ( x^{2} y )
c. ( x y^{2} )
D. ( x^{2} y^{2} )
E ( cdot x y^{3} )
11
238Ammonium sulfate is an example of:
A. an acid
B. a base
c. an acidic salt
D. a basic salt
11
239Which of the following according to LeChatelier’s principle is correct?
A. Increase in temperature favours the endothermic reaction
B. Increase in temperature favours the exothermic reaction
c. Increase in pressure shifts the equilibrium in that side in which number of gaseous moles increases
D. All of the above are true
11
240The value of ( K_{c}=4.24 ) at ( 800 K ) for the
reaction
( boldsymbol{C O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) )
Calculate equilibrium concentrations of
( C O_{2}, H_{2}, C O ) and ( H_{2} O ) at ( 800 K, ) if only
( C O ) and ( H_{2} O ) are present initially at concentration of ( 0.10 M ) each?
11
241( mathbf{5 0 m} boldsymbol{L} ) of ( mathbf{0 . 1 0} boldsymbol{M} boldsymbol{N} boldsymbol{a}_{3} boldsymbol{P} boldsymbol{O}_{4}+mathbf{5 0 m} boldsymbol{L} ) of
( mathbf{0 . 1 0} boldsymbol{M} boldsymbol{N a H}_{2} boldsymbol{O}_{4} )
11
242The unit of equilibrium constant for the following reaction is:
( mathbf{2} N boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{N}_{2} boldsymbol{O}_{4}(boldsymbol{g}) )
A ( . ) mol ( L^{-1} )
B. ( L ) mol ( ^{-1} )
c. ( m o l^{-1} L^{-1} )
D. Equilibrium constant is unitless
11
243The order of pH of ( 0.200 mathrm{M} ) solutions of
( N H_{4} N O_{3}, N a N O_{3} ) and ( N a_{2} C O_{3} ) is :
A. ( N H_{4} N O_{3}<N a_{2} C O_{3}<N a N O_{3} )
в. ( N H_{4} N O_{3}<N a N O_{3}<N a_{2} C O_{3} )
c. ( N a_{2} C O_{3}<N a N O_{3}<N H_{4} N O_{3} )
D. ( N a_{2} N O_{3}<N H_{4} N O_{3}<N a_{2} C O_{3} )
11
244When ( N a N O_{3} ) is heated in a closed
vessel, ( O_{2} ) is liberated and ( N a N O_{2} ) is left behind. At equilibrium:
A. increased temperature favours forward reaction
B. addition of ( N a N O_{2} ) favours reverse reaction
c. increased pressure favours forward reaction
D. adding of ( N a N O_{2} ) favours forward reaction
11
245( p H ) of a ( 0.001 mathrm{M} ) NaOH solution will be:
( A cdot 9 )
B. 3
( c )
D. 12
11
246The value of ( K_{c}=4.24 ) at ( 800 K ) for the
reaction
( boldsymbol{C O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) )
Calculate equilibrium concentrations of
( C O_{2}, H_{2}, C O ) and ( H_{2} O ) at ( 800 K, ) if only
( C O ) and ( H_{2} O ) are present initially at concentration of ( 0.10 M ) each?
11
247The value of ( K_{c} ) for the reaction: ( 2 A rightleftharpoons )
( B+C ) is ( 2 times 10^{-3} ). At a given time the
composition of reaction mixture is
( [boldsymbol{A}]=[boldsymbol{B}]=[boldsymbol{C}]=mathbf{3} times mathbf{1 0}^{-4} boldsymbol{M} . ) In which
direction the reaction will proceed?
A. Forward
B. Backward
c. At equilibrium
D. Forward or Backward
11
248The amount of ( left(N H_{4}right)_{2} S O_{4} ) to be added
to ( 500 mathrm{mL} ) of ( 0.01 mathrm{m} N H_{4} O H ) solution
( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}} ) for ( boldsymbol{N} boldsymbol{H}_{4}^{+} ) is ( boldsymbol{9} .2 boldsymbol{6} ) ) prepare a buffer
of ( p H=8.26 ) is?
A. 0.05 mole
B. 0.025 mole
c. 0.10 mole
D. 0.005 mole
11
249To ( 500 m L ) of ( 0.150 M A g N O_{3} ) solution
were added ( 500 m L ) of ( 1.09 M F e^{2+} )
solution and the reaction is allowed to
reach an equilibrium at 25
[
begin{array}{r}
boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q})+boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a} boldsymbol{q}) rightleftharpoons \
boldsymbol{F} boldsymbol{e}^{3+}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}(boldsymbol{s})
end{array}
]
For ( 25 m L ) of the solution, ( 30 m L ) of
( 0.0832 M K M n O_{4} ) were required for
oxidation. The equilibrium constant for
the reaction at ( 25^{circ} mathrm{C} ) is
11
250The homogeneous reaction is carried out in a 2 -litre container at a particular
temperature by taking 1 mole each of A,
B, ( C ) and ( D ) respectively. If ( K_{C} ) for the
reaction is ( frac{1}{4} ) then the equilibrium concentration of ( mathrm{C} ) is :
( boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}) rightleftharpoons boldsymbol{C}(boldsymbol{g})+boldsymbol{D}(boldsymbol{g}) )
A ( cdot frac{1}{3} M )
в. ( frac{2}{3} )
( ^{c} cdot frac{4}{3}^{M} )
D. ( frac{1}{2} M )
11
251Which of the following is a true
statement:
A. The ionisation constant and ionic product of water are same.
B. Water is a strong electrolyte.
C. The value of ionic product of water is less than that of its ionisation constant
D. At ( 298 K ), the number of ( H^{+} ) ions in a litre of water is ( 6.023 times 10^{16} )
11
252When heating ( P C l_{5}, ) it decompose
( P C l_{3} ) and ( C l_{2} ) in form of gas. The vapour density of gas mixture is 70.2 and 57.9
at ( 200^{circ} mathrm{C} ) and ( 250^{circ} mathrm{C} ). The degree of
dissociation of ( P C l_{5} ) at ( 200^{circ} C ) at ( 250^{circ} C )
is:
A . ( 48.50 % ) and ( 80 % )
B. 60% and 70%
c. ( 70 % ) and ( 80 % )
D. 80% and 90%
11
253The rate constant for the forward and
backward reactions of hydrolysis of
ester are ( 1.1 times 10^{-2} ) and ( 1.5 times 10^{-3} )
respectively. The equilibrium constant of the following reaction is:
( boldsymbol{C H}_{3} boldsymbol{C O O C}_{2} boldsymbol{H}_{5}+boldsymbol{H}^{+} rightleftharpoons )
( boldsymbol{C H}_{3} boldsymbol{C O O H}+boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{O H} )
A . 6.33
в. 7.75
( c .7 .33 )
D. 8.33
11
254Consider the two gaseous equilibrium
involving ( S O_{2} ) and the corresponding equilibrium constants at ( 299 mathrm{K} )
( boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+mathbf{1} / boldsymbol{2} boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ; boldsymbol{K}_{1} )
( mathbf{4} boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{4} boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{2} boldsymbol{O}_{2}(boldsymbol{g}) ; boldsymbol{K}_{2} )
The value of the equilibrium constant are related by :-
A ( cdot_{K_{2}}=frac{1}{left(K_{1}right)^{4}} )
B. ( K_{2}=K_{1}^{4} )
c. ( _{K_{2}}=left(frac{1}{K_{1}}right)^{1 / 4} )
D. ( _{K_{2}}=frac{1}{K_{1}} )
11
255Which of the following salts when dissolved in water will produce an
acidic solution?
( mathbf{1} cdot boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{C l} )
2. ( boldsymbol{K} boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4} )
3. ( boldsymbol{N a C N} )
A .2 and 3
B. 1 and 2
c. only 3
D. 2 and 4
11
2562 moles of ( P C l_{5} ) when heated in a
closed vessels of 2 litre capacity at
equilibrium ( 40 % ) of ( P C l_{5} ) dissociated
in ( P C l_{3} ) and ( C l_{2} . ) What is the value of the equilibrium constant?
A. 0.267
B. 0.786
c. 0.345
D. 1.879
11
2579.2 grams of ( N_{2} O_{4}(g) ) is taken in a
closed one litre vessel and heated till
the following equilibrium is reached,
( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) . ) At equilibrium,
( 50 % N_{2} O_{4}(g) ) is dissociated. What is
the equilibrium constant? (in ( M) )
(molecular weight of ( N_{2} O_{4}=92 ) )
A . ( 0 . )
B. 0.4
c. 0.3
D. 0.2
11
258Electrolytes include which of the following types of compounds?
A. Acids
B. Bases
c. Salts
D. All of the above
11
259Which of the following is an example of mineral acid?
A. Sulphuric acid
B. Acetic acid
c. Tartaric acid
D. All of above
11
260In the reaction, ( boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{I})= )
( N H_{4}^{+}+O H^{-} ) the water is a
A. bronsted acid
B. bronsted base
c. conjugate acid
D. conjugate base
11
261Passing ( boldsymbol{H}_{2} boldsymbol{S} ) gas into a mixture of ( M n^{2+}, N i^{2+}, C u^{2+} ) and ( H g^{2+} ) ions in
an acidified aqueous solution precipitates.
A. CuS and Hgs
B. MnS and cus
c. Mns and Nis
D. Nis and Hgs
11
262For the equilibrium in a closed vessel
( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) )
( K_{p} ) is found to be double of ( K_{c cdot} ) This is
attained when:
A. ( T=2 K )
в. ( T=12.18 K )
c. ( T=24.36 K )
D. ( T=27.3 K )
11
263What is the pH of ( 0.001 M H C l ? )
( A cdot 1 )
B. 2
( c .3 )
D. 4
11
264The equilibrium constant for the
reaction is 9.40 at ( 900^{circ} C )
( boldsymbol{S}_{2}(boldsymbol{g})+boldsymbol{C}(s) rightleftharpoons boldsymbol{C} boldsymbol{S}_{2}(boldsymbol{g}) )
Calculate the pressure of two gases at
equilibrium, when 1.42 at ( m ) of ( S_{2} ) and
excess of ( C(s) ) come to equilibrium.
11
265If the equilibrium constant for ( N_{2}(g)+ )
( O_{2}(g) rightleftharpoons 2 N O(g) ) is ( K, ) the equilibrium
constant for ( frac{1}{2} N_{2}(g)+frac{1}{2} O_{2}(g) rightleftharpoons )
( N O(g) ) will be:
A. ( K )
B. ( K^{2} )
c. ( K^{frac{1}{2}} )
D・( frac{1}{2} K )
11
266Q52. What is the pH of 0.001 M aniline solution? The ionization constant of aniline is
4.27 x 10-10. Calculate degree of ionization of aniline in the solution. Also calculate the
ionization constant of the conjugate acid of aniline.
(1)
Сттл
11
267A constant temperature, the
equilibrium constant ( left(boldsymbol{K}_{boldsymbol{p}}right) ) for the
decomposition reaction ( N_{2} O_{4} rightleftharpoons 2 N O_{2} )
is expressed by ( boldsymbol{K}_{boldsymbol{p}}=left(boldsymbol{4} boldsymbol{x}^{2} boldsymbol{p}right) /left(1-boldsymbol{x}^{2}right) )
where ( p= ) pressure and ( x= ) extent of
decomposition. Which one of the following statements is true?
A. ( K_{p} ) increases with increase in ( mathrm{p} )
B. ( K_{p} ) increases with increase in ( x )
C. ( K_{p} ) increases with decrease in ( x )
D. ( K_{p} ) remains constant with change in p and ( x )
11
268Litmus paper is turned red by the action
of:
( mathbf{A} cdot C H_{3} C H_{2} C H_{2} O H )
B ( cdot C H_{3} C H(B r) C H(B r) C H_{3} )
( mathbf{c} cdot C H_{3} C H_{2} C H(B r) C H_{3} )
D. ( C H_{3} C H_{2} C H_{2} C O O H )
( mathbf{E} cdot C H_{3} C H_{2} C H_{2} C H_{3} )
11
269In which of the following solution, ( A g C l )
has minimum solubility:
A. ( 0.05 M A g N O_{3} )
в. ( 0.01 M ) Са ( C l_{2} )
c. ( 0.01 M ) NaCl
D. ( 0.01 M N H_{4} O H )
11
270For a weak electrolyte molar conductance in dilute solution
increases sharply as its concentration in solution is decreased. Give reason.
11
271Law of mass action cannot be applied
to:
A. decomposition of gaseous ( H I )
B. decomposition of gaseous ( P C l_{5} )
C. transition of Rhombic Sulphur to Monoclicnic sulphur
D. decomposition of Calcium carbonate
11
272At ( 80^{circ} C, ) distilled water ( left(H_{3} O^{+}right) ) has
concentration equal to ( 1 times )
( 10^{-6} ) mol/litre. The value of ( K_{w} ) at this
temperature will be:
A ( cdot 1 times 10^{-6} )
B. ( 1 times 10^{-12} )
c. ( 1 times 10^{-9} )
D. ( 1 times 10^{-15} )
11
273Calculate the percentage ionization of
( 0.01 mathrm{M} ) acetic acid in ( 0.1 mathrm{M} ) HCl. ( boldsymbol{K}_{boldsymbol{a}} ) of
acetic acid is ( 1.8 times 10^{-5} )
A . ( 0.18 % )
B. 0.018%
c. ( 1.8 % )
D. 18%
11
274( mathrm{Ca}_{3}left(mathrm{PO}_{4}right)_{2}(mathrm{s}) leftrightharpoons 3 mathrm{Ca}^{2+}(mathrm{aq})+2 mathrm{PO}_{4}^{3-}(mathrm{aq}) )
Find the equilibrium expression for the
dissolution of ( boldsymbol{C a}_{3}left(boldsymbol{P} boldsymbol{O}_{4}right)_{2} ? )
( mathbf{A} cdot mathbf{K}_{s p}=left[mathbf{C} mathbf{a}^{2+}right]^{3}left[mathbf{P} mathbf{O}_{4}^{3-}right]^{2} )
B. ( kappa_{s p}=left[mathrm{Ca}^{2+}right]^{2}left[mathrm{PO}_{4}^{3-}right]^{3} )
C. ( kappa_{s p}=left[mathrm{Ca}^{2+}right]left[mathrm{PO}_{4}^{3-}right] /left[mathrm{Ca}_{3}left(mathrm{PO}_{4}right)_{2}right] )
D. ( kappa_{s p}=left[mathrm{Ca}^{2+}right]^{3}left[mathrm{PO}_{4}^{3-}right]^{2} /left[mathrm{C} mathrm{ca}_{3}left(mathrm{PO}_{4}right)_{2}right] )
E ( cdot K_{s p}=left[mathrm{Ca}^{2+}right]^{2}left[mathrm{PO}_{4}^{3-]}right]^{3} /left[mathrm{Ca}_{3}left(mathrm{PO}_{4}right)_{2}right] )
11
275( operatorname{Given} boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}^{+} rightleftharpoons boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{2} boldsymbol{N} boldsymbol{H}_{3} )
( boldsymbol{K}_{c}=mathbf{6 . 2} times mathbf{1 0}^{-8} ) and ( boldsymbol{K}_{s p} ) of ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) is
( 1.8 times 10^{-10} ) at ( 298 K . ) Calculate
concentration of the complex in ( 1 M )
aqueous ammonia.
11
2767. At constant temperature, the equilibrium constant (Kp)
for the decomposition reaction. NO. 2NO2 18
expressed by,
(44²P) ano ano to
(1-x²)
Кр
where P = pressure, x = extent of decomposition. Which
of the following statements is true?
(a) Kp increases with increase of P
(b) K, increases with increase of x
(C) K, increase with decrease of x
(d) K, remains constant with change in P or x
11
277Aqua regia consists of:
A. hydrochloric acid
B. carbonic acid
C. nitric acid
D. both ( A ) and ( C )
11
278State whether the given statement is true or false:
( boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2} ) is precipitated if ( left[boldsymbol{H} boldsymbol{g}_{2}^{2+}right]left[boldsymbol{C l}^{-}right]^{2} )
is greater than ( boldsymbol{K}_{boldsymbol{s p}}left(boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2}right) )
11
279Consider following reaction in equilibrium with equilibrium concentration ( 0.01 mathrm{M} ) of every species
(।) ( boldsymbol{P} boldsymbol{C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) )
(II) ( 2 H I(g) rightleftharpoons H_{2}(g)+I_{2}(g) )
(III) ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) )
Extend of the reaction taking place is:
A. ( I>I I>I I I )
в. ( I<I I<I I I )
c. ( I I<I I I<I )
D. III ( <I<I I )
11
280A sample of hard water contains
0.005 moles of ( C a C l_{2} ) per litre. What is
the minimum concentration Of
( N a_{2} S O_{4} ) which must be added for
removing ( C a^{2+} ) ions from the water
sample?
( left[K_{s p} text { for } C a S O_{4} text { is } 2.4 times 10^{-5} text {at } 25^{circ} Cright] )
A ( .2 .8 times 0^{-5} M )
В. ( 4.8 times 10^{-3} M )
c. ( 6.1 times 10^{-3} M )
D. ( 4.1 times 10^{-5} M )
11
281Molar solubility of ( mathbf{C a}(mathbf{O} mathbf{H})_{2} ) in a
solution that has a pH of 12.
( left[boldsymbol{K}_{boldsymbol{S P}}left[mathbf{C a}(mathbf{O H})_{2}right]=mathbf{5 . 6} times mathbf{1 0}^{-12}right] )
в. ( 5.6 times 10^{-8} M )
c. ( 4 times 10^{-4} M )
D. None
11
282Q50. The degree of ionization of a 0.1 M bromoacetic acid solution is 0.132. Calculate the pH of the
solution and the pk of bromoacetic acid.
TO
11
283For the reaction, ( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+ )
( C l_{2}(g), ) the position of equilibrium can
be shifted to the right by:
A. doubling the volume
B. increasing the temperature
c. addition of equimolar quantities of ( P C l_{3} ) and ( P C l_{5} )
D. addition of ( C l_{2} ) at constant volume
11
284The correct order of increasing basicity
of the given conjugate bases ( left(R=C H_{3}right. )
is:
A ( cdot mathrm{RCOO}^{-}<mathrm{HC}=mathrm{C}^{-}<mathrm{R}^{-}<mathrm{NH}_{2}^{-} )
B . ( mathrm{R}^{-}<mathrm{HC} equiv mathrm{C}^{-}<mathrm{RCOO}^{-}<mathrm{NH}_{2}^{-} )
C. ( mathrm{RCOO}^{-}<mathrm{NH}_{2}^{-}<mathrm{HC} equiv mathrm{C}^{-}<mathrm{R} )
D. ( mathrm{RCOO}^{-}<mathrm{HC} equiv mathrm{C}^{-}<mathrm{NH}_{2}^{-}<mathrm{R} )
11
285The reaction ( : boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{g}) rightleftharpoons )
( boldsymbol{C a O}(s)+boldsymbol{C O}_{2}(boldsymbol{g}), ) would proceed to
completion if the reaction vessel is
connected to bottle containing ( K O H )
solution or carried out in open vessel. If true enter ( 1, ) if false enter 0
11
286pH signifies
A. Power of hydrogen
B ( .-log left[H^{+}right] )
c. ( 14- ) pOH
D. All of the above
11
287A chemical reaction is said to have
attained equilibrium when:
A. equal amounts of reactants and products are formed
B. reactants are completely converted to products
C. the rate of forward reaction is equal to the rate of backward reaction
D. the concentration of the reactants and products is the
same
11
288When ( 16.8 g ) of white solid ( X ) was
heated ( 4.4 g ) of acid gas : ( (A) ) that
turned lime water milky was driven of
together with ( 1.8 g ) of a gas ( (B) ) which condensed to a colourless liquid the
solid that remained ( (Y) ) dissolved in
water to give an alkaline solution, which
with excess of ( B a C l_{2} ) solution gave a
white precipitate ( (Z) . ) The precipitate
effervescence with acid giving of ( boldsymbol{C O}_{2} )
gas. Identify the compound ( A, B ) and
write the chemical equations for the
thermal decomposition of ( X )
( mathbf{A} cdot(A)-C O_{2} )
( (B)-H_{2} O quad X rightarrow N a_{2} C O_{3} )
B. ( (A)-C O_{2} )
( (B)-H_{2} O_{2} quad X rightarrow N a C O_{3} )
( mathbf{c} cdot(A)-C O_{2} )
( (B)-H_{2} O_{2} quad X rightarrow N a_{2} C O_{3} )
D. ( (A)-C O_{2} )
( (B)-H_{2} O quad X rightarrow N a C O_{3} )
11
289The degree of dissociation of ( boldsymbol{P C l}_{5} ) will
be more at
A. constant pressure
B. low pressure
c. high pressure
D. none of these
11
290Assertion: Amphoteric species acts as either an acid or a base.

Reason: It contains both hydrophobic and hydrophilic regions.
A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion
B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
c. Assertion is true but Reason is false
D. Assertion is false but Reason is true
E. Both Assertion and Reason are false

11
291Consider the equilibrium set up:
( mathbf{2} boldsymbol{H}_{mathbf{2}(boldsymbol{g})}+boldsymbol{C} boldsymbol{O}_{(boldsymbol{g})} rightleftharpoons boldsymbol{C} boldsymbol{H}_{boldsymbol{3}} boldsymbol{O} boldsymbol{H}_{(boldsymbol{g})} )
What will be the effect of the following on the equilibrium of the reaction?
(i) Addition of ( boldsymbol{H}_{2} )
(ii) Addition of ( boldsymbol{C H}_{3} boldsymbol{O H} )
(iii) Removal of ( mathrm{CO} )
(iv) Removal of ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{O} boldsymbol{H} )
A. (i) – Forward direction
(ii) – Backward direction (iii) Backward direction (iv) – Forward direction
B. (i) – Backward direction
(ii) – Backward direction (iii) Forward direction (iv) – Forward direction
c. (i) – Forward direction
(ii) – Forward direction (iii) Backward direction
(iv) – Backward direction
D. (i) – Backward direction
(ii) – Forward direction (iii) Forward direction (iv) – Backward direction
11
292Which of the following expressions for ( % ) ionization of a monoacidic base
( (B O H) ) in aqueous solution is not correct at appreciable concentration?
A ( cdot_{100} times sqrt{frac{K_{b}}{c}} )
В. ( frac{1}{1+10left(p K_{b}-p O Hright)} )
с. ( frac{K_{w}left[H^{+}right]}{K_{b}+K_{w}} )
D. ( frac{K_{b}}{K_{b}+left[O H^{-}right]} )
11
293A well is dug in a bed of rock containing
fluorspar ( left(C a F_{2}right) . ) If the well contains ( 20000 mathrm{L} ) of water, what is the amount of
( boldsymbol{F}^{-} ) in it ( ?left(boldsymbol{K}_{s p}=boldsymbol{4} times mathbf{1 0}^{-11}right) )
A . 4.2 mol
B . 13.6 mol
c. 8.6 mol
D. 10 mol
11
294An equilibrium expression may
be forced to completion by:
B. increasing the pressure
C. increasing the temperature
D. removing the products from the reaction mixture as they are formed
E. decreasing the reactant concentration
11
295In an equilibrium reaction for which
( Delta G^{circ}=0 . ) Determine the value of
equilibrium constant ( mathrm{K} . delta G=0 )
A . 1.0
B. 2.7
( c .7 .6 )
D. 8.5
11
296The pH value of ( 10^{-7} ) M solution ( H C l ) is:
A. equal to 1
B. equal to 2
c. less than 7
D. equal to 0
11
297Common salt is chemically sodium chloride ( (N a C l) )
A. True
B. False
11
2982. 41 Match the following species with the corresponding conjugate acid.
Species Conjugate acid
A. NH4
1. co-
B. HCO3 2. NHỜ
с. Но
3. H₂O+
D. HSO:
4. H2SO4
5. H,
COW
11
299The solubility of ( M g(O H)_{2} ) in pure
water is ( 9.57 times 10^{-3} g L^{-1} . ) Calculate its
solubility in ( g L^{-1} ) in ( 0.02 M )
( M gleft(N O_{3}right)_{2} ) solution.
11
300Chemical equation of the industrial
preparation of ( boldsymbol{S} boldsymbol{O}_{3} ) is given?
( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3}+ ) Heat
What is the influence of the following factors in this system at equilibrium?
(a) Increasing the amount of ( boldsymbol{O}_{2} )
(b) ( S O_{2} ) is removed from the system.
(c) Decreasing the temperature.
11
301On decomposition of ( N H_{4} H S, ) the
following equilibrium is established:
( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{H} boldsymbol{S}(boldsymbol{s}) rightleftharpoons boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) ) If
the total pressure is ( P ) atm, then
the equilibrium constant ( boldsymbol{K}_{boldsymbol{P}} ) is equal
to:
( A cdot P ) atm
B. ( P^{2} a t m^{2} )
( mathbf{c} cdot P^{2} / 4 a t m^{2} )
D. 2P atm
11
302An equilibrium mixture in a vessel of capacity 100 litre contain
1 mol ( N_{2}, 2 ) mol ( O_{2} ) and
3 mol NO.No. of moles of ( 0_{2} ) to be
added so that at new equilibrium the conc. of NO is found to be 0.04 mol/lit :
A ( .(101 / 18) )
B. (101/9)
c. (202/9)
D. None of these
11
303Any salt ( M C l_{2} ) is soluble in water, if
it’s hydration energy exceeds the lattice
energy of ( M C l_{2} )
A. True
B. False
11
304Q38. Write the conjugate acids for the following Bronsted bases:
NH, NH, and HCOO-
11
305Hydronium exist even in pure water
A. True
B. False
11
306( H_{3} B O_{3} ) is named as
A. boric acid
B. monobasic and weak bronsted acid
c. dibasic and strong lewis acid
D. tribasic and weak bronsted acid
11
307(A) pH of ( 10^{-7} ) M NaOH solution exists
between 7 to 7.3 at ( 25^{circ} C )
(R) Due to common ion effect ionization
of water is suppressed.
A. Both (R) and (A) are true and reason is the correct explanation of assertion
B. Both (R) and (A) are true but reason is not correct explanation of assertion
c. Assertion
(A) is true but reason
(R) is false
D. Assertion
(A) and reason
(R) both are false
E. Assertion (A) is false but reason (R) is true
11
308What is the ( K_{b} ) of a weak base
that produces an ( O H^{-} ) per molecule if a 0.05 M solution is ( 2.5 % ) ionized?
( mathbf{A} cdot 7.8 times 10^{-8} )
B . ( 1.6 times 10^{-6} )
c. ( 3.125 times 10^{-5} )
D. ( 1.2 times 10^{-3} )
11
309Assertion
The energy profile of the reaction ( boldsymbol{A}+ )
( B rightleftharpoons C ) is given as above, then the K of
the above equilibrium increases with
increase of temperature
Reason
Endothermic reaction is favoured by
increase of temperature
A. Both assertion and reason are true but reason is the correct explanation for assertion
B. Both assertion and reason are true but reason is not the correct explanation for assertion
c. Assertion is true but reason is false
D. Assertion is false but the reason is true
11
310Assertion
It is difficult to distinguish the strengths of the strong acids such as
( boldsymbol{H} boldsymbol{C l}, boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}, boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} boldsymbol{H} boldsymbol{B} boldsymbol{r}, boldsymbol{H} boldsymbol{I} ) or
( boldsymbol{H} boldsymbol{C l O}_{4} ) in dilute aqueous solutions.
Reason

In dilute aqueous solution all strong acids donate a proton to water and are
essentially ( 100 % ) ionised to produce a
solution containing ( H_{3} O^{+} ) ions plus the anions of strong acid.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct

11
311Available chlorine can be liberated from
bleaching powder by the reaction with:
This question has multiple correct options
A ( cdot ) conc. ( H_{2} S O_{4} )
в. ( d i l . H_{2} S O_{4} )
( c cdot C O_{2} )
D. ( d i l . H N O_{3} )
11
312mole of ( A(g) ) is heated to ( 300^{circ} C ) in closed one litre vessel till the following equilibrium is reached: ( boldsymbol{A}(boldsymbol{g}) Leftrightarrow boldsymbol{B}(boldsymbol{g}) )
The equilibrium constant for
the reaction at ( 300^{circ} mathrm{C} ) is ( 4 . ) What is the
concentration of ( mathrm{B}left(text { in } operatorname{mol} . l i t^{-1}right) ) at
equilibrium?
A . 0.2
B. 0.6
( c cdot 0.8 )
D. 0.1
11
313Match the column I with column II and
mark the appropriate choice.
Column I
(i) Saturated
(A) Liquid ( leftrightarrow ) Vapour
(B) Solid ( leftrightarrow ) Liquid
(ii) Boiling point
(C) Solid ( leftrightarrow )
(iii) Sublimation vapour ( quad ) point
(D) Solute
( (s) leftrightarrow )
(iv) Melting point Solute(solution)
( A cdot(A)-(i),(B)-(i i i),(C)-(i i),(D)-(i v) )
B. (A) – (ii), (B) – (iv), (C) – (iii), (D) – (i)
C. ( (A)-(i v),(B)-(i i),(C)-(i),(D)-(i i i) )
D. (A) – (iii), (B) – (iv), (C) – (ii), (D) – (i)
11
314The equilibrium constant for the reaction ( boldsymbol{w}+boldsymbol{x} rightleftharpoons boldsymbol{y}+boldsymbol{z} ) is ( 9 . ) If one mole
of each of wand ( x ) are mixed and there is
no change in volume, the number of moles of y for formed is :
A . 0.10
B. 0.50
c. 0.75
D. 0.54
11
31512 lowerg we dluvallun energyu) HILU
5. What is the correct expression for the representation of the solubility product constant
of Ag, Cro?
(a) [Ag+12 [Cro1(b) [2Ag 1 [Cro21 (c) (Ag 1 [Cro2-1 (d) [2Ag+1? [Cro21
11
31616. Amphoprotic substances are those
(a) which can donate a proton
(b) which can accept a proton
(c) which can accept and donate proton
(d) which can donate hydroxyl ion
11
3170.010
Q10. At 450 K, K, = 2.0 < 1010 bar-1 for the equilibrium reaction:
250, (g) + 02 (8) = 250, (8)
What is K at this temperature?
11
318Q62. A 0.02 M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization
constant of pyridine.
TT
1+1
10-4 M
11
319The ( K_{p} ) value for ( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons )
( 2 S O_{3}(g) ) is ( 5.0 a t m^{-1} )
If the equilibrium pressures of ( S O_{2} ) and
( boldsymbol{S} boldsymbol{O}_{3} ) are equal. What is the equilibrium
pressure of ( boldsymbol{O}_{2} ? )
A. 0.2 atm
B. 0.3 atm
( c .0 .4 ) atm
D. ( 0.1 mathrm{atm} )
11
320Mark the correct statement(s) based on
the phase diagram of ( C O_{2} ) shown in the graph.
rhis question has multiple correct options
A ( cdot 298 mathrm{K} ) is the normal boiling point of liquid ( C O_{2} )
B. At 1 atm & 190 K ( C O_{2} ) will exist as gas.
( mathrm{c} cdot mathrm{CO}_{2}(s) ) will sublime above ( 195 mathrm{K} ) under norma atmospheric pressure
D. Melting point & boiling point of ( C O_{2} ) will increase on increasing pressure.
11
321A vessel contains 1 mole ( boldsymbol{P} C l_{5}(g) ) at 4
( operatorname{atm} ) and 0.5 mole ( P C l_{3} ) formed at
equilibrium. Now, equilibrium pressure of mixture is (assume ideal behavior)
( A cdot 16 ) atm
B. 6 atm
( c cdot 2 ) atm
D. 4.5 atm
11
3224 moles of ( H_{2} ) at ( 500 mathrm{K} ) is kept in an
adiabatic rigid container.After some time it was found that 1 mole of the gas
dissociated intoHatoms. The
dissociation energy permole of ( boldsymbol{H}_{2} ) gas is 2000 cal,Let the new temperature of
the gas be 100 T. The integral value of ( T ) is : (Use ( mathrm{R}=2 mathrm{cal} / mathrm{mole}-mathrm{K}) )
A. 3
B. 4
( c cdot 5 )
D. 6
E. 2
11
323If the solubility of the salt
( boldsymbol{L} boldsymbol{i}_{3} boldsymbol{N} boldsymbol{a}_{3}left(boldsymbol{A l} boldsymbol{F}_{6}right)_{2} ) is ( boldsymbol{x}, ) then its solubility
product would be:
A ( cdot 26 x^{8} )
B . ( 2916 x^{8} )
( mathbf{c} cdot 256 x^{6} )
D. none of these
11
324An exothermic reaction which proceeds with decrease in volume will give
maximum yield at high ( P ) and low ( T )
If true enter 1 , if false enter 0 .
11
325What is buffer solution? Give an
example.
11
326A buffer solution is prepared in which the concentration of ( N H_{3} ) is ( 0.30 M ) and
the concentration of ( N H_{4}^{+} ) is ( 0.20 M . ) If
the equilibrium constant, ( boldsymbol{K}_{boldsymbol{b}} ) for ( boldsymbol{N} boldsymbol{H}_{3} )
equals ( 1.8 times 10^{-5}, ) what is the pH of
this solution? ( (log 2.7=0.433) )
A . 9.08
B. 9.43
c. 11.72
D. 8.73
11
327In a three litre vessel, 2 moles of ( N_{2} ) and
3 moles of length ( boldsymbol{H}_{2} ) are taken. If at
equilibrium ( x ) moles of ( N_{2} ) were obtained then the concentration of
( N H_{3} ) at equilibrium will be:
( mathbf{A} cdot 2-x )
B. ( 4-2 x )
c. ( frac{2 x}{3} )
D. ( frac{4-2 x}{3} )
11
328When one mole of ( P(g) ) is introduced in one litre closed rigid vessel maintained at constant temperature, the following equilibrium is established. ( boldsymbol{P}(boldsymbol{g}) rightleftharpoons boldsymbol{Q}(boldsymbol{g})+boldsymbol{R}(boldsymbol{g}) quad Longrightarrow boldsymbol{K}left(boldsymbol{C}_{1}right) )
( boldsymbol{R}(boldsymbol{g}) rightleftharpoons boldsymbol{S}(boldsymbol{g})+boldsymbol{Q}(boldsymbol{g}) quad Longrightarrow boldsymbol{K}left(boldsymbol{C}_{2}right) )
f the final equilibrium pressure is 2 times of the initial pressure, then the value of ( frac{boldsymbol{K}left(boldsymbol{C}_{2}right)}{boldsymbol{K}left(boldsymbol{C}_{1}right)} ) is
[Ratio of the equilibrium concentration of ( Q text { and } R text { is } 5] )
11
329Calculate the weight of ( left(N H_{4}right)_{2} S O_{4} ) which must be added to ( 500 mathrm{mL} ) of ( 0.2 mathrm{M} )
( N H_{3} ) to yield a solution of ( mathrm{pH}=9.35, K_{b} )
for ( boldsymbol{N} boldsymbol{H}_{3}=mathbf{1 . 7 8} times mathbf{1 0}^{-mathbf{5}} ) (in ( mathrm{gm} ) )(Write
11
330The solubility in water of a sparingly soluble salt ( A B_{2} ) is ( 1.0 times 10^{-5} ) mol ( L^{-1} )
Its solubility product will be:
A ( cdot 4 times 10^{-15} )
В. ( 4 times 10^{-10} )
c. ( 1 times 10^{-15} )
D. ( 1 times 10^{-10} )
11
331Iron filling and water were placed in a 5
litre vessel and sealed. The tank was
heated to ( 1000^{circ} mathrm{C} ). Upon analysis the tank was found to contain ( 1.1 mathrm{g} ) of hydrogen and 42.5 g of water vapour. If the reaction in the tank is represented
by ( 3 mathrm{Fe}(mathrm{s})+4 boldsymbol{H}_{2} boldsymbol{O}_{(g)} rightleftharpoons boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4}(boldsymbol{s})+ )
( mathbf{4} boldsymbol{H}_{2}(boldsymbol{g}) )
The value of equilibrium constant, ( boldsymbol{K}_{c} )
is:
A . 30
B. 0.03
( c cdot 3 )
D. 0.003
11
332If the solubility product of a sparingly
soluble salt ( M X_{2} ) at ( 25^{circ} C ) is ( 1.0 times )
( mathbf{1 0}^{-11}, ) the solubility of the salt in moles
( L^{-1} ) at this temperature will be:
A ( .2 .46 times 10^{14} )
B . ( 1.36 times 10^{-4} )
c. ( 2.60 times 10^{-7} )
D. ( 1.20 times 10^{-10} )
11
333At ( 25^{circ} C,_{-}-_{-}– ) produces an aqueous
solution with ( p H>7 )
A. Arrhenius acid
B. Arrhenius base
c. Buffer
D. Indicator
E. Salt
11
334A buffer solution with ( p H=9 ) is to be
prepared by mixing ( N H_{4} C I ) and
( N H_{4} O H . ) Calculate the number of
moles of ( N H_{4} C I ) that should be added
to one litre pf ( 1.0 M N H_{4} O H .left[K_{b}=right. )
( left.1.8 times 10^{-5}right] )
A . 3.4
B . 2.
c. 1.5
D. 1.8
11
335A beaker contains a saturated solution
of copper(l) chloride. Copper(l) chloride is slightly soluble salt with a solubility product of ( 1.2 times 10^{-6} )
Which of the following salts when added to the solution would precipitate
copper(l) chloride?
A. Sodium chloride
B. Potassium bromide
c. Silver(I) nitrate
E. Magnesium iodide
11
336What is the ( p H ) of ( 0.001 mathrm{M} ) aniline
solution ? The ionization constant of
aniline can be taken from Table 7.7
Calculate the degree of ionization of
aniline in the solution. Also calculate
the ionization constant of the conjugate acid of aniline.
11
337The ( p H ) of ( 0.1 M ) solution of the
following salts increases in the order:
A ( cdot operatorname{NaCl}<N H_{4}^{+}<N a C N<H C l )
в. ( H C l<N H_{4}^{+}<N a C l<N a C N )
c. ( operatorname{NaCN}<N H_{4}^{+}<N a C l<H C l )
D. ( H C l<N a C l<N a C N<N H_{4} )
11
338Acetyl salicylic acid (aspirin) ionises in
water as: ( boldsymbol{H} boldsymbol{C}_{9} boldsymbol{H}_{7} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O} rightarrow )
( boldsymbol{H}_{3} boldsymbol{O}^{+}+boldsymbol{C}_{9} boldsymbol{H}_{7} boldsymbol{O}_{4}^{-} ;left(boldsymbol{K}_{a}=boldsymbol{2} . boldsymbol{7} boldsymbol{5} times mathbf{1} boldsymbol{0}^{-boldsymbol{9}}right) )
If two tablets of aspirin each of 0.32 g is dissolved in water to produce ( 250 mathrm{mL} ) solution, calculate ( [stackrel{ominus}{boldsymbol{O}} boldsymbol{H}] )
A ( cdot 1.61 times 10^{-9} M )
В. ( 1.61 times 10^{-7} ) М
c. ( 1.61 times 10^{-3} M )
D. ( 1.61 times 10^{-5} M )
11
339What is the concentration of
( C H_{3} C O O H ) which can be added to 0.5 M HCOOH solution so that dissociation
of both is same.
[Given that ( : boldsymbol{K}_{boldsymbol{C H}_{3} text { COOH}}=mathbf{1 . 8} times )
( mathbf{1 0}^{-5}, quad boldsymbol{K}_{boldsymbol{H} mathrm{COOH}}=mathbf{2 . 4} times mathbf{1 0}^{-4} mathbf{j} )
(as nearest integer)
11
340Extent of a reaction can always be increased by increasing the temperature.
A. True
B. False
11
341( p K_{a} ) values of four acids are given
below at ( 25^{circ} mathrm{C} ). The strongest acid is:
A . 2.0
в. 2.
c. 3.0
D. 4.0
11
342At ( 25^{circ} C, K_{p} ) for the reaction:
( N_{2} O_{4}(g) leftrightharpoons 2 N O_{2}(g) )
has a value of 0.14 atm. Calculate the
value of ( K_{c} ) in which the concentrations
are measured in mol ( boldsymbol{L}^{-1} )
11
343Which information can be obtained
from Le Chatelier’s principle?
A. Shift in equilibrium position on changing ( P, T ) and concentration
B. Dissociation constant of a weak acid
c. Energy change in a reaction
D. Equilibrium constant of a chemical reaction
11
344Which one of the following is a strong
electrolyte?
A. ( C H_{3} ) СООН
в. ( H C O O H )
c. ( H_{2} C O_{3} )
D. ( N a O H )
11
345( X Y_{2} ) dissociates as: ( X Y_{2}(g) rightleftharpoons )
( boldsymbol{X} boldsymbol{Y}(boldsymbol{g})+boldsymbol{Y}(boldsymbol{g}) )
Initial pressure of ( boldsymbol{X} boldsymbol{Y}_{2} ) is ( boldsymbol{6} boldsymbol{0} boldsymbol{0} boldsymbol{m} boldsymbol{m} boldsymbol{H} boldsymbol{g} )
The total pressure at equilibrium is ( 800 m m H g . ) Assuming volume of system to remain constant, the value of
( boldsymbol{K}_{p} ) is:
A . 50
в. 100
c. 200
D. 400
11
346Q. 38 Match the following equilibria with the corresponding condition.
A Liquid Vapour
Saturated solution
B. Solid Liquid
2. Boiling point
C. Solid Vapour
3. Sublimation point
D. Solute (s) Solute (solution) 4. Melting point
5. Unsaturated solution
11
347In a 0.25 -liter tube dissociation of 4
moles of NO is took place. If its degree of
dissociation is ( 10 % . ) The value of ( boldsymbol{K}_{boldsymbol{p}} ) for
reaction ( 2 N O rightleftharpoons N_{2}+O_{2} ) is:
A ( cdot frac{1}{(18)^{2}} )
в. ( frac{1}{(8)^{2}} )
c. ( frac{1}{(16)} )
D. ( frac{1}{(32)} )
11
348By which method you can dilute a
concentrated acid properly?
A. Carefully replace unused or excess chemicals into their properly labeled containers from which they came
B. The rule is to add water to the concentrated acid slowly
C. Dispose of chemicals in the proper places following posted procedures. Do not return them to their original containers
D. Flush eyes with water at the eyewash fountain for at least 15 minutes, and then report the accident for further help
E. The rule is to add concentrated acid to water slowly
11
349In the reaction ( 2 P(g)+Q(g) rightleftharpoons )
( 3 R(g)+S(g) . ) If 2 moles each of ( P ) and
( Q ) is taken initially in a 1 litre flask. At equilibrium which of the following is
true?
( mathbf{A} cdot[P]<[Q] )
B ( cdot[P]=[Q] )
( mathbf{c} cdot[Q]=[R] )
D. None of these
11
350( N a H C O_{3} ) can be used on its own to
make cakes or bread. Baking powder is more commonly used, and contains
( N a H C O_{3}, C aleft(H_{2} P O_{4}right)_{2} ) and starch. An
improved combination baking powder contains about ( 40 % ) starch, ( 30 % )
( N a H C O_{3} 20 % N a A lleft(S O_{4}right)_{2} ) and ( 10 % )
( boldsymbol{C a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}right)_{2} )
Answer the following questions based on above study.
( boldsymbol{C} boldsymbol{a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}right)_{2} ) in baking powder:
A. behaves as an acid in moist condition and decomposes ( N a H C O_{3} ) to give ( C O_{2} )
B. behaves as a base in moist condition and gives ( H_{3} P O_{4} )
c. behaves as a binder
D. behaves as a filler
11
351One mole of nitrogen and three moles of hydrogen are mixed in a 4 litre container. If 0.25 percent of nitrogen is converted to ammonia by the following reaction
( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) )
What will be the value of ( K ) for the
following equilibrium? ( frac{1}{2} N_{2}(g)+frac{3}{2} H_{2}(g) rightleftharpoons N H_{3}(g) )
A ( cdot 1.49 times 10^{-5} L ) mol ( ^{-1} )
В . ( 2.22 times 10^{-10} L ) mol ( ^{-1} )
D. None of these
11
352The equilibrium ( boldsymbol{A}_{4}(boldsymbol{g})+boldsymbol{6} boldsymbol{B}_{2}(boldsymbol{g}) rightleftharpoons )
( 4 A B_{3}(g) ) is established in a closed
container by taking equal moles of
( A_{4}(g) ) and ( B_{2}(g) . ) Which of the following options must be correct at equilibrium?
( mathbf{A} cdotleft[A_{4}right]left[A B_{3}right] )
c. ( left[A_{4}right]<left[A B_{3}right] )
D. None of the above
11
353Some of alkali metal salts are coloured
( N a_{2} C r O_{4}- ) yellow, ( K M n O_{4}- ) pink
( K_{2} M n O_{4} ) -green. It is due to:
A. cations are coloured ions
B. anions are coloured ions
c. both ( A ) and ( B )
D. none of the above
11
354In the reaction :-
[
begin{array}{r}
boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons mathbf{2} boldsymbol{C u} boldsymbol{S} boldsymbol{O}_{4} \
boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})+mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{v})
end{array}
]
Dissociation pressure is ( 7 times 10^{-3} ) atm
at 25 and ( Delta H=2700 ) cal. If the
dissociation pressure at 127 is ( X times )
[
10^{-3} text {atm, then } 100 X
]
is
11
355The solubility of ( C a C O_{3} ) is ( 7 m g / )litre. Calculate the solubility product of
( B a C O_{3} ) from this information and from
the fact that when ( N a_{2} C O_{3} ) is added
slowly to a sloution containing equimolar concentration of ( C a^{2+} ) and
( B a^{2+}, ) no precipitate is formed until 90
( % ) of ( B a^{2+} ) has been precipitated as
( B a C O_{3} . ) The solubility product of ( B a C O_{3} ) is ( X times 10^{-10} ) mol ( ^{2} l i t r e^{-2}, ) the
value of integer nearest to ( boldsymbol{X} ) is:
11
356The relative strength of two weak bases at same concentration may be given as:
This question has multiple correct options
( ^{mathbf{A}} cdot frac{K_{b_{1}}}{K_{b_{2}}} )
( ^{mathrm{B}} cdotleft[frac{left[O H^{-}right]_{1}}{left[O H^{-}right]_{2}}right. )
c. ( frac{alpha_{1}}{alpha_{2}} )
D. ( frac{sqrt{K_{b_{1}}}}{sqrt{K_{b_{2}}}} )
11
357Q54. The ionization constant of dimethylamine is 5.4 x 104. Calculate its degree of ionization in its
0.02 M solution. What percentage of dimethylamine is ionized if the solution is also 0.1 Min
NaOH?
054. Trezimi solution. W
11
358Match the following
( begin{array}{lll}text { S.No } & text { Source } & text { Acid present } \ 1 . & text { Apple } & text { Oxalic acid } \ 2 . & text { Lemon } & text { Tartaric acid } \ 3 . & text { Grape } & text { Malic Acid } \ 4 . & text { Tomato } & text { Citric Acid }end{array} )
11
359What is the minimum pH of a solution
( 0.10 M ) in ( M g^{2+} ) from which ( M g(O H)_{2} )
will not precipitate? ( boldsymbol{K}_{s p} boldsymbol{M} boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2}= )
( mathbf{1} . mathbf{2} times mathbf{1 0}^{-mathbf{1 1}} mathbf{M}^{mathbf{3}} )
11
360Determine the number of moles of ( boldsymbol{A} boldsymbol{g} boldsymbol{I} )
which may be dissolved in 1 litre of ( 1 M )
of ( C N^{-} ) solution ( K_{s p} ) for ( A g I ) and ( K_{c} ) for
( A g(C N)_{2}^{-} 1.2 times 10^{-17} M^{2} ) and ( 7.1 times )
( 10^{-19} M^{-2} ) respectively.
11
361Calculate percentage degree of hydrolysis in a ( 0.1 ~ M ) solution of
( boldsymbol{C H}_{3} boldsymbol{C O O N a} )
Given that ( :left[boldsymbol{K}_{boldsymbol{a}} boldsymbol{o} boldsymbol{f} boldsymbol{C H}_{3} boldsymbol{C O O H}=right. )
( left.mathbf{1 0}^{-mathbf{5}}right] )
A . 1.0
B. 0.01
( c cdot 10^{-4} )
D. None of these
11
362The dissociation constants for acetic
acid and ( H C N ) at ( 25^{circ} C ) are ( 1.5 times 10^{-5} )
and ( 4.5 times 10^{-10} ) respectively. The
equilibrium constant for the following equilibrium would be:
[
begin{array}{r}
C N^{-}+C H_{3} C O O H rightleftharpoons \
H C N+C H_{3} C O O^{-}
end{array}
]
A ( cdot 3 times 10^{4} )
B. ( 3 times 10^{5} )
( mathrm{c} cdot 3 times 10^{-5} )
D. ( 3 times 10^{-4} )
11
363The compounds ( A ) and ( B ) are mixed in equimolar proportion to form the products, ( boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{C}+boldsymbol{D} . ) At
equilibrium, one-third of ( A ) and ( B ) are
consumed. The equilibrium constant for the reaction is:
A . 0.5
в. 4.0
c. 2.5
D. 0.25
11
364The solubility product of ( A g B r ) is ( 4.9 times )
( 10^{-9} . ) The solubility of AgBr will be:
A. ( 7 times 10^{-4} ) mole /litre
B. ( 7 times 10^{-5} g / )litre
c. ( 1.316 times 10^{-2} g / )litre
D. ( 1 times 10^{-3} ) mole ( / )litre
11
365Solubility of ( A s_{2} S_{3} ) in aqueous solution
is ( operatorname{Smol} L^{-1} ). Its solubility product is
( 108 S^{n} . ) What will be the value of ( n ? )
11
366Assertion
Sodium bicarbonate is an acidic salt.
Reason
It gives basic solution in water.
A. If both assertion and reason are correct and reason is the correct explaination of the assertion
B. If both assertion and reason are correct, but reason is
not the correct explanation of the assertion
C. If assertion is correct, but reason is incorrect
D. If assertion is incorrect, but reason is correct
11
367Nitric acid is a:
A. diprotic acid
B. strong acid
C . organic acid
D. both ( A ) and ( C )
11
368( N a C l ) is less soluble in ( D_{2} O ) than ( H_{2} O )
why?
11
369( 0.001 M N H_{4} C l ) aqueous solution has
( mathbf{p H}: )
A . 6.127
B. 7.126
c. 2.167
D. 1.267
11
370( boldsymbol{K} boldsymbol{O} boldsymbol{H}(boldsymbol{a} boldsymbol{q}) rightleftharpoons )
A ( cdot K^{-}+O H^{+} )
B. ( K^{+}+O H^{+} )
( mathbf{c} cdot K^{-}+O H^{-} )
( mathbf{D} cdot K^{+}+O H^{-} )
11
371A definite amount of solid ( N H_{4} H S ) is placed in a flask already containing gas at a certain temperature and 0.50 atm
pressure. ( N H_{4} H S ) decomposes to give
( N H_{3} ) and ( H_{2} S ) and at equilibrium total
pressure in flask is 0.84 atm. The
equilibrium constant for the reaction is:
A . 0.30
B. 0.18
c. 0.17
D. 0.11
11
372A 0.004 M solution of ( N a_{2} S O_{4} ) is
isotonic with a ( 0.010 mathrm{M} ) solution of
glucose at same temperature. The apparent degree of dissociation of
( N a_{2} S O_{4} ) is:
A . ( 25 % )
B . 50%
c. ( 75 % )
D. 85%
11
373The graph (2) tells us that:
A. The reaction is irreversible
B. The reaction is reversible
C. The reaction is exothermic
D. The reaction is endothermic
11
374Which acid helps in the digestion of food without harming the stomach?
A. ( H_{2} S O_{4} )
в. НС l
c. ( C H_{3} ) СООН
D. ( H_{3} P O_{4} )
11
375Q.8 The ionisation constant of an acid, K, is the measure of strength of an
acid. The K, values of acetic acid, hypochlorous acid and formic acid are
1.74 X 10″, 3.0 x 10-8 and 1.8 x 10-4 respectively. Which of the
following orders of pH of 0 1 mol dm–solutions of these acids is correct?
(a) Acetic acid > hypochlorous acid > formic acid
(b) Hypochlorous acid > acetic acid > formic acid
(c) Formic acid > hypochlorous acid > acetic acid
(d) Formic acid > acetic acid > hypochlorous acid
TL
11
376The values of ( boldsymbol{K}_{s p} ) of ( boldsymbol{C a C O}_{3} ) and ( mathrm{CaC}_{2} mathrm{O}_{4} ) are ( 4.7 times 10^{-9} ) and ( 1.3 times 10^{-9} )
respectively at ( 25^{circ} mathrm{C} ). If the mixture of these two is washed with water, what is
the concentration of ( C a^{2+} ) ions in
water?
A ( cdot 7.746 times 10^{-5} M )
В. ( 5.831 times 10^{-5} M )
c. ( 6.856 times 10^{-5} M )
D. ( 3.606 times 10^{-5} M )
11
377In the aqueous solution of sodium acetate the ion that undergoes hydrolysis is :
A. ( C H_{3} C O O^{-} )
В. ( N a^{+} )
c. ( N a^{+} ) and ( C H_{3} C O O )
D. ( N a^{-} )
11
378Equilibrium constant for the following
reaction is ( 1 times 10^{-9} )
( boldsymbol{C}_{5} boldsymbol{H}_{5} boldsymbol{N}(boldsymbol{a} boldsymbol{q} cdot)+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) rightleftharpoons )
( boldsymbol{C}_{5} boldsymbol{H}_{5} boldsymbol{N} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q} cdot)+boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{a} boldsymbol{q} cdot) )
Determine the mole of pyridinium
chloride ( left(C_{5} H_{5} N . H C Iright) ) that should be
added to ( 500 mathrm{mL} ) solution of ( 0.4 mathrm{M} )
pyridine ( left(C_{5} H_{5} Nright) ) to obtain a buffer
solution of ( mathrm{pH}=5 )
A. 0.1 mole
B. 0.2 mole
c. 0.3 mole
D. 0.4 mole
11
379Which of the following is not a characteristic of equilibrium?
A. Rate is equal in both directions
B. Measurable quantities are constant at equilibrium
C . Equilibrium occurs in reversible condition
D. Equilibrium occurs only in open vessel at constant temperature
11
380( 20 % ) of ( N_{2} O_{4} ) molecule are dissociated
in a sample of ( operatorname{gas} ) at 27 degree ( C ) and 760 torr mixture has the density at the equilibrium
11
381Select the anion which is the
strongest bronsted base.
A ( cdot C l O_{4}^{-} )
B. ( C l O_{3}^{-} )
( mathrm{c} cdot mathrm{ClO}_{2}^{-} )
D. ( C l O^{-} )
11
382The solubility of ( P b S O_{4} ) in water is
( 0.038 g L^{-1} ) at ( 25^{circ} C . ) Calculate its
solubility at the same temperature.
11
383Common salt containing small amount of sodium iodide, is called iodised salt.
A. True
B. False
11
384A buffer solution is prepared by mixing ( 10 mathrm{ml} ) of ( 1.0 mathrm{M} ) acetic acid ( & 20 mathrm{ml} ) of 0.5
M sodium acetate and then diluted to
( 100 mathrm{ml} ) with distilled water. If the ( p K_{a} ) of
( C H_{3} C O O H ) is ( 4.76 . ) What is the pH of the buffer solution prepared? (1998)
A . 3.84
B. 4.76
( c cdot 4.34 )
D. 5.21
11
385Calculate the pressure of ( C O_{2} ) gas at 700 K in heterogeneous equilibrium
reaction ( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+ )
( C O_{2}(g) ) if ( Delta H ) for this reaction is
( 130.2 k J )
11
386Plaster of paris should be stored in a moisture proof container because:
A. it absorbs moisture from the atmosphere and becomes hard
B. it cannot be stored in plastic
c. it will change its colour
D. it will become soft
11
387Which of the following give brisk effervescence with baking soda?
A. methanoic acid
B. propanoic acid
c. ethanoic acid
D. all of these
11
388The gaseous phase neutralisation reaction can be explained only on the basis of:
A. Arrhenius theory
B. Lowry -Bronsted theory
c. Lewis theory
D. Bohrs theory
11
389( 25 m L ) of ( 0.107 M H_{3} P O_{4} ) was titrated
with ( 0.115 M ) solution of ( N a O H ) to the
end point identified by indicator bromocresol green. This required
( 23.1 m L ) The titration was repeated using phenolphthalein as indicator. This time ( 25 m L ) of ( 0.107 M H_{3} P O_{4} )
required ( 46.2 m L ) of the
( mathbf{0 . 1 1 5} M_{N a O H . text { What is the }} )
coefficient ( ^{prime} boldsymbol{n}^{prime} ) in the following reaction?
( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4}+boldsymbol{n} boldsymbol{O} boldsymbol{H}^{-} rightarrowleft[boldsymbol{H}_{3-n} boldsymbol{P} boldsymbol{O}_{4}right]^{n-}+ )
( boldsymbol{n} boldsymbol{H}_{2} boldsymbol{O} )
11
390Equilibrium constants for the following reaction at ( 1200 mathrm{K} ) are given
( 2 H_{2} O(g) leftrightharpoons 2 H_{2}(g)+O_{2}(g) ; K_{1}= )
( 6.4 times 10^{-8} )
( 2 C O_{2}(g) leftrightharpoons 2 C O(g)+O_{2}(g) ; K_{2}= )
( mathbf{1 . 6} times mathbf{1 0}^{-mathbf{6}} )
The equilibrium constant for the reaction
( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) leftrightharpoons boldsymbol{C} boldsymbol{O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) )
at ( 1200 mathrm{K} ) will be:
A. 0.05
в. 20
c. 0.2
D. 5.0
11
391Calculate the equilibrium constants for the reactions with water of
( H_{2} P O_{4}^{ominus}, H P O_{4}^{2-} ) and ( P O_{4}^{3-} ) as base
Comparing the relative values of two equilibrium constants of ( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{ominus} ) with
water, deduce whether solutions of this
ion in water are acidic or bases. Deduce
whether solutions of ( boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} ) are acidic
or bases. Given ( K_{1}, K_{2} ) and ( K_{3} ) for
( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} ) are ( mathbf{7 . 1} times mathbf{1 0}^{-mathbf{3}}, mathbf{6 . 3} times mathbf{1 0}^{-mathbf{8}} ) and
( 4.5 times 10^{-13} ) respectively
A ( .1 .4 times 10^{-12}, 1.6 times 10^{-7}, 2.2 times 10^{-2}, H_{2} P O_{4}^{circ} ) is acidic
and ( H P O_{4}^{2-} ) is basic
B . ( 2.2 times 10^{-12}, 1.6 times 10^{-7}, 1.4 times 10^{-2}, H_{2} P O_{4}^{ominus} ) is basic and
( H P O_{4}^{2-} ) is basic
C ( .2 .2 times 10^{-12}, 1.6 times 10^{-7}, 1.4 times 10^{-2}, H_{2} P O_{4}^{circ} ) is acidic
and ( H P O_{4}^{2-} ) is basic
D. ( 1.4 times 10^{-12}, 1.6 times 10^{-7}, 2.2 times 10^{-2}, H_{2} P O_{4}^{circ} ) is basic
and ( H P O_{4}^{2-} ) is acidic
11
392In a mixture of weak acid and its salt,
the ratio of the concentration of salt to
acid is increased tenfold.The pH of the solution would increase by:
A. 0.5
B.
( c cdot 10 )
D.
11
393What do the letters I ( C ) and ( E ) stand for in
a RICE table?
A . Initial, Change, Equilibrium
B. Initial, Concentration, Equilibrium
c. Instant, Change Equilibrium
D. Instant, Concentration, Equilibrium
E. Initial, Change, Exact amounts
11
394When inert gas at constant pressure is added to the given reversible process then the equilibrium will:
A. be unaffected
B. shift in backward direction
c. shift in forward direction
D. cannot predicted
11
395Which of the following is/are ionization?
This question has multiple correct options
A ( cdot N a rightarrow N a^{+}+e^{-} )
B. ( C l+e^{-} rightarrow C l^{-} )
c. ( N a C l rightarrow N a^{+}+C l^{-} )
D. ( M g B r_{2} rightarrow M g^{2+}+2 B r )
11
396Which of the following is correct for acid buffer?
( [text { salt }=H A, text { acid }=A] )
A ( cdot p^{K a}=p^{H}-log frac{[H A]}{|A|} )
B・ ( p^{H}=p^{K a}+log frac{[H A]}{|A|} )
c. ( p^{K a}=p^{H}-log frac{[A]}{[H A]} )
D・ ( p^{H}=p^{K a}+log frac{[A]}{[H A]} )
11
397Which of the following is correct regarding buffer solution?
A. It contains weak acid and its conjugate base.
B. It shows low change in pH on adding small amount of acid or base.
c. (A) and (B) both
D. None of these
11
398Which of the following are Bronsted acids as well as Bronsted bases?
( N H_{3}, H S O_{4}^{-}, H_{2} S O_{4}, H C O_{3}^{-}, H_{3} O )
11
399In the following strong acid and strong alkaine base is-
(a) Acetic Acid or Hydrochloric Acid
(b) Sodium hydroxide or calcium hydroxide
11
400A chemical which turns red litmus to
blue is:
A . acidic in nature
B. basic in nature
c. neutral in nature
D. can be acidic or basic in nature
11
401Q2. The values of Ksp of two sparingly soluble salts Ni(OH), and AgCN are 2.0 * 10
6x 10-respectively. Which salt is more soluble? Explain.
ana
OT
11
402Given that ( boldsymbol{K}_{c}=mathbf{1 3 . 7} ) at ( mathbf{5 4 6 K} ) for
( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) )
calculate what pressure will develop in a 10 litre box at equilibrium at ( 546 K )
when 1.00 mole of ( P C l_{5} ) is injected into
the empty box?
11
403( P C l_{2} rightleftharpoons P C l_{3}+C l_{2} ) in the reversible
reaction the moles of ( boldsymbol{P C l}_{2}, boldsymbol{P C l}_{3} ) and
( C l_{2} ) are ( a, b ) and ( c ) respectively and total
pressure is ( boldsymbol{P} ) then value of ( boldsymbol{K}_{boldsymbol{p}} )
is
A ( cdot frac{b c}{a} R T )
в. ( frac{b}{(a+b+c)} P )
c. ( frac{b c P}{a(a+b+c)} )
D. ( frac{c}{(a+b+c)} P )
11
404Addition of water to this solution will
not change ( left[boldsymbol{H}_{3} boldsymbol{O}^{+}right] )
A. Chemical pH indicator
B. Acid/base buffer
c. Anhydrous solution
D. Hypotonic solution
11
405What will be the pH of solution when ‘A’
and ‘C’ solutions are mixed completely?
A. 9.5
B. 5
c. 10.15
D. 8.85
11
406The pH of the solution obtained by mixing ( 100 mathrm{ml} ) of a solution of ( mathrm{pH}=3 ) with ( 400 mathrm{ml} ) of a solution of ( mathrm{pH}=4 ) is :
A. ( 3-log 2.8 )
B. ( 7-log 2.8 )
c. ( 4-log 2.8 )
D. ( 5-log 2.8 )
11
407Which of the following statement is correct about an aqueous solution of an acid and a base?
(i) Higher the pH, stronger the acid.
(ii) Higher the pH, weaker the acid.
(iii) Lower the pH, stronger the base.
(iv) lower the pH, weaker the base.
( A cdot ) (i) and (iii)
B. (ii) and (iii)
c. (i) and (iv)
D. (ii) and (iv)
11
408The equation for the solubility product
constant of ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4} ) is:
A ( cdot K_{s p}=left[A g^{2+}right] cdotleft[C r O^{2-}right] )
B . ( K_{s p}=left[A g^{+}right]^{2} cdotleft[C r^{6+}right] cdotleft[O_{4}^{8-}right] )
C ( cdot K_{s p}=left[A g^{+}right] cdotleft[C r^{6+}right] cdotleft[O_{4}^{8-}right. )
D. ( K_{s p}=left[A g^{+}right]^{2} cdotleft[C r O_{4}^{2-}right] )
11
409Q16. What is the equilibrium concentration of each of the substances in the equilibrium when the
initial concentration of ICI was 0.78 M?
2ICI(g) = 1,(8) + C1,(g); K = 0.14
11-1
11
410What will happen if the pH of the
solution of ( 0.001 mathrm{M} M gleft(N O_{3}right)_{2} ) solution
is adjusted to ( boldsymbol{p} boldsymbol{H}=mathbf{9} ? )
( left[text { Given that }: boldsymbol{K}_{s p} text { of } M g(boldsymbol{O} boldsymbol{H})_{2}=mathbf{8 . 9} timesright. )
( mathbf{1 0}^{-12} ) )
A. ppt will take place
B. ppt will not take place
c. solution will be saturated
D. none of the above
11
411An aqueous solution at room temperature is ( 0.1 M ) with respect to
ammonium chloride and ( 0.1 M ) with
respect to ( N H_{4} O Hleft(p K_{b}=5right), ) the ( p H )
of the solution is:
A . 7.5
B. 6.8
c. 6.5
D. 9.
11
412The rate law for a reaction between the
substances ( A ) and ( B ) is given by:
Rate ( =boldsymbol{K}[boldsymbol{A}]^{n}[boldsymbol{B}]^{m} . ) On doubling the
concentration of ( A ) and having concentration of ( B ) the ratio of new rate
law to the earlier rate of the reaction will
be as
( mathbf{A} cdot n-m )
B ( cdot 2^{(n-m)} )
c. ( frac{1}{2^{m+n}} )
D. ( m+n )
11
413Assertion
Osmotic pressure of ( 0.1 N ) urea solution
is less than that of ( 0.1 M ) NaCl
solution.
Reason
Osmotic pressure is not colligative property.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
414Assertion
On adding ( H_{2} S O_{4} ) to water, the
resulting aqueous solution get corrosive.
Reason
Hydronium ions are responsible for
corrosive action.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion.
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
415( boldsymbol{p} boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{N} boldsymbol{H}_{3} ) is ( boldsymbol{4} . boldsymbol{7} 4 ) and ( boldsymbol{p} boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{A}^{-}, boldsymbol{B}^{-} )
and ( C^{-} ) are 4,5 and 6 respectively.
Aqueous solution of ( 0.01 M ) has ( p H ) in
the increasing order.
A ( . N H_{4} A<N H_{4} B<N H_{4} C )
B. ( N H_{4} C<N H_{4} B<N H_{4} A )
C . ( N H_{4} C<N H_{4} A<N H_{4} B )
D. All have equal ( p H )
11
416Assertion: The solubility product of hydroxide of ( F e^{2+} ) is higher than that of
( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} )
Reason: The lattice energy of ( boldsymbol{F e}(boldsymbol{O} boldsymbol{H})_{2} )
is lower than that of ( F e(O H)_{3} )
A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion
B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
c. Assertion is true but Reason is false
D. Assertion is false but Reason is true
E. Both Assertion and Reason are false
11
417. 44 Assertion (A) Increasing order or acidity of hydrogen halides is
HF < HCI < HBr < HI.
Reason (R) While comparing acids formed by the elements belonging to
the same group of periodic table, H-A bond strength is a more
important factor in determining acidity of an acid than the polar nature
of the bond.
(a) Both A and R are true R is the correct explanation of A
(b) Both A and Rare true but is not the correct explanation of A
(c) A is true but R is false
(d) Both A and Rare false
11
418Species acting as Bronsted acid and
base is:
A. ( H S O_{4}^{-} )
в. ( N a_{2} C O_{3} )
c. ( N H_{3} )
D. ( O H^{-} )
11
419State which of the following solutions contain both molecules and ions?
A. ( C H_{3} ) СООН
в. ( N a_{2} C O_{3} )
c. oxalic acid
D. All of these
11
420For the reaction, ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) rightleftharpoons )
( 2 H I(g), ) the equilibrium constant ( K_{p} )
changes with:
A. total pressure
B. catalyst
C. the amounts of ( H_{2} ) and ( I_{2} ) present
D. temperature
11
421The pH of blood stream is maintained
by a proper balance of ( boldsymbol{H}_{2} boldsymbol{C O}_{3} ) and
( N a H C O_{3} ) concentration. What volume
of ( 5 M N a H C O_{3} ) solution should be
mixed with a ( 10 mathrm{mL} ) sample of blood
which is ( 2 M ) in ( H_{2} C O_{3} ) in order to
maintain its pH?
( mathbf{A} cdot 40 mathrm{mL} )
B . ( 38 mathrm{mL} )
c. ( 50 mathrm{mL} )
D. ( 78 mathrm{mL} )
11
422( C H_{3} C H_{2} O H ) on reaction with
bleaching powder forms:
A ( . C H C l_{3} )
в. ( C C l C H O )
c. ( C H_{2} ) ClCHO
D. ( C C l_{4} )
11
423Match the items in column-I with those
in column – II
begin{tabular}{lllll}
& Column I & & Column II \
& & & \
1. & Electric Fuse & A & Chemical Effect \
hline 2. & Relay & B & Electric Discharge \
3. & CFL & C & Magnetic effect \
4. & Button Cell & D & Heating Effect
end{tabular} Which of the following shows the correct
matching?
( A cdot 1-C, 2-B, 3-A, 4-D )
B. ( 1-B, 2-A, 3-C, 4-D )
c. ( 1- ) D, ( 2-c, 3-B, 4-A )
D. ( 1- ) D, ( 2-B, 3-C, 4-A )
11
424Show that for reaction ( A B(g) rightleftharpoons A(g)+ ) ( mathrm{B}(mathrm{g}), ) the total pressure at which ( mathrm{AB} ) is ( 50 % ) dissociated is numerically equal to
three times of ( boldsymbol{K}_{boldsymbol{p}} )
11
425The ( p H ) of ( 0.001 M C H_{3} C O O H ) is:
( A cdot 3 )
B. 1
c. ( 3-7 )
D.
11
426Q66. Calculate the pH of the resultant mixtures
(a) 10 mL of 0.2 M Ca (OH), + 25 mL of 0.1 M HCI
(b) 10 mL of 0.01 M H,SO, + 10 mL of 0.01 M Ca (OH),
(c) 10 mL of 0.1 MH,50, + 10 mL of 0.1 M KOH
10
:11:
11
427A buffer solution, ( 0.080 M ) in ( N a_{2} P O_{4} )
and ( 0.020 M ) in ( N a_{3} P O_{4} ) is prepared. The electrolytic oxidation of 1.0 mmol of
the organic compound ( R N H O H ) is carried out in ( 100 mathrm{m} L ) of the buffer. The
reaction is as follows:
( boldsymbol{R} boldsymbol{N} boldsymbol{H} boldsymbol{O} boldsymbol{H}+boldsymbol{H}_{2} boldsymbol{O} longrightarrow boldsymbol{R} boldsymbol{N} boldsymbol{O}_{2}+ )
( 4 H^{+}+4 e )
Calculate the approximate ( p H ) of the solution after the oxidation is complete.
A . 6.19
B. 7.81
c. 10.34
D. 12.45
11
428Q13. SO,2-is Bronsted base or acid and why?11
429Then equilibrium constant for the
reaction is:
For the following reactions, equilibrium constants are indicated on the arrow
[
begin{array}{l}
mathrm{H}_{3} mathrm{PO}_{4} stackrel{K_{1}}{Leftrightarrow} mathrm{H}^{+}+mathrm{H}_{2} mathrm{PO}_{4} \
mathrm{H}_{2} mathrm{PO}_{4}^{*} Leftrightarrow mathrm{H}^{*}+mathrm{HPO}_{4}^{-2} \
mathrm{HPO}_{4}^{-2} stackrel{K_{3}}{Leftrightarrow} mathrm{H}^{+}+mathrm{PO}_{4}^{-3}
end{array}
]
Then equilibrium constant for the reaction
[
mathrm{H}_{3} mathrm{PO}_{4} Leftrightarrow quad 3 mathrm{H}^{+}+mathrm{PO}_{4}^{3} text { will be }
]
( mathbf{A} cdot K_{1}+K_{2}+K_{3} )
B . ( sqrt{K_{1} K_{2} K_{3}} )
( mathbf{c} cdot K_{1} times K_{2} times K_{3} )
D. ( frac{1}{K_{1} K_{2} K_{3}} )
11
430The chemical formula of king of chemicals, sulphuric acid is :
A ( cdot H_{2} S_{2} O_{3} )
в. ( H_{2} S O_{3} )
c. ( H S O_{4} )
D. ( H_{2} S O_{4} )
11
431Ammonia is a weak base that reacts
with water according to the equation:
( N H_{3}(a q)+2 H_{2} O(l) quad rightleftharpoons )
( N H_{4}^{+}(a q)+O H^{-}(a q) )
Which of the following conditions will decrease the moles of ammonium in
water?
This question has multiple correct options
A. Addition of ( H C l )
B. Addition of ( N a O H )
c. Addtion of ( N H_{4} C l )
D. Addition of ( H_{2} O )
11
432For ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{-2}+mathbf{1 4} boldsymbol{H}^{+}+boldsymbol{6} boldsymbol{e}^{-} rightarrow )
( mathbf{2} boldsymbol{C r}^{+mathbf{3}}+mathbf{7 H}_{mathbf{2}} boldsymbol{O} ; quad boldsymbol{E}^{boldsymbol{o}}=mathbf{1 . 3 3} boldsymbol{V} )
At ( left[boldsymbol{C r}_{2} boldsymbol{O}_{7}^{-2}right]=mathbf{4 . 5} ) millimole, ( left[boldsymbol{C r}^{+3}right]= )
15 millimole, ( boldsymbol{E} ) is 1.067 V. The pH of the
solution is nearly equal to :
A . 3
B. 4
( c cdot 2 )
D. 5
11
433The conjugate acid of ( boldsymbol{O}^{-2} ) ion is:
A ( . O H^{-} )
B. ( O H^{+} )
c. ( H_{2} O )
D. ( H O_{2}^{-} )
11
434For the reaction ( boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons )
( boldsymbol{P C l}_{5}(boldsymbol{g}) ) the value of ( boldsymbol{K}_{c} ) at ( 250^{circ} boldsymbol{C} ) is 26
The value of ( boldsymbol{K}_{boldsymbol{p}} ) at this temperature will
be:
A . 0.61
B. 0.57
c. 0.83
D. 0.46
11
435The pH of a solution of hydrochloric acid is ( 4 . ) The molar concentration of this solution is:
A . 4.0
B. 0.4
c. 0.000
D. 0.04
11
436Two weak acids ( H A ) and ( H B ) have
same ( p H ) when their concentration
ratio is ( 3: 1 . ) The ratio of the
dissociation constants of ( H B ) and ( H A )
is
11
437An equimolar solution of ( N a N O_{2} ) and
( H N O_{2} ) can act as a:
A. strong reductant
B. strong oxidant
c. buffer solution
D. none of these
11
438In the reaction, ( C(s)+C O_{2}(g) leftrightharpoons )
( 2 C O(g), ) the equilibrium pressure is 12
atm. If ( 50 % ) of ( C O_{2} ) reacts, calculate ( K_{p} )
A. 1.6 atm
B. 0.16 atm
( c cdot 16 operatorname{atm} )
D. 160 atm
11
439Which of the following will not change the concentration of ammonia in the
equilibrium?
( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) ; Delta H= )
( -boldsymbol{x} boldsymbol{k} boldsymbol{J} )
A. increase of pressure
B. increase of temperature
c. decrease of volume
11
440For the reaction ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) )
if percentage dissociation of ( N_{2} O_{4} ) and
( 20 %, 45 %, 65 % ) and ( 80 % ) then the
sequence of observed vapour densities
will be:
A ( cdot d_{20}>d_{45}>d_{65}>d_{80} )
В. ( d_{80}>d_{65}>d_{45}>d_{20} )
C ( . d_{20}=d_{45}=d_{65}=d_{80} )
D ( cdotleft(d_{20}=d_{45}right)>left(d_{65}=d_{80}right) )
11
441Of the following solutions, the one that
is acidic is:
A ( cdot Z n S O_{4}(a q .) )
в. ( operatorname{NaAl}(O H)_{4}(text {аq.}) )
( mathbf{c} cdot operatorname{NaH} C O_{3}(a q) )
D ( cdot K N O_{3}(a q .) )
11
442Which change in the system will drive
equilibrium to the left in the following reaction?
( N_{2} O_{5}(g)=N O_{2}(g)+N O_{3}(g) )
A. Increase the volume
B. Increase the pressure
c. Decrease the amount of ( N O_{3} )
D. Increase the amount of ( N_{2} O_{5} )
11
443The ( p H ) of a buffer solution is ( 5 . p K a ) of
the acid present in it is 4. What is the ratio of acid and salt present in the solution?
A . 1:
B. 1:10
( c cdot 10: )
D. 1: 2
11
444Which has the highest pH?
A. ( C H_{3} ) СООК
в. ( N a_{2} C O_{3} )
c. ( N H_{4} C l )
D. ( operatorname{NaNO}_{3} )
11
445( N_{2(g)}+3 H_{2(g)} leftrightarrow 2 N H_{3(g)} ) If some ( H C l )
gas is passed into the reaction mixture at the equilibrium of this reaction,then:
A. Equilibrium position shifts towards left
B. Equilibrium position shifts towards right
c. concentration of ( H_{2} ) increases
D. The equilibrium position is not affected
11
446Which of the following acids is a weak
electrolyte?
A. ( H_{2} C O_{3} )
в. ( C H_{3} ) СООН
c. Both A and B
D. None of the above
11
447( boldsymbol{K}_{s p} ) of ( M boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2} ) is ( 1 times )
( mathbf{1 0}^{-mathbf{1 2}}, mathbf{0 . 0 1} boldsymbol{M} mathbf{M g} mathbf{C l}_{mathbf{2}} ) will
be precipitating at the limiting pH:
( A cdot 8 )
B. 9
( c cdot 10 )
D. 12
11
448For the equilibrium, ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) Leftrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) )
which of the following is true?
A. The pressure changes do not affect the equilibrium.
B. The amount of ice that melts is more, if the pressure on the system is increased
c. The amount of liquid that freezes is more, if the pressure on the system is increased.
D. At low pressure, the nature of equilibrium changes to forward direction
11
449What is the partial pressure (atm) of HI in the equilibrium mixture?
A . 6.385
в. 12.77
c. 40.768
D. 646.58
11
450Which of the following acids, listed with
their ionization constant at ( 25^{circ} C ), is the
strongest?
A . Nitrous acid ( left(H N O_{2}right) K_{i}=4.5 times 10^{-4} )
B. Formic acid ( left(H C H O_{2}right) K_{i}=1.8 times 10^{-4} )
C . Benzoic acid ( left(H C_{7} H_{5} O_{2}right) K_{i}=6.3 times 10^{-5} )
D. Acetic acid ( left(H C_{2} H_{3} O_{2}right) K_{i}=1.8 times 10^{-5} )
E . Hydrocyanic acid (H ( C N ) ) ( K_{i}=4.0 times 10^{-10} )
11
451( K_{h} ) values for
( boldsymbol{A} boldsymbol{r}(boldsymbol{g}), boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}), boldsymbol{H} boldsymbol{C} boldsymbol{H} boldsymbol{O}_{(boldsymbol{g})} ) and ( boldsymbol{C} boldsymbol{H}_{4}(boldsymbol{g}) )
are ( 40.39,1.67,1.83 times 10^{-5} ) and 0.413
respectively. The order of their increasing solubility is:
A. ( H C H O<C H_{4}<C O_{2}<A r )
в. ( H C H O<C O_{2}<C H_{4}<A r )
c. ( A r<C O_{2}<C H_{4}<H C H O )
D. ( A r<C H_{4}<C O_{2}<H C H O )
11
452Q11. State Ostwald’s dilution law.11
453For the reaction ( boldsymbol{P} boldsymbol{C l}_{5}_{5} rightleftharpoons boldsymbol{p} boldsymbol{C l}_{3(g)}+ )
( C l_{2(g)}, ) the forward reaction at constant
temperature is favoured by:
A. introducing an inert gas at constant volume
B . introducing ( C l_{2} ) at constant volume
C . introducing ( P C l_{5} ) at constant volume
D. reducing the volume of the container
11
454What is the ( H^{+} ) ion concentration in
ammonium acetate solution?
( left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{b}}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{v}}right. )
11
455What ( left(H_{3} O^{+}right) ) must be maintained in a
saturated ( H_{2} S ) solution to precipitate
( P b^{2+}, ) but not ( Z n^{2+} ) from a solution in
which each ion is present at a concentration of ( 0.01 M ? )
( left(K_{s p} H_{2} S=1.1 times 10^{-22} ) and right.
( boldsymbol{K}_{s p} Z boldsymbol{n} boldsymbol{S}=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{2 1}} mathbf{)} )
11
456( 0.16 g ) of ( N_{2} H_{4} ) are dissolved in water
and the total volume made up to
500 ( m L ). Calculate the percentage of
( N_{2} H_{4} ) that has reached with water at
this dilution. The ( K_{b} ) for ( N_{2} H_{4} ) is ( 4.0 times )
( mathbf{1 0}^{-6} boldsymbol{M} )
11
457Degree of ionisation does not depend
on:
A. nature of the solvent
B. nature of the electrolyte
c. dilution
D. molecular mass of the electrolyte
11
458The ( p K_{a} ) of acetylsalicylic acid (aspirin) is 3.5 The pH of gastric juice in human stomach is about ( 2-3 ) and the pH in
the same intestine is about ( 8 . ) Aspirin will be
A. Unionised in the small intestine and in the stomach
B. Completely ionised in the small intestine and in the stomach
c. lonised in the stomach and almost unionised in the samılı intestine
D. lonised in small intestine and almost unionised in the stomach
11
459Which of the following will function as
buffer?
This question has multiple correct options
A. ( N a C l+N a O H )
в. Borax + Boric acid
c. ( N a H_{2} P O_{4}+N a_{2} H P O_{4} )
D. ( N H_{4} C l+N H_{4} O H )
11
460According to Lewis concept, acid is:
A. proton donor
B. electron pair donor
C . electron pair acceptor
D. proton acceptor
11
461To which type of reaction, Le Chatelier’s principle can always be applied?
A . Reversible
B. Elementary
c. synthesis
D. Decomposition
E. Double Replacement
11
462A mixture of ( boldsymbol{H}_{2} boldsymbol{O} ) and solid ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} )
shaken to obtain saturated solution.
The solid is filtered and to ( 100 m L )
filtrate, ( 100 m L ) of ( 0.03 M N a B r ) is added, will a precipitate formed? ( boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g} boldsymbol{C l}=mathbf{1 0}^{-10}, boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g} boldsymbol{B r}=mathbf{5} times )
( mathbf{1 0}^{-13} )
11
463The equilibrium constant for the reaction ( 3 A+2 B rightleftharpoons C ) will be:
A ( cdot frac{[3 A][2 B]}{[C]} )
( ^{mathbf{B}} cdot frac{[A]^{3}[B]}{[C]} )
c. ( frac{[C]}{[A]^{3}[B]^{2}} )
D. ( frac{[C]}{[3 A][2 B]} )
11
464State whether the given statement is
true or false:

Bleaching powder contains about 50 % available chlorine.
A. True
B. False

11
465( Z n S rightarrow ) solubility in water ( =0.97 g K ) we
mixed 2 moles of ( Z nleft(N O_{3}right)_{2} ) is ( 5 L )
solution. Find new solubility of Zn?
11
466Q2. State the law of mass action?11
467A gaseous hypothetical chemical
equation ( 2 A rightleftharpoons 4 B+C ) is carried out
in a closed vessel. The concentration of ( B ) is found to be increase by ( 5 x )
( 10^{3} ) mol. ( L^{-1} . ) in 10 seconds. The rate of
appearance of ( B ) is:
A ( cdot 5 times 10^{2} mathrm{molL}^{-1} mathrm{sec}^{-1} )
B. ( 5 times 10^{5} mathrm{mol} mathrm{L}^{-1} mathrm{sec}^{-1} )
c. ( 6 times 10^{-5} mathrm{mol} mathrm{L}^{-1} mathrm{sec}^{-1} )
D. ( 4 times 10^{-4} mathrm{mol} mathrm{L}^{-1} mathrm{sec}^{-1} )
11
468( X e F_{6}+H_{2} O rightleftharpoons X e O F_{4}+2 H F )
constant ( =k_{1}, X e O_{4}+X e F_{6} rightleftharpoons )
( X e O F_{4}+X e O_{3} F_{2} ) constant ( =K_{2} )
Then equilibrium constant for the
following reaction will be:
( boldsymbol{X} boldsymbol{e} boldsymbol{O}_{4}+boldsymbol{2} boldsymbol{H} boldsymbol{F} rightleftharpoons boldsymbol{X} boldsymbol{e} boldsymbol{O}_{3} boldsymbol{F}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
A ( cdot frac{K_{2}}{K_{1}} )
в. ( K_{1}+K_{2} )
c. ( frac{K_{1}}{K_{2}} )
D. ( frac{K_{1}}{left(K_{2}right)^{2}} )
11
469R. 35 Calculate the volume of water required to dissolve 0.1 g lead (11)
chloride to get a saturated solution.
(Ksp of PbCl2 = 3.2x 10-8, atomic mass of Pb= 207u)
11
470Chemical equilibrium is dynamic
because:
A. the equilibrium attained quickly
B. the concentration of the reactants and products become same at equilibrium
c. the concentration of reactants and products are constant but different
D. both forward and backward reactions occur at all time with the same speedd
11
471( 40 % ) of ( P C l_{s} ) is not dissociated at
( 300^{0} C . ) The reaction is carried out in a
flask of 1 litre capacity. The value of ( boldsymbol{K}_{boldsymbol{c}} )
would be:
A. 3.2
B. 1.6
( c .2 .8 )
D. 0.9
11
472The equilibrium constant ( K ) for the
reaction ( : 2 H I(g) rightleftharpoons H_{2}(g)+I_{2}(g) ) at
room temperature is 2.85 and that at ( 698 K ) is ( 1.4 times ! 0^{-2} . ) This implies that
the forward reaction is:
A. exothermic
B. endothermic
c. slow
D. unpredictable
11
acid or base is added to it. Buffer
solutions have wide applications.
( 20.0 m L ) of ( 0.10 M ) of 1 -aminopropane is
titrated with ( 0.10 M ) of ( H C l . ) The ( p H ) at
the equivalence point is ( p simeq 6 ) and the appropriate acid-base indicator. is
Methyl red. (4.2-6.2) wright the right
Table 1.
Table 1: List of acid/base indicators
Common name ( quad ) Transition
range, ( p boldsymbol{H} quad ) color
change ser red-
orange Methyl orange
Methyl red ( 4.2^{-6.2} ) red-
yellow
Phenol red ( 6.8-8.2 ) yellow-
red ( y )
( r )
11
474In the reaction ( C_{(g)}+C O_{2(g)} rightleftharpoons 2 C O_{(g)} )
the equilibrium pressure is 12 atm. IF
( 50 % ) of ( C O_{2} ) reacts, ( K_{p} ) for the change
is:
A . 12 atm
B. 32 atm
( c .64 a t m )
D. 16 atm
11
475Which solution has the greatest percent
ionization?
( mathbf{A} cdot 0.10 mathrm{M} N H_{3}left(K_{b}=1.8 times 10^{-5}right) )
B. 0.25 M ( H N O_{2}left(K_{1}=4.5 times 10^{-4}right) )
C . 1.000 M HCOOH ( left(K_{a}=1.7 times 10^{-4}right) )
D . ( 2.000 mathrm{M} C H_{3} N H_{2}left(K_{b}=4.4 times 10^{-4}right) )
11
476( boldsymbol{B} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{s}) rightleftharpoons boldsymbol{B} boldsymbol{a}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{S} boldsymbol{O}_{4}^{2-}(boldsymbol{a} boldsymbol{q}) )
Whai is ( K_{s p} ) for above reaction?
( mathbf{A} cdotleft[B a^{2+}right]left[S O_{4}^{2-}right] )
( ^{mathbf{B} cdot} frac{left[B a^{2+}right]left[S O_{4}^{2-}right]}{B a S O_{4}} )
( ^{mathrm{c}} cdot frac{left[B a^{2+}right]left[S O_{4}^{2-}right]}{left[B a S O_{4}right]} )
D. None
11
477The ( p H ) of a solution which is ( 0.1 M ) sodium acetate and ( 0.01 M ) acetic acid
( left(p K_{a}=4.74right) ) would be:
A . 4.2
B. 5.1
( c .5 .74 )
D. None of these
11
478The solubility product of lead iodide is ( 1.4 times 10^{-8} . ) Calculate its molar
solubility in ( 0.1 M K I ) solution.
11
479The equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) for the reaction ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) is 4.5
What would be the average molar mass (in g/mol) of an equilibrium
mixture of ( N_{2} O_{4} ) and ( N O_{2} ) formed by
the dissociation of pure ( N_{2} O_{4} ) at a total
pressure of 2 atm?
( mathbf{A} cdot 69 )
в. 57.5
( c .80 .5 )
D. 85.5
11
480( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} rightleftharpoons boldsymbol{H}^{oplus}+boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{ominus} ; boldsymbol{K}_{a_{1}} )
( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4}^{ominus} rightleftharpoons boldsymbol{H}^{oplus}+boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} ; boldsymbol{K}_{a_{2}} )
( boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} rightleftharpoons boldsymbol{H}^{oplus}+boldsymbol{P} boldsymbol{O}_{4}^{3-} ; boldsymbol{K}_{a_{3}} )
Mark out the incorrect statements
This question has multiple correct options
( mathbf{A} cdot K_{a_{1}}>K_{a_{2}}>K_{a_{3}} )
B. ( _{p Hleft(H_{2} P O_{4}^{circ}right)=frac{p K_{a_{1}}+p K_{a_{2}}}{2}} )
C. Both ( H_{3} P O_{4} ) and ( H_{2} P O_{4}^{odot} ) are more acidic than ( H P O_{4}^{2} )
D. only ( H P O_{4}^{2-} ) is amphiprotic anion in the solution
11
481How many of the following reactions goes almost all the way to completion?
( N_{2}(g)+O_{2}(g) rightleftharpoons 2 N O(g) ; K_{c}=2.7 times )
( mathbf{1 0}^{-18} )
( mathbf{2} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{N} boldsymbol{O}_{2}(boldsymbol{g}) )
11
482At ( 1200^{circ} C, ) the following equilibrium is established between chlorine atoms &
molecule.
( boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{C l}(boldsymbol{g}) )
The composition of the equilibrium mixture may be determined by measuring the rate of effusion of the mixture through a pinhole. It is found
that at ( 1200^{circ} ) Cand 1 atm pressure the
mixture effuses 1.16 times as fast as
krypton effuses under the same condition.
Calculate the equilibrium constant ( boldsymbol{K}_{c} )
A ( .3 .1 times 10^{5} )
В . ( 6.3 times 10^{4} )
c. ( 12.6 times 10^{5} )
D. None of these
11
483If one-third of ( H I ) decomposes at a
particular temperature, ( boldsymbol{K}_{c} ) for the equilibrium is:
( boldsymbol{H} boldsymbol{I} rightleftharpoons boldsymbol{H}_{2}+boldsymbol{I}_{2} )
A . ( 1 / 16 )
B. ( 1 / 4 )
( c cdot 1 / 6 )
D. ( 1 / 2 )
11
484The standard Gibbs energy change at ( 300 K ) for the reaction ( 2 A rightleftharpoons B+C ) is
( 2494.2 J . ) At a given time, the composition of the reaction mixture is
( [boldsymbol{A}]=frac{1}{2},[boldsymbol{B}]=mathbf{2},[boldsymbol{C}]=frac{1}{2} . ) The reaction
proceeds in the:
( [boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} / boldsymbol{K} / boldsymbol{m o l}, boldsymbol{e}=mathbf{2 . 7 1 8}] )
A. Reverse direction because ( QK_{c} )
c. Reverse direction because ( Q>K_{c} )
D. Forward direction because ( Q<K_{c} )
11
485The thermal dissociation equilibrium of
( boldsymbol{C a C O}_{3}(s) ) is studied under different
conditions.
[
begin{array}{r}
boldsymbol{C a C O}_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+ \
boldsymbol{C O}_{2}(boldsymbol{g})
end{array}
]
For this equilibrium, the correct statement(s) is (are):
A. ( Delta H ) is dependent on ( T )
B. ( K ) is independent of the initial amount of ( C a C O_{3} )
C. ( K ) is dependent on the pressure of ( C O_{2} ) at a given ( T )
D. ( Delta H ) is independent of the catalyst, if any
11
486In the graph ( (1), A, B ) and ( C ) respectively
are:
( A cdot S O_{3}, S O_{2} ) and ( O_{2} )
B. ( S O_{3}, O_{2} ) and ( S O_{2} )
( c cdot S O_{2}, O_{2} ) and ( S O_{3} )
D. ( O_{2}, S O_{2} ) and ( S O_{3} )
11
487The molar solubility of ( mathrm{PbCl}_{2} ) in ( 0.20 mathrm{M} )
( mathrm{Pb}left(mathrm{NO}_{3}right)_{2} ) solution is:
( left(boldsymbol{K}_{boldsymbol{s} p} text { for } boldsymbol{P b C l}_{2}=mathbf{1 . 6} times mathbf{1 0}^{-mathbf{5}}right) )
A . ( 1.7 times 10^{-4} M )
В. ( 9.2 times 10^{-3} M )
c. ( 1.7 times 10^{-5} M )
D. ( 4.6 times 10^{-3} M )
E . ( 8.5 times 10^{-5} M )
11
488One litre of water contains ( 1.0 times 10^{-7} )
moles of ( boldsymbol{H}^{+} ) ions. The degree of
ionization of water is:
A ( cdot 1.8 times 10^{-9} % )
В. ( 0.8 times 10^{-9} % )
c. ( 3.6 times 10^{-9} % )
D. ( 3.6 times 10^{-7} % )
11
489An acid ( H A ) ionises as
( boldsymbol{H} boldsymbol{A} rightleftharpoons boldsymbol{H}^{+}+boldsymbol{A}^{-} )
The pH of ( 1.0 mathrm{M} ) solution is ( 5 . ) Its dissociation constant would be:
11
490Assertion
According to Bronsted Lowry theory ( B F_{3} )
is an acid.
Reason
( B F_{3} ) is an electron deficient compound.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
491Q73. The concentration of sulphide ion in 0.1 M HCl solution saturated with hydrogen sulphide is
1.0 10-19 M. IF 10 mL of this solution is added to 5 mL of 0.04 M solution of FeSO,, MnCI,
ZnCl, and Cdci, in which of these solutions precipitation will take place? Given K for Fes
= 6.3 x 10-18, MnS = 2.5 x 10-13, ZnS = 1.6 x 10-24 and CAS = 8.0 x 10-27
1
11
492Which of the following is an example of
weak electrolyte?
A ( cdot C H_{3} C O O H rightarrow C H_{3} C O O^{-}+H^{+} )
в. ( K O H rightarrow K^{+}+O H^{-} )
( mathrm{c} cdot A g N O_{3} rightarrow A g^{+}+N O_{3} )
D. all of the above
11
493Which of the following is not a Lewis acid?
A. Aluminum chloride
B. Ammonia
c. sulphur trioxide
D. cupric ion
11
494The equilibrium constants for the
reactions are:
[
begin{array}{l}
boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} stackrel{boldsymbol{K}_{1}}{rightleftharpoons} boldsymbol{H}^{+}+boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-} ; boldsymbol{K}_{mathbf{1}} \
boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-} frac{boldsymbol{K}_{2}}{rightleftharpoons} boldsymbol{H}^{+}+boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} ; boldsymbol{K}_{2} \
boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} stackrel{boldsymbol{K}_{3}}{rightleftharpoons} boldsymbol{H}^{+}+boldsymbol{P} boldsymbol{O}_{4}^{3-} ; boldsymbol{K}_{3}
end{array}
]
The equilibrium constant for
[
boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} rightleftharpoons mathbf{3} boldsymbol{H}^{+}+boldsymbol{P} boldsymbol{O}_{4}^{3-} text { will be: }
]
( A )
[
frac{K_{1}}{K_{2} times K_{3}}
]
В. ( K_{1} times K_{2} times K_{3} )
( c )
[
frac{K_{2}}{K_{1} times K_{3}}
]
D. ( K_{1}+K_{2}+K_{3} )
11
495( boldsymbol{K}_{boldsymbol{a}_{1}}, boldsymbol{K}_{boldsymbol{a}_{2}}, boldsymbol{K}_{boldsymbol{a}_{3}} ) values for ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} ) are
( 10^{-3}, 10^{-8}, 10^{-12} ) respectively. If
( boldsymbol{K}_{boldsymbol{w}}left(boldsymbol{H}_{2} boldsymbol{O}right)=mathbf{1 0}^{-14}, ) then
(i) What is dissociation constant of ( H P O_{4}^{2-} ? )
(ii) What is ( K_{b} ) of ( H P O_{4}^{2-} )
(iii) What is ( K_{b} ) of ( H_{2} P O_{4}^{2-} ) ?
(iv) What order of ( boldsymbol{K}_{boldsymbol{b}} ) of
( boldsymbol{P O}_{4}^{3-}left(boldsymbol{K}_{b_{3}}right), boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-}left(boldsymbol{K}_{b_{2}}right) ) and
( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-}left(boldsymbol{K}_{b_{1}}right) ? )
11
496( 9.2 mathrm{gm} ) of ( N_{2} O_{4}(g) ) is taken in a closed
one-litre vessel and heated till the
following equilibrium is reached
( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) )
At equilibrium ( 50 % ) of ( N_{2} O_{4}(g) ) is dissociated. What is the
equilibrium constant?
[in mole lit ( ^{-1} ) ] [M.wt. of ( N_{2} O_{4} ) is 92]
A. ( 0 . )
в. 0.2
( c cdot 0.4 )
D. 2
11
497Sodium bicarbonate is also known as:
A. washing soda
B. baking soda
c. glauber’s salt
D. lime soda
11
498Ammonia is basic in nature hence it
turns:
A . red litmus to blue
B. blue litmus to red
c. white litmus to red
D. white litmus to blue
11
499Consider the following statements
(a) The ( p H ) of a mixture containing
( 400 m L ) of ( 0.1 M H_{2} S O_{4} ) and ( 400 m L ) of
( 0.1 M N a O H ) will be approximately 1.3
(b) lonic product of water is temperature dependent
(c) A monobasic acid with ( boldsymbol{K}_{boldsymbol{a}}=mathbf{1 0}^{-5} )
has a ( p H=5 . ) The degree of
dissociation of this acid is ( 50 % )
(d) The Le Chatelier’s principle is not applicable to common-ion effect.
The correct statement are :
A ( cdot(a),(b) ) and ( (d) )
B. (a), (b) and (c)
c. (a) and (b)
D. (b) and (c)
11
500( 2 S O_{2}(g)+O_{2}(g) leftrightharpoons 2 S O_{3}(g) )
Given that the equilirbium constant for
the reaction above has a value of 278 at
a particular temperature, what is the value of equilibrium constant for the following reaction at same temperature?
( boldsymbol{S O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) )
A ( cdot 1.3 times 10^{-5} )
B . ( 1.8 times 10^{-3} )
c. ( 3.6 times 10^{-3} )
D. ( 6 times 10^{-2} )
11
501The gas released when baking soda is mixed with vinegar, is:
A. ( C O )
в. ( C O_{2} )
c. ( C H_{4} )
D. ( O_{2} )
11
502If the salts ( M_{2} X, Q Y_{2} ) and ( P Z_{3} ) have
the same solubilities,their ( boldsymbol{K}_{s p} ) values are related as ( -(S<1) )
A ( cdot K_{s p}left(M_{2} Xright)=K_{s p}left(Q Y_{2}right)K_{s p}left(Q Y_{2}right)=K_{s p}left(P Z_{3}right) )
C. ( K_{s p}left(M_{2} Xright)=K_{s p}left(Q Y_{2}right)>K_{s p}left(P Z_{3}right) )
D. ( K_{s p}left(M_{2} Xright)>K_{s p}left(Q Y_{2}right)>K_{s p}left(P Z_{3}right. )
11
503The equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) for the
following reaction at ( 191^{circ} mathrm{C} ) is 1.24
What is ( boldsymbol{K}_{c} ) ? ( B(s)+frac{3}{2} F_{2}(g) rightleftharpoons B F_{3}(g) )
A . 6.7
B. 0.61
c. 8.30
D. 7.6
11
504Fill in the blanks:
¡. ( quad ) taste is a
characteristic property of all acids in
aqueous solution.
ii. Acids react with some metals to
produce
iii. Because aqueous acid solutions conduct electricity, they are identified
as
iv. Acids react with bases to produce a
and water.
v. Acids turn
different colours.
11
505The ( p H ) of the solution cantaining
( mathbf{0 . 1} boldsymbol{M} boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} & mathbf{0 . 1} boldsymbol{M} boldsymbol{H} boldsymbol{C O O H} mathbf{~ i s : ~} )
( left[boldsymbol{K}_{s} text { of } boldsymbol{H} boldsymbol{C O O H} text { is } mathbf{1 . 8} times mathbf{1 0}^{-mathbf{1 4}}right] )
A . ( 0 . )
B.
( c cdot 2 )
D. 0.2
11
506Which of the following has a very high
( boldsymbol{K}_{boldsymbol{a}} ? )
A. Bronsted acid
B. Bronsted base
c. Strong acid
D. weak base
11
507For the reaction ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C} ) at
equilibrium ( [boldsymbol{C}]=mathbf{1 . 4} boldsymbol{M} cdot[boldsymbol{A}]_{o}= )
( mathbf{1} boldsymbol{M},[boldsymbol{B}]_{o}=mathbf{2} boldsymbol{M},[boldsymbol{C}]_{o}=mathbf{3} M . ) The value
of ( K_{c} ) is:
(Given: volume =1 litre, [ ] ( _{o} ) is initial concentration)
A .0 .084
B. 8.4
( c cdot 48 )
D. None of these.
11
508If the pH of pure water is ( 7, ) then the
hydrogen ion concentration, ( left[boldsymbol{H}^{+}right] ) in mol
( mathbf{L}^{-1} ) will be:
A ( cdot 10^{-7} )
7
B. 0
( c cdot 7 )
D. ( 10^{+7} )
11
509Q42. The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.11
510lonisation constant of ( C H_{3} C O O H ) is
( 1.7 times 10^{-5} ) and concentration of ( H^{+} )
ions is ( 3.4 times 10^{-4} . ) Then find out initia
concentration of ( boldsymbol{C H}_{3} ) COOH
molecules:
A ( .3 .4 times 10^{-4} )
B . ( 3.4 times 10^{-3} )
c. ( 6.8 times 10^{-4} )
D. ( 6.8 times 10^{-3} )
11
511Q4. (a) In the reaction A + B +C+D, what will happen to the equilibrium if concentration of
A is increased?
(b) The equilibrium constant for a reaction is 2 x 10-23 at 25°C and 2 x 10-2 at 50°C. Is the
reaction endothermic or exothermic?
(c) Mention at least three ways by which the concentration of so, can be increased in the
following reaction in a state of equilibrium.
.
11
512A 0.02 M solution of pyridinium
hydrochloride has ( p H=3.44 . ) Calculate
the ionization constant of pyridine.
11
513m
illoride
ced in terms of bult
13. Effectiveness of a buffer is measured in
capacity (). Select correct statement
capacity
d[Base]
(a) B =
| d[pH]
d[Base]
(6) B=
-d[AH]
(c) B is maximum for an acidic buffer at pH = pk
(d) If pH = pK, +1, then it is most effective range for
a buffer
11
514Which of the following salts has the
greatest molar solubility in pure water?
A ( cdot C a C O_{3} ; K_{s p}=8.7 times 10^{-9} )
B. ( C u S ; K_{s p}=8.5 times 10^{-45} )
C ( cdot A g_{2} C O_{3} ; K_{s p}=6.2 times 10^{-12} )
D. ( P bleft(I O_{3}right)_{2} ; K_{s p}=2.6 times 10^{-13} )
11
515Will ( C a F_{2} ) be precipitated?
A. Yes
B. No
c. Data insufficient
D. None of these
11
516The correct order of pH is
A. Lemon juice < water water> Milk of Magnesia
C. Water > lemon juice > milk of Magnesia
D. Milk of Magnesia > lemon juice > water
11
517Calculate the pH of a ( 0.033 M )
ammonia solution, if ( 0.033 M N H_{4} C l ) is introduced in this solution at the
same temperature. ( left(k_{b} text { for } N H_{3}=right. ) ( left.1.77 times 10^{-5}right) )
11
518( 20 m L ) of ( 0.1 N ) acetic acid is mixed
with ( 10 m L ) of ( 0.1 N ) solution of ( N a O H )
The ( p H ) of the resulting solution is :
( left[text { Given }: p K_{a} text { of acetic acid is } 4.74right] )
A . 3.74
в. 4.74
( c .5 .74 )
D. 6.74
11
519For the reaction, ( boldsymbol{A B}(boldsymbol{g}) rightleftharpoons boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}), boldsymbol{A B} ) is ( boldsymbol{3} boldsymbol{3} % )
dissociated at a total pressure of ( boldsymbol{P} )
Therefore, ( P ) is related to ( K_{p} ) by one of
the following option:
A ( cdot P=K_{p} )
В. ( P=3 K_{p} )
( mathbf{c} cdot P=4 K_{p} )
D. ( P=8 K_{p} )
11
520The process in which metal surface is made inactive is called:
A. passivation
B. galvanizing
c. corrosion
D. pickling
11
521A solution contains ( 0.1 M C l^{-} ) and
( mathbf{0 . 0 0 1} boldsymbol{M} boldsymbol{C r} boldsymbol{O}_{4}^{2-} . ) If solid ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) is
will precipitate first, ( A g C l ) or ( A g_{2} C r O_{4} )
? Assume that the addition causes no
change in volume. Given ( boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g} boldsymbol{C l}=mathbf{1 . 7} times mathbf{1 0}^{-mathbf{1 0}} boldsymbol{M}^{mathbf{2}} )
( boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4}=mathbf{1 . 7 9} times mathbf{1 0}^{-mathbf{1 2}} boldsymbol{M}^{mathbf{3}} )
What percent of ( C l^{-} ) remains in the
solution when ( C r O_{4}^{2-} ) starts precipitating?
11
522In the reaction ( boldsymbol{F e}(boldsymbol{O} boldsymbol{H})_{3}, boldsymbol{F} boldsymbol{e}_{boldsymbol{a} boldsymbol{q}}^{3+}+ )
( 3 O H_{a q}^{-}, ) if the concentration of ( O H^{-} ) is decreased by ( frac{1}{4} ) times then the equilibrium concentration of ( boldsymbol{F} boldsymbol{e}^{mathbf{3}+} )
increased by how many times??
11
5230.23 The aqueous solution of sugar does not conduct electricity. However
when sodium chloride is added to water, it conducts electricity. How will
you explain this statement on the basis of ionisation and how is it
affected by concentration of sodium chloride?
11
524The equilibrium constant for the
following reaction is ( 64 . H_{2} O(l)+ )
( boldsymbol{C O}(boldsymbol{g}) leftrightharpoons boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) . ) If the rate
constant for the forward reaction is 160
the rate constant for the backward
reaction is:
A . 0.4
B . 2.
c. 6.2
D. 10.24
11
525Which of the following is not a conjugate acid-base pair?
( mathbf{A} cdot H P O_{3}^{2-}, P O_{3}^{3-} )
B . ( H_{2} P O_{4}^{-}, H P O_{4}^{2-} )
c. ( H_{2} P O_{4}^{-}, H_{3} P O_{4} )
D. ( H_{2} P O_{4}^{-}, P O_{3}^{3-} )
11
526If two gases ( A B_{2} ) and ( B_{2} C ) are mixed
established
( boldsymbol{A B}_{2}(boldsymbol{g})+boldsymbol{B}_{2} boldsymbol{C}(boldsymbol{g}) rightarrow boldsymbol{A} boldsymbol{B}_{3}(boldsymbol{g})+boldsymbol{B C}(boldsymbol{g}) )
( boldsymbol{B C}(boldsymbol{g})+boldsymbol{B}_{2} boldsymbol{C}(boldsymbol{g}) rightarrow boldsymbol{B}_{3} boldsymbol{C}_{2}(boldsymbol{g}) )
If the reaction is started only with ( A B_{2} )
with ( B_{2} C, ) then which of the following is
necessarily true at equilibrium:
This question has multiple correct options
( mathbf{A} cdotleft[A B_{3}right]_{e q}=[B C]_{e q} )
( mathbf{B} cdotleft[A B_{2}right]_{e q}=left[B_{2} Cright]_{e q} )
( mathbf{c} cdotleft[A B_{3}right]_{e q}>left[B_{3} C_{2}right]_{e q} )
( mathbf{D} cdotleft[A B_{3}right]_{e q}>[B C]_{e q} )
11
527( H_{3} P O_{4} ) is a tribasic acid with
( boldsymbol{p} boldsymbol{K}_{a_{1}}, boldsymbol{p} boldsymbol{K}_{a_{2}} ) and ( boldsymbol{p} boldsymbol{K}_{a_{3}} boldsymbol{2} .12, boldsymbol{7} .21 ) and
( 12.32, ) respectively. It is used in fertiliser productions and its various salts are used in food, detergent, toothpaste, and in metal treatment.
Small quantities of ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} ) are used in imparting the sour or tart taste to soft drinkes, such as Coca Cola, and beers
in which ( H_{3} P O_{4} ) is present ( 0.05 % ) by weight (density ( left.=1.0 g m L^{-1}right) ) ( mathbf{1 0}^{-3} boldsymbol{M} boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4}(boldsymbol{p} boldsymbol{H}=mathbf{7}) ) is used in
fertilisers as an aqueous soil digesting. Plants can absorb zinc in water soluble
form only. Zinc phosphate is the source of zinc and ( P O_{2}^{3-} ) ions in the soil. ( K_{s p} ) of zonic phosphate ( =9.1 times 10^{-33}left[Z n^{2+}right] ) ion in the soil is:
A ( .2 .9 times 10^{-11} mathrm{M} )
В. ( 4.0 times 10^{-10} M )
c. ( 3.0 times 10^{-6} M )
D. ( 9.1 times 10^{-5} M )
11
528A buffer solution of ( p H=9 ) can be
prepared by mixing:
A. ( C H_{3} C O O N a ) and ( C H_{3} C O O O H )
B. ( N a C l ) and ( N a O H )
c. ( N H_{4} C l ) and ( N H_{4} O H )
D. ( K H_{2} P O_{4} ) and ( K_{2} H P O_{4} )
11
529The pH of a solution of ( B(O H)_{2} ) is 10.6
Calculate the solubility and solubility product of hydroxide.
11
530For the equilibrium reaction
( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+boldsymbol{C O}_{2}(boldsymbol{g}) . ) The
addition of more ( C a C O_{3}(s) ) causes?
A. The decrease in the concentration of ( C O_{2}(g) )
B. The increase in the concentration of ( C O_{2}(g) )
C. No change in the concentration of ( C O_{2}(g) )
D. Increase in the concentration of ( C a O(s) )
11
531( boldsymbol{C O}_{2}+boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{X} )
( boldsymbol{X}+boldsymbol{N} boldsymbol{a} boldsymbol{C l} rightarrow boldsymbol{Y}+boldsymbol{N} boldsymbol{H}_{4} boldsymbol{C l} )
‘Y’ in the above reaction is:
( mathbf{A} cdot N a_{2} C O_{3} )
в. ( left(N H_{4}right)_{2} C O_{3} )
c. ( N H_{4} H C O_{3} )
D. ( N a H C O_{3} )
11
532Assertion
At ( 25^{circ} C ), the pH of ( 10^{-8} M ) HClis 8
Reason
pH of acidic solution is always below 7
( operatorname{at} 25^{circ} C )
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but the Reason is correct
11
533The equilibrium state can be attained from both sides of the chemical
reaction.
A. True
B. False
11
534In an experiment starting with 1 mole of ethyl of alcohol, 1 mole of acetic acid
and 1 mole of water at ( 100^{circ} mathrm{C} ), the
equilibrium mixture on analysis shows that ( 54.3 % ) of the acid is esterified.
Calculate the equilibrium constant of this reaction.
11
535In the reaction, ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) rightleftharpoons )
( 2 H I(g) ) the concentration of ( H_{2}, I_{2} ) and
( H I ) at equilibrium are 8.0,3.0 and 28 moles per litre respectively. What will be the equilibrium constant?
( A cdot 30.61 )
B. 32.66
c. 29.40
D. 20.90
11
536The percentage hydrolysis in ( 0.003 M )
aqueous solution of ( N a O C Nleft(K_{a} ) for right.
( left.boldsymbol{H} boldsymbol{O} boldsymbol{C} boldsymbol{N} text { is } boldsymbol{3} boldsymbol{3} boldsymbol{3} times mathbf{1 0}^{-4} boldsymbol{M}right) ) is:
A . ( 0.1 % )
B. ( 0.01 % )
( c .0 .5 % )
D. ( 0.8 % )
11
537Bleaching powder gives smell of chlorine because it:
A . is unstable
B. gives chlorine on exposure to atmosphere
c. is a mixture of chlorine and slaked lime
D. contains excess of chlorine
11
538Q8. Write conjugate acid and conjugate base of H,O?
Ana Caninote :: In
11
539Q1. What is meant by equilibrium?
11
11
540Calculate the ratio of pH of a solution
containing 1 mol. of ( C H_{3} C O O N a+ )
1 mol of HCl per litre and of
other solution containing 1 mol of
( boldsymbol{C H}_{3} boldsymbol{C O O N a +} mathbf{1 m o l} ) of ( boldsymbol{C H}_{3} boldsymbol{C O O H} )
per litre.
11
541What would be the pH of an aqueous
solution of ( 1 N ) tribasic acid?
A. 3
B.
( c cdot 0 )
D. 1.5
11
542Consider the two gaseous equilibria involving ( S O_{2} ) and the corresponding equilibrium constants at ( 298 mathrm{K} )
( boldsymbol{S O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) Leftrightarrow boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ; boldsymbol{K}_{1} )
( 2 S O_{3}(g) Leftrightarrow 2 S O_{2}(g)+O_{2}(g) ; K_{2} )
The values of the equilibrium constants are related by:
A ( cdot K_{1}=K_{2} )
в. ( K_{2}=K_{1}^{2} )
c. ( _{K_{2}=frac{1}{K_{1}^{2}}} )
D. ( _{K_{2}}=frac{1}{K_{1}} )
11
543A reaction system in equilibrium
according to reaction ( 2 S O_{2}(g)+ )
( O_{2}(g) rightarrow 2 S O_{3}(g)(k=5) ) in one litre
vessel at a given temperature was
found to be 0.12 mole each of ( S O_{2} ) and
( boldsymbol{S} boldsymbol{O}_{3} ) and 5 mole of of ( boldsymbol{O}_{2} ) must be added
to this vessel to order that at
equilibrium ( 20 % ) of ( S O_{2} ) is oxidized to
( S O_{3} . ) Find out the mass of oxygen formed?
A. ( 0.41245 mathrm{g} )
B. ( 11.6 g )
c. ( 1.6 g )
D. None of these.
11
544( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g)+ ) heat
For the reaction above, what is the effect
on the equilibrium position when the pressure is decreased?
A. Increased production of products
B. Increased production of reactants
c. Fluctuations in the amounts of reactants and products
D. No impact on the equilibrium
E. Cannot be determined
11
545( A l F_{3} ) is soluble in ( H F ) only in presence
of ( K F ). It is due to the formation of :
A. ( A l H_{3} )
B . ( Kleft[A l F_{3} Hright] )
c. ( K_{3}left[A l F_{3} H_{3}right] )
D. ( K_{3}left[A l F_{6}right] )
11
546If the ( p H ) of a solution is ( 8, ) its ( left[H^{+}right] ) is:
A ( cdot log 10^{-8} )
B . ( 10^{6} )
( c cdot 10^{-8} )
D. 8
11
547For a gaseous phase reaction ( boldsymbol{A}+ ) ( mathbf{2} boldsymbol{B} rightleftharpoons boldsymbol{A} boldsymbol{B}_{2}, boldsymbol{K}_{C}=mathbf{0 . 3 4 7 5} boldsymbol{L}^{2} boldsymbol{m o l} boldsymbol{e}^{-mathbf{2}} mathbf{a} )
( 200^{circ} mathrm{C} ). When 2 moles of ( B ) are mixed
with one mole of ( A ), what total pressure
is required to convert ( 60 % ) of ( A ) in ( A B_{2} ) ?
A ( . P=1.8 a t m )
B. ( P=63 ) atm
c. ( P=181.5 ) atm
( D . P=34 a t m )
11
548For a reversible chemical reaction
where the forward process is
exothermic, which of the following
statements is correct?
A. The backward reaction has higher activation energy than the forward reaction
B. The backward and the forward processes have the same activation energy
C. The backward reaction has lower activation energy
D. No activation energy is required at all since energy is liberated in the process
11
549If equal concentrations of products and reactants are mixed, then which of the following reactions will proceed to the right and which will proceed to the left?
( (A) H_{2} S O_{4}(a q)+N H_{3}(a q) rightleftharpoons )
( N H_{4}^{+}(a q)+H S O_{4}^{-}(a q) )
(B) ( boldsymbol{H} boldsymbol{C O}_{3}^{-}(boldsymbol{a q})+boldsymbol{S O}_{4}^{2-}(boldsymbol{a q}) rightleftharpoons )
( boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{C} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q}) )
11
550Given ( 2 N O_{(g)}+O_{2(g)} rightarrow 2 N O_{2(g)} ; ) rate
( =mathbf{k}[boldsymbol{N} boldsymbol{O}]^{2}left[boldsymbol{O}_{2}right]^{1} . ) By how many times does
the rate of the reaction change when the volume of the reaction vessel is reduced
to ( 1 / 3 ) rd of its original volume? Will there be any change in the order of the reaction?
11
551LUL
CICLO LO TOLLIC PIULUICIDE
Q19. A sample of pure PCI was introduced into an evacuated vessel at 473 K. After equilibrium
was reached, the concentration of PCI, was found to be 0.5 x 10-1 mol L-1. If K is 8.3 x 10″,
what are the concentrations of PCI, and Cl, at equilibrium?
11
552f pressure increases then its effect on given equilibrium
( boldsymbol{C}(s)+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{O}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) )
It is shifted in:
A. forward direction
B. backward direction
c. no effect
D. none of these
11
553A buffer solution is made up of acetic
acid ( left[boldsymbol{p} boldsymbol{K}_{boldsymbol{a}}=mathbf{5}right] ) having conc. ( =mathbf{1 . 5} boldsymbol{M} )
and sodium acetate having conc. ( = )
( 0.15 M . ) What is the number of ( O H^{-} )
ions present in 1 litre solution?
В. ( 10^{-4} M )
( mathrm{c} cdot 10^{-3} M )
D. ( 10^{-6} M )
11
554Addition of water to ( boldsymbol{X} ) solution will not
change concentration of ( boldsymbol{H}_{3} boldsymbol{O}^{+} . boldsymbol{X} ) is:
A. chemical pH indicator
B. acid/base buffer
c. anhydrous solution
D. hypotonic solution
E. supersaturated solution
11
555Assertion: Addition of ( N H_{4} O H ) to
an aqueous solution of ( B a C l_{2} ) in the
presence of excess ( N H_{4} C l ) precipitates
( boldsymbol{B} boldsymbol{a}(boldsymbol{O} boldsymbol{H})_{2} )

Reason: ( boldsymbol{B a}(boldsymbol{O H})_{2} ) is soluble in water.
A. Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
c. Assertion is correct but Reason is not correct
D. Assertion is not correct but Reason is correct
E. Both Assertion and Reason are not correct

11
556Which of the following statements
relationships is correct?
( mathbf{A} cdot K_{P}=K_{C} ) for ( N_{2}+O_{2} rightleftharpoons 2 N O )
B. ( Q_{P}>K_{C} ) corresponds to backward reaction
C ( . K_{P} ) is not defined for ( C H_{3} C O O C H_{3}+H_{2} O rightleftharpoons )
( C H_{3} C O O H+C H_{3} O H )
D. ( K_{s p}=4 s^{-1} ) (for salt like ( C a F_{2} ) ) is applicable even in an ( H F ) solution
11
557Assertion
( boldsymbol{I}_{2}+boldsymbol{I}^{-} longrightarrow boldsymbol{I}_{boldsymbol{3}} )
In above reaction, ( boldsymbol{I}_{2} ) is Lewis base.
Reason

Electron pair acceptor is Lewis base.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect

11
558On increasing temperature, the equilibrium constant of exothermic and endothermic reactions
and ( ——- ) respectively:
A. increases and decreases
B. decreases and increases
c. increases and increases
D. decreases and decreases
11
559Q59. The ionization constant of propanoic acid is 1.32 x 10-6. Calculate the degree of ionization of
the acid in its 0.05 M solution and also its pH. What will be its degree of ionization if the
solution is 0.01 M HCl also?
Be the formula
11
560A weak mono acidic base is ( 5 % ) ionized
in ( 0.01 M ) solution. The hydroxide ion
concentration in the solution is:
A. ( 5 times 10^{-2} )
В. ( 5 times 10^{-4} )
c. ( 5 times 10^{-10} )
D. ( 2 times 10^{-11} )
11
561For a given exothermic reaction ( boldsymbol{K}_{boldsymbol{p}} ) and ( K_{p}^{prime} ) are the equilibrium constants at
temperature ( T_{1} ) and ( T_{2} ) respectively. Assuming that heat of reaction is constant in temperature range between
183. ( T_{1} ) and ( T_{2} ) it is readily observed
that:
( mathbf{A} cdot K_{p}=K_{p}^{prime} )
B . ( K_{p}=1 / K_{p}^{prime} )
( mathbf{c} cdot K_{p}>K_{p}^{prime} )
D. ( K_{p}<K_{p}^{prime} )
11
562Which of the following solution cannot act as a buffer?
A. ( N a H_{2} P O_{4}+H_{3} P O_{4} )
в. ( C H_{3} ) СООН ( +C H_{3} ) СОО Na
c. ( H C l+N H_{4} C l )
D. ( H_{3} P O_{4}+N a_{2} H P O_{4} )
11
563Which of the following is an organic acid?
A. Sulphurous acid
B. Nitric acid
c. Hydrochloric acid
D. Formic acid
11
564For the reaction
[
boldsymbol{P C l}_{3(g)}+boldsymbol{C l}_{2(g)} rightleftharpoons boldsymbol{P} boldsymbol{C l}_{5(g)}
]
the value of ( boldsymbol{K}_{c} ) at ( 250^{circ} mathrm{C} ) is ( 26 . ) The
value of ( K_{p} ) a this temperature will be
A . 0.61
B. 0.57
c. 0.83
D. 0.46
11
565When sulphur in the form of ( S_{8} ) is
heated at ( 900 K ) and constant volume,
the initial pressure of 1 atm increases
by ( 27 % ) at equilibrium. This is because
of conversion of some ( S_{8} ) to ( S_{2} ). Find the
value of the equilibrium constant for this reaction.
11
566Le Chatelier’s principle is applicable to what equilibrium.
A. Physical equilibrium.
B. Chemical equilibrium.
c. Both equilibrium.
D. None of these
11
567Match List-I with List-II.11
568If the pressure of ( N_{2} / H_{2} ) mixture in a
closed apparatus is 100 atm and ( 20 % ) of the mixture reacts,then the pressure at same temperature would be:
A. 100
B. 90
( c cdot 85 )
( D cdot 80 )
11
569Ethylene dibromide ( left(C_{2} H_{4} B r_{2}right) ) and
1, 2 – dibromopropane ( left(C_{3} H_{6} B r_{2}right) )
forms a series of ideal solution over the
whole range of composition. At ( 85^{circ} C )
the vapour pressure of these pure liquids are are ( 183 mathrm{mmHg} ) and 127 mm ( H g ) respectively. 10gm of ethylene dibromide is
dissolved in ( 80 g m ) of ( 1,2- ) dibromo – propane. Calculate the
partial pressures of each components and the total pressure of the solution at
( 85^{circ} C )
Calculate the composition of vapour in equilibrium with the above and express as mole fraction of ethylene dibromide.
11
570( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+boldsymbol{C O}_{2}(boldsymbol{g}), boldsymbol{K}= )
( 10^{-9} ) at ( 300 K . ) The value of ( p_{c o_{2}} ) is ( 10^{-x} )
( x ) is
11
571Assertion
A substance that can either act as an
acid or a base is called ampholyte.
Reason
Bisulphide ion ( left(boldsymbol{H} boldsymbol{S}^{-}right) ) and bicarbonate
ion ( left(H C O_{3}^{-}right) ) are ampholytes.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
572Which of the following is a weak acid?
A. Acetic acid
B. Formic acid
c. Carbonic acid
D. All of the above
11
573Which of the following is true about the
reaction quotient?
A. It relates the ratio of the concentrations of products to reactants once the reaction has reached chemical equilibrium.
B. It is always equal to the equilibrium constant.
C. It can never be equal to the equilibrium constant.
D. It relates the concentrations of products to reactants at any point in time.
E. None of these answers are correct
11
574The correct relationship between free energy change in a reaction and the corresponding equilibrium constant ( boldsymbol{K} )
is:
A ( .-Delta G^{circ}= ) RTin ( K )
в. ( Delta G= ) RT in ( K )
c. ( -Delta G=R T ) in ( K )
D. ( Delta G^{circ}=R T ) in ( K )
11
575Starting with sodium chloride how would you proceed to prepare (i) sodium metal,
(ii) sodium hydroxide,
(iii) sodium peroxide,
(iv) sodium
carbonate?
11
576In a vessel containing ( S O_{3}, S O_{2} ) and ( O_{2} )
at equilibrium, some helium gas is introduced so that total pressure
increases while temperature and volume remain the same. According to Le Chatelier’s principle the dissociation
of ( boldsymbol{S O}_{3} )
A. increases
B. decreases
c. remains unaltered
D. changes unpredictably
11
577( mathrm{HX} ) is a weak acid ( left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1 0}^{-mathbf{5}}right) . ) It forms
a salt ( mathrm{NaX}(0.1 mathrm{M}) ) on reacting with caustic soda. The degree of hydrolysis of NaX is:
A . 0.01 %
B. 0.0001 %
c. ( 0.1 % )
D. 0.5 %
11
578Compare the concentrations of each of the species ( N a^{+}, H^{+} ) and ( C N ) in the
solution.
A ( cdot N a^{+}>O H^{-}>C N^{-} )
В. ( C N^{-}>O H^{-}>N a^{+} )
c. ( N a^{+}>C N^{-}>O H^{-} )
D. ( O H^{-}>C N^{-}>N a^{+} )
11
579Q7. How does common ion affect the solubility of electrolyte?11
580Which of the following reactions
proceed at low pressure
( mathbf{A} cdot N_{2}+3 H_{2} rightleftharpoons 2 N H_{3} )
( mathbf{B} cdot H_{2}+I_{2} rightleftharpoons 2 H I )
( mathbf{c} cdot P C l_{5} rightleftharpoons P C l_{3}+C l_{2} )
D. ( N_{2}+O_{2} rightleftharpoons 2 N O )
11
581For a gaseous phase reaction, ( boldsymbol{A}+ ) ( mathbf{2} boldsymbol{B} rightleftharpoons boldsymbol{A} boldsymbol{B}_{2} boldsymbol{K}_{C}=mathbf{0 . 3 4 7 5} ) litre ( ^{2} boldsymbol{m o l}^{-2} )
at ( 200^{circ} mathrm{C} ). When 2 mole of ( B ) are mixed
with one mole of ( A ). What total pressure
is required to convert ( 60 % ) of ( A ) in ( A B_{2} ) ?
11
582Which of the following statement is
correct regarding container B?
Container ( (mathbf{A}) )

Container
( (mathbf{B}) )
A. Water will migrate from Glass (i) to Glass (ii) and no equilibrium will establish
B. Water will migrate from Glass (i) to Glass (ii) and equilibrium will establish after some time
c. Water will not migrate to any side
D. None of these

11
583What is the ( p H ) of dil.HCl solution
with concentration ( 10^{-8} ) mol ( / L ) ?
( A cdot 7 )
B. 8
c. 6.98
D. 10
11
5840.6 mole of ( N H_{3} ) in a reaction vessel of
( 2 d m^{3} ) capacity was brought to
equilibrium. The vessel was then found
to contain 0.15 mole of ( H_{2} ) formed by
the reaction
( mathbf{2} N boldsymbol{H}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{N}_{2}(boldsymbol{g})+mathbf{3} boldsymbol{H}_{2}(boldsymbol{g}) )
Which of the following statements is
true?
A. 0.15 mole of the original ( N H_{3} ) had dissociated at equilibrium
B. 0.55 mole of ammonia is left in the vessel
C . At equilibrium the vessel contained 0.45 mole of ( N_{2} )
D. The concentration of ( N H_{3} ) at equilibrium is 0.25 mole per ( d m^{3} )
11
585( boldsymbol{A}_{boldsymbol{3}(boldsymbol{g})} rightleftharpoons mathbf{3} boldsymbol{A}_{(boldsymbol{g})} )
In the above reaction, the initial moles
of ( A_{3} ) is “a”. If ( alpha ) is degree of
dissociation of ( A_{3} ). The total number of
moles at equilibrium will be:
A ( cdot a-frac{a alpha}{3} )
B. ( frac{a}{3}-alpha )
c. ( left(frac{a-a alpha}{2}right) )
D. None of these
11
586( 100 mathrm{mL} ) of a solution contains ( 2 mathrm{g} ) of acetic acid and 3 g of sodium acetate providing ( K_{a}=1.8 times 10^{-5} . ) Choose the
correct option.
A. This solution is basic in nature
B. This solution is acidic in nature
c. This solution is amphoteric in nature
D. This solution is neutral in nature
11
587The reaction ( boldsymbol{C H}_{3} boldsymbol{C O O H}+ )
( C_{2} H_{5} O H leftrightharpoons C H_{3} C O O C_{2} H_{5}+H_{2} O )
can be made to proceed in the forward direction by:
A. increasing the temperature
B. sudden cooling of the reaction mixture
c. conducting the reaction in the presence of a small quantity of ( N a O H )
D. taking excess of ( C_{2} H_{5} O H ) and ( C H_{3} C O O H )
11
588Strength of an acid solution or a basic solution can be determined by knowing the hydrogen ion concentrations in
them, using a pH scale.
(i) Neutral solution has pH 7.
(ii) Acidic solution has pH less than 7 .
(iii) Basic solution has pH more than 7 .
The pH of a solution is inversely proportional to hydrogen(H+) ion concentration in it.
Teacher told three students Renuka,
Bhawna and Seema to test their saliva
with pH paper before and after having their lunch. Identify the correct observation from the following.
A. Bhawna observed that pH paper turned red and recorded pH value of ( 2.3-2.5 ) after having lunch
B. Seema observed that pH paper turned yellow and recorded pH value of ( 5.6-5.8 ) before having lunch
c. Renuka observed that pH paper turned green and recorded pH value of 7.4-7.9 before having lunch
D. observations made by both Renuka and Seema were correct
11
589The solubility of ( P b F_{2} ) in water at ( 25^{circ} C )
is ( sim 10^{-3} M . ) What is its solubility in
( mathbf{0 . 0 5} boldsymbol{M} boldsymbol{N} boldsymbol{a} boldsymbol{F} ) solution?
Assume the latter to be fully ionised.
A . ( 1.6 times 10^{-6} M )
В. ( 1.2 times 10^{-6} M )
c. ( 1.2 times 10^{-5} M )
D. ( 1.6 times 10^{-4} M )
11
590What is the maximum ( p H ) of ( 0.10 M )
solution in ( M g^{2+} ) from which
( M g(O H)_{2} ) will not precipitate. Given :
( boldsymbol{K}_{s p}left(boldsymbol{M} boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2}right)=mathbf{1 . 2} times mathbf{1 0}^{-11} )
11
591Assertion
( boldsymbol{K}_{boldsymbol{p}}=boldsymbol{K}_{c} ) for all reactions. BECAUSE
Reason
( boldsymbol{K}_{boldsymbol{p}} ) and ( boldsymbol{K}_{boldsymbol{c}} ) are interrelated by the
equation ( boldsymbol{K}_{boldsymbol{p}}=boldsymbol{K}_{c}(boldsymbol{R} boldsymbol{T})^{boldsymbol{Delta} boldsymbol{n}} )
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
592For the reaction ( A+B rightleftharpoons 3 C ) at ( 25^{0} C )
A 3 Lvessel contains ( 1,2, ) and 4 moles of
A, ( B, ) and ( C ) respectively. Predict the direction of reaction if:
a) ( K_{C} ) for the reaction is 10
b) ( K_{C} ) for the reaction is 15
c) ( K_{C} ) for the reaction is 10.66
A. a) Backward direction
b) Forward direction ( c ) ) At equilibrium
B. a) Forward direction b) Backward direction c) Forward direction
c. a) Backward direction b) Forward direction c) Back direction
D. a) Backward direction
b) Backrward direction c) At equilibrium
11
593If the concentration of ( mathrm{H}^{+}(mathrm{aq}) ) ions increases in a solution, the acidity:
A . increases
B. decreases
C. remains same
D. None of the above
11
594Which of the following represents a bronsted acid-base reaction?
( mathbf{A} cdot 3 O_{2}(g) rightleftharpoons 2 O_{3}(g) )
B. ( O H^{-}+H_{3} O^{+} rightleftharpoons 2 H_{2} O )
( mathbf{c} cdot B a C l_{2} cdot 2 H_{2} O(s) triangleq B a C l_{2}(s)+2 H_{2} O(g) )
( mathbf{D} cdot C a^{2+}+C O_{3}^{2-} rightarrow C a C O_{3}(s) )
( mathbf{E} cdot F e+C u^{2+} rightleftharpoons F e^{2+}+C u )
11
595What is the equation for the
equilibrium constant ( left(K_{c}right) ) for the
following equilibrium reaction?
( frac{1}{2} A(g)+frac{1}{3} B(g) rightleftharpoons frac{3}{2} C(g) )
( ^{mathbf{A}} cdot_{K_{C}}=frac{[A]^{frac{1}{2}}[B]^{frac{1}{3}}}{[C]^{frac{3}{2}}} )
( ^{mathrm{B}} K_{C}=frac{[C]^{frac{3}{2}}}{[A]^{2}[B]^{2}} )
( ^{mathbf{c}}_{K_{C}}=frac{[C]^{frac{3}{2}}}{[A]^{frac{1}{2}}[B]^{frac{1}{5}}} )
( ^{mathrm{D}} K_{C}=frac{[C]^{frac{3}{2}}}{[A]^{frac{1}{2}}+[B]^{frac{1}{3}}} )
11
596Fresh milk has a pH of 6. On changing into curd, its pH becomes:
A. more than 6
B. less than 6
c. does not change
( D )
11
597Calculate pH of solution obtained by
mixing ( 500 mathrm{ml} ) of ( 0.4 mathrm{M}, M_{1} O H ) and
1500ml of ( frac{mathbf{0 . 8}}{mathbf{3}} ) molar ( boldsymbol{N}_{mathbf{2}} boldsymbol{O} boldsymbol{H} . boldsymbol{K}_{boldsymbol{b}_{1}}= )
( mathbf{1 0}^{-mathbf{7}} boldsymbol{K}_{boldsymbol{b}_{2}}=mathbf{4} times mathbf{1 0}^{-mathbf{7}} )
11
598The value of ( boldsymbol{K}_{s p} ) is ( boldsymbol{H} boldsymbol{g} boldsymbol{C l}_{2} ) at room
temperture is ( 4.0 times 10^{-15} ). The
concentration of ( C l^{ominus} ) ion in its
aqueous solution at saturation point is:
A ( cdot 1 times 10^{-5} )
В. ( 2 times 10^{-5} )
c. ( 2 times 10^{-15} )
D. ( 8 times 10^{-15} )
11
599Consider the reaction,
( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}(boldsymbol{a} boldsymbol{q})+boldsymbol{S} boldsymbol{C} boldsymbol{N}^{-}(boldsymbol{a} boldsymbol{q}) rightleftharpoons )
( boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{C} boldsymbol{N}^{2-}(boldsymbol{a} boldsymbol{q}) )
How will the equilibrium position shift
if ( A g N O_{3}(a q) ) is added? ( (A g S C N ) is insoluble)
11
600You have two solutions A and B. The pH
of solution ( A ) is 6 and ( p H ) of solution ( B ) is
8. Which solution has more hydrogen ion concentration? Which of this is
acidic and which one is basic?
11
601Discuss the relation between ( boldsymbol{K}_{boldsymbol{p}} ) and
( K_{c} ) for this equilibrium:
( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})+mathbf{2} boldsymbol{C} boldsymbol{l}_{2(boldsymbol{g})} rightleftharpoons boldsymbol{4} boldsymbol{H} boldsymbol{C l}_{(boldsymbol{g})}+ )
( boldsymbol{O}_{2(boldsymbol{g})} )
A. ( K_{p}=K_{c} )
( mathbf{B} cdot K_{p}>K_{c} )
c. ( K_{p}<K_{c} )
( ^{mathrm{D}} K_{p}=frac{1}{K_{c}} )
11
602What is ( p H ) Scale? Explain that ( p H )
change of the mouth is the cause of tooth decay
11
603Sodium carbonate exists as(in):
A ( cdot N a_{2} C O_{3} cdot 10 H_{2} O(s) )
B . ( N a_{2} C O_{3} cdot H_{2} O(s) )
c. ( N a_{2} C O_{3} )
D. All of the above
11
604un
9. The process depicted by the equation
H2O (s) — H2O (1)
AH = +1.43 kcal represents
(a) fusion
(b) melting
(c) evaporation
(d) boiling
11
605Introduction of inert gas at constant
volume to a gaseous reaction at equilibrium, results in formation of :
A. same amount of product
B. more quantity of product
c. less quantity of product
D. no product
11
606Which of the following metal sulphides
has maximum solubility in water?
( mathbf{A} cdot C d Sleft(K_{s p}=36 times 10^{-30}right) )
B ( cdot operatorname{Fe} Sleft(K_{s p}=11 times 10^{-20}right) )
( mathbf{c} cdot H g Sleft(K_{s p}=32 times 10^{-54}right) )
D. ( Z n Sleft(K_{s p}=11 times 10^{-22}right) )
11
607Which of the following will give a neutral pH solution when dissolved in
water?
A. ( N a O H )
B. ( C s C l )
( mathbf{c} cdot H B r )
D. ( C H_{3} ) СООН
E. ( O_{2} )
11
608Which of the following is not Lewis
base?
A. ( A g^{+} )
в. ( H_{2} ) о
c. ( C N^{-} )
D. ( R N H_{2} )
11
6094. Calculate the oxalate concentration necessary to
precipitate CaC,0, in a saturated solution of calcium
carbonate. Kcac,0. = 2.6 10-9; Kcaco, = 8.7 x 10-9.
(a) 2.6 x 10-9M (b) 2.8 x 10-5 M
(c) 9.3 x 10-5 M (d) 3.4 x 10-3 M
11
610The hydrogen, ion concentration of a
solution is 0.001 M. What is the ( p H ) of
the solution?
11
611Which buffer solution comprising of the
following has its ( p H ) value greater than
( 7 ? )
A ( cdot C H_{3} C O O H+C H_{3} C O O N a )
в. ( H C O O H+H C O O K )
c. ( C H_{3} C O O N H_{4} )
D. ( N H_{4} O H+N H_{4} C l )
11
612The ionization constant of
dimethylamine is ( 5.4 times 10^{-4} ). Calculate
its degree of ionization in its ( 0.02 mathrm{M} ) solution. What percentage of dimethylamine is ionized if the solution
is also 0.1M in NaOH?
11
613( 100 mathrm{ml} ) of ( 0.1 mathrm{M} C mathrm{H}_{3} mathrm{COOH} ) is mixed
with ( 50 mathrm{ml} ) of ( 0.1 mathrm{M} ) NaOH solution and
pH of the resulting solution is 5. The change in pH if ( 100 mathrm{ml} ) of ( 0.05 mathrm{M} ) NaOH
is added in the above solution is:
A . 1.30
B. 4.74
( c cdot 5 )
D. 3.8
11
614Two moles of ( P C l_{5} ) are heated in a
closed vessel of 2 litre capacity. When
the equilibrium is attained ( 40 % ) of it has been found to be dissociated. What
is the value of ( K_{c} ) in ( m o l / d m^{3} ? )
A. 0.532
B. 0.266
c. 0.133
D. 0.174
E . 0.25
11
615Which compound is used for bleaching cloths in laundry?
A. Bleaching powder
B. Washing powder
c. Baking powder
D. Plaster of Paris
11
616The equilibrium constant for the reaction ( N_{2}(g)+O_{2}(g) leftrightharpoons 2 N O(g) ) is
( 4 times 10^{-4} ) at ( 2000 mathrm{K} . ) In the presence of a
catalyst, the equilibrium is attained three times faster. The
equilibrium constant in the presence of the catalyst at ( 2000 mathrm{K} ) is:
A. ( 40 times 10^{-4} )
B. ( 4 times 10^{-4} )
c. ( 4 times 10^{-3} )
D. ( 4 times 10^{-8} )
11
617The ( p H ) of ( 10^{-4} M K O H ) solution will
be:
( A cdot 4 )
B. 1
( c cdot 10.5 )
D. 10
11
618pH of saturated solution of ( C a(O H)_{2} ) is
9. the solubility product ( left(K_{s p}right) ) of
( boldsymbol{C a}(boldsymbol{O H})_{2} ) is:
A ( .0 .5 times 10^{-15} )
В. ( 0.25 times 10^{-10} )
( c cdot 0.125 times 10^{-15} )
5
D. ( 0.5 times 10^{10} )
11
619The conductivity of a saturated solution of ( A g_{3} P O_{4} ) is ( 9 times 10^{-6} S m^{-1} ) and its
equivalent conductivity is ( 1.50 times ) ( 10^{-4} S m^{2} ) equivalent ( ^{-1} . ) The ( K_{s p} ) of
( A g_{3} P O_{4} ) is:
A ( cdot 4.32 times 10^{-18} )
B. ( 1.8 times 10^{-9} )
c. ( 8.64 times 10^{-13} )
D. None of these
11
620On long standing, bleaching powder undergoes auto oxidation.
A. True
B. False
11
621The ( p H ) of ( 0.1 mathrm{M} ) acetic acid is ( 3, ) the
dissociation constant of acid will be:
A ( cdot 1.0 times 10^{-4} )
В. ( 1.0 times 10^{-5} )
c. ( 1.0 times 10^{-3} )
D. ( 1.0 times 10^{-8} )
11
622Choose the correct combination among thefollowing
A) A mixture of weak acid and its salt of strong base acts as acidic buffer.
B) As number of moles of acid or base required to change the ( p^{H} ) of the buffer
by one unit increases, the quality of buffer increases.
C) Buffer action is maximum at ( boldsymbol{p}^{boldsymbol{H}}= )
( P^{K a} ) in case of acidic buffer.
A. All are correct
B. A only correct
c. B only correct
D. A only false
11
623In which of the following cases, does the reaction go furthest to completion?
A ( cdot K=10^{3} )
B. ( K=10^{-2} )
c. ( K=10^{5} )
D. ( K=1 )
11
624In which of the following ( K_{p} ) is less than
( boldsymbol{K}_{c} ? )
A ( cdot N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) )
B . ( 2 H I(g) rightleftharpoons H_{2}(g)+I_{2}(g) )
c. ( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons 2 S O_{3}(g) )
D. ( P C l_{5}(g) rightleftharpoons P C l_{3}(g)+C l_{2}(g) )
11
625Calculate the ( mathrm{pH} ) of ( 10^{-8} mathrm{M} mathrm{HCl} )
( A cdot 8 )
B. 6
( c cdot 7 )
D. 6.98
11
626Equilibrium constant for the reaction
( mathbf{2} N boldsymbol{O}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons 2 boldsymbol{N} boldsymbol{O} boldsymbol{C l}(boldsymbol{g}) ) is
correctly given by the expression:
( ^{mathbf{A}} cdot_{K}=frac{[2 N O C l]}{[2 N O]left[C l_{2}right]} )
в. ( _{K}=frac{[N O C l]^{2}}{[N O]^{2}left[C l_{2}right]} )
( ^{mathbf{c}}_{K}=frac{[N O]^{2}[C l]^{2}}{[N O]^{2}+left[C l_{2}right]} )
( K=frac{[N O]^{2}+[C l]^{2}}{[N O C l]} )
11
627The following reaction is at equilibrium, ( boldsymbol{F} boldsymbol{e}_{(a q)}^{3+}+boldsymbol{S C} boldsymbol{N}_{(a q)}^{-} rightleftharpoons )
( left[boldsymbol{F e}(boldsymbol{S C N})_{(a q)}^{2+} ; boldsymbol{K}_{c}=frac{[boldsymbol{F e}(boldsymbol{S C N})]^{2+}}{left[boldsymbol{F e}^{3+}right]left[boldsymbol{S C N}^{-}right]}right. )
In the above reaction, color intensity of
red colour can be increased by:
B. addition of oxalic acid which reacts with ( F e^{3+} ) ions
C. addition of ( H g^{2+} ) ions which reacts with ( S C N^{-} ) ions
D. red colour intensity cannot be changed.
11
628( boldsymbol{K}_{s p} ) of ( boldsymbol{C u} boldsymbol{S}, boldsymbol{A} boldsymbol{g}_{2} boldsymbol{S} ) and ( boldsymbol{H} boldsymbol{g} boldsymbol{S} ) are
( 10^{-31}, 10^{-44} ) and ( 10^{-54} ) mol ( ^{2} ) litre ( ^{-2} )
respectively. Select the correct order for their solubility in water
( mathbf{A} cdot A g_{2} S>H g S>C u S )
B. ( H g S>C u S>A g_{2} S )
c. ( H g S>A g_{2} S>C u S )
D. ( A g_{2} S>C u S>H g S )
11
629The equilibrium constant ( left(boldsymbol{K}_{c}right) ) for the
reaction ( boldsymbol{H} boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{B} boldsymbol{H}^{+}+boldsymbol{A}^{-} ) is ( mathbf{1 0 0} )
If the rate constant for the forward
reaction is ( 10^{5} ), then rate constant for
the backward reaction is
A ( cdot 10^{7} )
B . ( 10^{3} )
( mathbf{c} cdot 10^{-3} )
D. ( 10^{-5} )
11
630Sulphide ions in alkaline solution react with solid sulphur to form polyvalent
sulphide ions. The equilibrium constant for the formation of ( S_{2}^{2-} ) and ( S_{3}^{2-} ) from. ( S )
and ( S^{2-} ) ions are 1.7 and 5.3 respectively.
Calculate equuilibrium constant for the
formation of ( S_{3}^{2-} ) from ( S_{2}^{2-} ) and ( S )
A . 0.31
в. 3.11
c. 31.3
D. 0.0313
11
631A buffer of ( mathrm{pH} 8.50 ) is prepared from
0.02 mole of ( K C N . ) The desired volume
of buffer solution is to be 1 litre. How
will you make this buffer using ( boldsymbol{H} boldsymbol{C l} ) ? What is the change after addition of ( 0.5 times 10^{-4} ) mole ( H C l ) to ( 100 c m^{3} ) and
same amount of ( N a O H ) in ( 100 c m^{3} ) of
buffer?
( left(boldsymbol{K}_{boldsymbol{a}} boldsymbol{H} boldsymbol{C} boldsymbol{N}=boldsymbol{6} . boldsymbol{2} times mathbf{1 0}^{-10}right) )
11
632Which of the following compounds will be dissociated into its constituent
ions?
This question has multiple correct options
A. Solid ( N a C l )
B. Molten NaCl
c. solid ( C a C l_{2} )
D. Molten ( C a C l )
11
633In a buffer solution consisting of a weak
acid and its salt, the ratio of the
concentration of salt to acid is
increased tenfold, then the ( p H ) of the solution will:
A. Increase by one
B. Increase tenfold
c. Decrease by one
D. Decrease tenfold
11
634The solubility of all solids in water increase with increase in temperature.
A. True
B. False
11
635For an equilibrium reaction involving gases, the forward reaction is first order
while the reverse reaction is second
order. The units of ( boldsymbol{K}_{boldsymbol{p}} ) for forward equilibrium is:
A . atm
B ( . a t m^{2} )
c. ( a t m^{-1} )
D. ( a t m^{-2} )
11
636( p K_{a_{1}} ) of carbonic acid in blood at body
temperature ( left(37^{circ} Cright) ) is ( 6.1 . ) Hence, ratio
( left[boldsymbol{H} boldsymbol{C O}_{3}^{-}right] /left[boldsymbol{H}_{2} boldsymbol{C O}_{3}right] ) is approximately:
A . 1.3:
B. 1: 1.3
( c cdot 20: )
D. 1: 20
11
637Q47. It has been found that the pH of a 0.01 M solution of an organic acid is 4.15. Calculate the
concentration of the anion, the ionization constant of the acid and its pk
11
638For the equilibrium ( N_{2}+3 H_{2} rightleftharpoons )
( 2 N H_{3}, K_{c} ) at ( 1000 K ) is ( 2.37 times 10^{-3} . ) If
at equilibrium ( left[boldsymbol{N}_{2}right]=mathbf{2} boldsymbol{M},left[boldsymbol{H}_{2}right]=boldsymbol{3} boldsymbol{M} )
the concentration of ( boldsymbol{N} boldsymbol{H}_{3} ) is:
A . ( 0.00358 M )
B. ( 0.0358 M )
c. ( 0.358 M )
D. 3.58 М
11
639The ( p H ) of ( 0.1 ~ M ) solution of the following salts increases in the order
A. ( N a C l<N H_{4} C l<N a C N<H C l )
в. ( operatorname{NaCN}<N H_{4} C l<N a C l<H C l )
c. ( H C l<N a C l<N a C N<N H_{4} C l )
D. ( H C l<N H_{4} C l<N a C l<N a C N )
11
640( boldsymbol{p} boldsymbol{K}_{a} ) of Quinoline base is ( 4.88 . ) What will
be the ( p K_{a} ) of ( 0.01 mathrm{M} ) solution of it?
A . 4.88
B. 0.01
c. 9.12
D. 14
11
6411.6 mole of ( boldsymbol{P C l}_{5}(boldsymbol{g}) ) is placed in ( boldsymbol{4} boldsymbol{d} boldsymbol{m}^{3} )
closed vessel. When the temperature is
raised to ( 500 K ), it decomposes and at
equilibrium 1.2 mole of ( P C l_{5}(g) )
remains.What is the ( K_{c} ) value for the
decomposition of ( boldsymbol{P} boldsymbol{C l}_{mathbf{5}}(boldsymbol{g}) ) to ( boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g}) )
and ( C l_{2}(g) ) at ( 500 K ? )
( mathbf{A} cdot 0.013 )
B. 0.050
c. 0.033
D. 0.067
11
642Q61. The ionization constant of nitrous acid is 4.5 x 10-4. Calculate the pH of 0.04 M sodium
nitrite solution and also its degree of hydrolysis.
11
643The solubility product of ( boldsymbol{H} boldsymbol{g}_{2} mathbf{1}_{2} ) is equal
to
( mathbf{A} cdotleft[H g_{2}^{2+}right]left[I^{-}right] )
B ( cdotleft[H g^{2+}right]left[I^{-}right] )
c. ( left[H g_{2}^{2+}right]left[I^{-}right]^{2} )
D ( cdotleft[H g^{2+}right]left[I^{-}right]^{2} )
11
644Which of the following is not Lewis acid?
A. ( B F_{3} )
в. ( A l C l_{3} )
c. ( F e C l_{3} )
D. ( P H_{3} )
11
645A reaction in equilibrium is represented by the following equation:
( mathbf{2 A}(s)+mathbf{3 B}(boldsymbol{g}) rightleftharpoons mathbf{3} boldsymbol{C}(boldsymbol{g})+boldsymbol{D}(boldsymbol{g})+boldsymbol{O}_{2} )
if the pressure on the system is reduced to half of its original value then
A. The amounts of ( C ) and ( D ) increases
B. The amounts of ( C ) and ( D ) decreases
c. The amounts of ( B ) and ( D ) decreases
D. All the amounts remain constant
11
646Which of the following salts is a strong
electrolyte?
A . ( N a C l )
в. ( K C l )
c. ( M g C l_{2} )
D. All of the above
11
647For the given reaction the equilibrium expression
( mathbf{2} boldsymbol{A}_{(boldsymbol{g})}+boldsymbol{B}_{(boldsymbol{g})} Leftrightarrow mathbf{3} boldsymbol{C}_{(boldsymbol{g})}+boldsymbol{D}_{(boldsymbol{g})} )
( mathbf{A} cdot[A]^{2}[B][D] )
В. ( frac{[C]^{3}[D]}{left.[A]^{2}[] Bright]} )
c. ( frac{[2 C][D]}{[2 A][B]} )
D. ( frac{[D]}{[A]^{2}[B]} )
E ( cdot frac{[A]^{2}[B]}{[C]^{3}[D]} )
11
648Table salt is contaminated with
( N a H C O_{3} ) due to presence of ( M g C l_{2} ) as impurity (from sea).
If true enter 1 , else enter 0 .
11
649Solid Ammonium carbamate
dissociates as:
( N H_{2} C O O N H_{4}(s) rightleftharpoons 2 N H_{3}(g)+ )
( boldsymbol{C O}_{2}(boldsymbol{g}) )
In a closed vessel, solid ammonium
carbonate is in equilibrium with its dissociation products. At equilibrium, ammonia is added such that the partial
pressure of ( N H_{3} ) at new equilibrium
now equals the original total pressure. Calculate the ratio of total pressure at new equilibrium to that of original total
pressure.
A ( cdot frac{31}{27} )
в. ( frac{17}{7} )
c. ( frac{49}{29} )
D. None of these
11
650Q12. A mixture of 1.57 mol of N, 1.92 mol of H, and 8.13 mol of NH, is introduced into a 20L
reaction vessel at 500 K. At this temperature, the equilibrium constant K for the reaction
N. (g) + 3H, (g) + 2NH, () is 1.7 x 10-2.
Is this reaction at equilibrium? If not, what is the direction of net reaction?
11
651At same temperature and under a
pressure of ( 4 a t m, P C l_{5} ) is ( 10 % ) dissociation. Calculate the pressure at
which ( P C l_{5} ) will be ( 20 % ) dissociated
temperature remaining same.
11
652Solid rightleftharpoons liquid equilibrium can be achieved only at the melting point of the substance.
A. True
B. False
11
653( Z n(O H)_{2} ) is an amphoteric hydroxide which is involved in the following two equilibria existing simultaneously in aqueous solution.
( boldsymbol{Z n}(boldsymbol{O} boldsymbol{H})_{2}(boldsymbol{s}) rightleftharpoons boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{a} boldsymbol{q})+ )
( mathbf{2 O H}^{-}(boldsymbol{a q}) ; boldsymbol{K}_{s p}=mathbf{1 . 2} times mathbf{1 0}^{-mathbf{1 7}} )
( operatorname{Zn}(O H)_{2}(s)+2 O H^{-}(a q) rightleftharpoons )
( left[Z n(O H)_{4}right]^{2-}(a q) ; K_{c}=0.12 )
At what ( p H ) the solubility of ( Z n(O H)_{2} ) will be minimum?
A. ( p H=4.11 )
в. ( p H=6.32 )
c. ( p H=7.68 )
D. ( p H=9.99 )
11
654The decrease in % in ( left[boldsymbol{H}^{+}right] ) when ( boldsymbol{p} boldsymbol{H} )
increases by 0.1 will be:
A . 10
B. 30
c. 50
D. 20
11
655Assertion
pH of 10 M H Cl aqueous solution is
less than 1.
Reason
pH is negative logarithm of ( boldsymbol{H}^{+} )
concentration.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
656The value of ( k_{c} ) for the reaction
( mathbf{2} boldsymbol{A} rightleftharpoons boldsymbol{B}+boldsymbol{C} ) is ( 2 times 10^{-3} )
At a given time the composition of reaction mixture is ( [A]=[B]=[C]=3 x )
( 10^{-4} ) M. In which direction the reaction
will proceed?
A. From left to right
B. From right to left
c. The reaction is at equilibrium
D. First to the right than left
11
657The experimental curve obtained when the rate of a reaction is plotted against
time, appeared parallel to the time axis
some time after the reaction started.
This indicates that:
A. the reaction has stopped
B. the equilibrium is established
c. the concentration of the reactants is negligible
D. the reaction is complex
11
658At ( 1400 K, K_{c}=2.5 times 10^{-3} ) for reaction
( boldsymbol{C H}_{4}(boldsymbol{g})+mathbf{2} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{S}_{2}(boldsymbol{g})+ )
( 4 H_{2}(g) . ) At ( 10.0 L ) reaction vessel at
( 1400 mathrm{K} ) contains 2.00 mole of ( mathrm{CH}_{4}, 3.0 )
mol of ( mathrm{CS}_{2}, 3.0 ) mole of ( mathrm{H}_{2} ) and 4.0 mole
of ( mathrm{H}_{2} mathrm{S} ). Then
A. this reaction is at equilibrium with above concentrations
B. the reaction will proceed in forward direction to reach equilibrium
c. the reaction will proceed in backward direction to each equilibrium
D. the information is insufficient to decide the direction of progress of reaction
11
659Which of the following cannot
decompose on heating to give ( C O_{2} ? )
A ( cdot L i_{2} C O_{3} )
в. ( N a_{2} C O_{3} )
( mathbf{c} cdot K H C O_{3} )
D. ( B a C O_{3} )
11
660( boldsymbol{K}_{boldsymbol{w}} ) of pure water is ( mathbf{1 0}^{-12} ) at ( mathbf{6 0}^{circ} boldsymbol{C} ). The
( p H ) of pure water at ( 60^{circ} mathrm{C} ) is:
11
661Which has highest ( p H ? )
A. ( C H_{3} ) СООК
в. ( N a_{2} C O_{3} )
c. ( N H_{4} C l )
D. ( N a N O_{3} )
11
662The solubility of a substance is 40 to 50
C such that at same temperature its solution contains 5 g of it in 10 gof water
A . True
B. False
c. Nither
D. Either
11
663Which of the following compounds is known as baking soda?
A. Sodium carbonate
B. Calcium carbonate
c. Sodium bicarbonate
D. Calcium bicarbonate
11
664The degree of dissociation ( (alpha) ) of a weak
electrolyte, ( A_{x} B_{y} ) is related to van’t Hoff
factor (i) by the expression:
A ( cdot alpha=frac{i-1}{(x+y-1)} )
B. ( alpha=frac{i-1}{x+y+1} )
c. ( alpha=frac{x+y-1}{i-1} )
D. ( alpha=frac{x+y+1}{i-1} )
11
665Solubility product of ( C a C O_{3} ) is
( 5 times 10^{-9} . ) Find its solubility.
11
666Concentration of ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{C l} ) and ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{O} boldsymbol{H} )
in a buffer solution are in the ratio of
( 1: 10, mathrm{Kb} ) for ( N H_{4} O H ) is ( 10^{-10} . ) The pH of
the buffer is:
(BHU, 1994)
A .4
B. 5
( c cdot 9 )
D. 1
11
667Which of the following statement is
correct:
A. Sodium hydroxide turns blue litmus red.
B. Nitric acid turns red litmus blue.
C. Sodium hydroxide turns red litmus blue
D. tooth decay is caused by the presence of a base
11
668When strong base ( (N a O H) ) is added to the weak acid (acetic acid,
( left.C H_{3} C O O Hright), ) then dissociation of
acetic acid increases; this effect is
known as:
A. Common ion effect
B. Reverse ion effect
c. Saltation effect
D. Solubility effect
11
669If very small amount of phenolphthalein is added to 0.15 mol litre ( ^{-1} ) solution
of sodium benzoate, what fraction of the
indicator will exist in the coloured
form? State any assumption that you make.
( K_{a}(text { Benzoic acid })=6.2 times )
( mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{w}}left(boldsymbol{H}_{mathbf{2}} boldsymbol{O}right)=mathbf{1} times mathbf{1 0}^{-mathbf{1 4}} )
( boldsymbol{K}_{l n} ) (Phenolphthalein) ( mathbf{3} . mathbf{1 6} times mathbf{1 0}^{-mathbf{1 0}} )
11
670In the system, ( C a F_{2}(s) rightleftharpoons )
( C a^{+2}(a q)+2 F^{-} ) increasing the
concentration of ( C a^{2+} ) ions four times
will cause the equilibrium
concentration of ( boldsymbol{F}^{-} ) ions to change to
times the initial value.
A . 4
B. ( frac{1}{2} )
( c cdot 2 )
D.
11
671A reversible reaction ( A rightleftharpoons C ) takes
place in two steps ( boldsymbol{A} rightleftharpoons boldsymbol{B} ; boldsymbol{B} rightleftharpoons boldsymbol{C} )
which are also equilibrium steps. If the equilibrium constants of the two steps
are ( K_{1} ) and ( K_{2} ) respectively, the overall equilibrium constant ( boldsymbol{K} ) is equal to:
( ^{text {A }} cdot frac{K_{1}}{K_{2}} )
в. ( frac{K_{2}}{K_{1}} )
( mathbf{c} cdot K_{1} times K_{2} )
D. ( K_{1}-K_{2} )
11
672For an equilibrium ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(ell) )
which of the following statement is
true?
A. The pressure changes do not affect the equilibrium
B. More of ice melts if pressure on the system is increased
c. More of liquid freezes if pressure on the system is increase
D. The pressure changes may increase or decrease the degree of advancement of the reaction depending upon the temperature of the system.
11
673( boldsymbol{C C l}_{4} rightleftharpoons boldsymbol{C}+mathbf{2 C l}_{2} )
The equilibrium constant ( p K ) for the given reaction at ( 700^{0} C ) is 0.76 atm.
The initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at
( mathbf{7} mathbf{0 0}^{mathbf{o}} mathbf{C} ) is:
A. 0.22 atm
B. 0.44 atm
c. 0.84 atm
D. 0.11 atm
11
674The real bleaching agent present in bleaching powder is:
A. chlorine
B. oxygen
c. сао
D. None of the above
11
675The ( K_{s p} ) for a sparingly soluble ( A g_{2} C r O_{4} ) is ( 4 times 10^{-12} . ) The molar
solubility of the salt is:
( begin{array}{lll}text { A } cdot 2.0 times 10^{-6} & text {mol } & L^{-1}end{array} )
( begin{array}{lll}text { В. } 1.0 times 10^{-4} & text {тод } L^{-1}end{array} )
( begin{array}{lll}text { C. } 2.0 times 10^{-12} & text {mol } & L^{-1}end{array} )
D. ( 1.0 times 10^{-15} ) mol ( L^{-1} )
11
676List 1 and List 2 contains four entries
each. Entries of List 1 are to be matched
with some entries of List 2. One or more
than one entries of List 1 may have the matching with the same entries of List
2
11
677The equilibrium constant for the
reaction, ( N_{2}(g)+O_{2}(g)=2 N O(g) ) is
( 4 times 10^{-4} ) at ( 2000 mathrm{k} . ) In the presence of a
catalyst, the equilibrium is attained ten times faster. Therefore, the equilibrium constant in the presence of the catalyst of ( 2000 mathrm{k} ) is:
A. ( 4 times 10^{-2} )
B. ( 40 times 10^{-4} )
c. ( 4 times 10^{-4} )
D. ( 4 times 10^{-1} )
11
678Assume that the decomposition of
( H N O_{3} ) can be represented by the following equation
( 4 H N O_{3}(g) rightleftharpoons 4 N O_{2}(g)+ )
( mathbf{2} boldsymbol{H}_{mathbf{2}} boldsymbol{O}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) )
The reaction approaches equilibrium at ( 400 K ) temperature and 30 atm pressure. At equilibrium partial
pressure of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) is ( boldsymbol{2} ) atm.
Calculate ( boldsymbol{K}_{c} ) in ( (boldsymbol{m} boldsymbol{o l} / boldsymbol{L})^{3} ) at ( boldsymbol{4} boldsymbol{0} boldsymbol{0} boldsymbol{K} )
( (text { Use }: boldsymbol{R}=mathbf{0 . 0 8 a t m}-boldsymbol{L} / boldsymbol{m o l}-boldsymbol{K}) )
( A cdot 4 )
B. 8
( c cdot 16 )
D. 32
11
679The following reaction is known to occur in the human body:
( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{H}_{2} boldsymbol{C O}_{3} rightleftharpoons boldsymbol{H}^{+}+ )
( boldsymbol{H} boldsymbol{C O}_{mathbf{3}}^{-} )
If ( C O_{2} ) escapes from the system
A . pH will decrease
B. ( H^{+} ) ion concentration will decrease
c. ( H_{2} C O_{3} ) concentration will be unaltered
D. The forward reaction will be promoted
11
680In reversible reactions concentration of:
A. reactants decreases with time at equilibrium
B. products increases with time at equilibrium
C. reactants decreases and then increases with time at equilibrium
D. reactants and products are constant at equilibrium
11
681( 0.5 mathrm{ml} ) of ( H_{2} ) and 0.5 mole of ( I_{2} ) react in
10 litre flask at ( 448^{circ} mathrm{C} ). The equilibrium
constant ( boldsymbol{K}_{c} ) is ( mathbf{5 0} ) for ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) rightleftharpoons )
( 2 H I(g) )
What is the value of ( boldsymbol{K}_{boldsymbol{p}} ) ?
A . 50
B. 20
c. 10
D. 40
11
682Molten NaCl conducts electricity due to the presence of :
( mathbf{A} cdot ) free molecules
B. free ions
c. free electrons
D. free atoms
11
683A buffer solution is formed by mixing ( 100 mathrm{mL} 0.01 mathrm{M} C mathrm{H}_{3} mathrm{COOH} ) with ( 200 mathrm{mL} )
( 0.02 mathrm{M} C H_{3} C O O N a . ) If this buffer
mL of water, ( boldsymbol{p} boldsymbol{H} ) will change by a factor
of:
11
684For the following reaction at ( 250^{circ} mathrm{C} ), the
value of ( K_{c} ) is ( 26, ) then the value of ( K_{p} ) at the same temperature will be:
( boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{5}(boldsymbol{g}) )
A . 0.57
B. 0.61
c. 0.83
D. 0.91
11
685The ( p H ) at which a ( 0.01 mathrm{M} A l^{+3} ) solution
is ( 99.99 % ) precipitated is:
( left(boldsymbol{K}_{s p} boldsymbol{A l}(boldsymbol{O H})_{3}=mathbf{1} times mathbf{1 0}^{-18} boldsymbol{a t} quad mathbf{2 5}right) )
A . 6.67
B. 7.67
c. 8.67
D. 9.617
11
686At a certain temperature 2 moles of
carbonmonoxide and 3 moles of
chlorinw were allowed to reach
equilibrium according to the reaction ( boldsymbol{C O}_{(g)}+boldsymbol{C l}_{2} leftrightharpoons boldsymbol{C O C l}_{2} ) in a 5 lit vessel.
At equilibrium if one mole of ( C O ) is
present then equilibrium constant for the reaction is
11
687State which of the following solutions contains only ions?
A ( cdot d i l . H N O_{3} )
B. Kerosene
c. ( C H_{3} ) СООН
D. Oxalic acid
11
688In a 20 litre vessel initially ( 1-1 ) mole
( C O, H_{2} O, C O_{2} ) is present, then for the
equilibrium of ( boldsymbol{C O}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{C} boldsymbol{O}_{2}+ )
( boldsymbol{H}_{2} ) following is true?
A. ( H_{2}, ) more than 1 mole
B. ( C O, H_{2} O, H_{2} ) less then 1 mole
c. ( C O_{2} & H_{2} O ) both more than 1 mole
D. All of these
11
689Le Chatelier’s principle is applicable to both homogeneous and heterogeneous equilibria.
If true enter 1 , if false enter 0 .
11
690A ( 20 L ) box contains ( O_{3} ) and ( O_{2} ) at ( t )
equilibrium at ( 202 K . K_{p}=2 times 10^{14} )
for ( 2 O_{3} rightleftharpoons 3 O_{2} . ) Assume that ( p_{O_{3}}>> )
( p_{O_{2}} ) and total pressure is 8 at ( m ), then
the partial pressure of ( boldsymbol{O}_{3} ) is:
A . exactly ( 1.6 times 10^{-6} ) at ( m )
B. sufficiently less than ( 1.6 times 10^{-6} ) atm
C. slightly more than ( 1.6 times 10^{-6} ) atm
D. very slightly less than ( 1.6 times 10^{-6} ) atm
11
691In the third group of qualitative
analysis, the precipatitating reagent is
( N H_{4} C l / N H_{4} O H . ) The function of
( N H_{4} C l ) is to
A. increase the ionisation of ( N H_{4} O H )
B. supress the ionisation of ( N H_{4} O H )
C. convert the ions of group third into their respective chlorides
D. stabilise the hydroxides of group III cations
11
692The equilibrium constant for a reaction
is ( K, ) and the reaction quotient is ( Q ). For a reaction mixture, the ratio ( frac{K}{Q} ) is 0.33 This means that:
A. the reaction mixture will equilibrium to form more reactant species
B. the reaction mixture will equilibrium to form more product species
c. the equilibrium ratio of reactant to product concentrations will be 3
D. the equilibrium ratio of reactant to product concentrations will be 0.33
11
693What is the ( K_{b} ) for ( N H_{2} ) group in glycine?
( mathbf{A} cdot 4 times 10^{-3} )
в. ( 1.6 times 10^{-10} )
c. ( 6.25 times 10^{-5} )
D. ( 2.5 times 10^{-12} )
11
694Assertion
Solubility of sparingly soluble salt decreases due to common ion effect
Reason

Solubility product constant does not
depend on common ion effect.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect

11
695Two systems, ( boldsymbol{P C l}_{5(g)} rightleftharpoons boldsymbol{P C l}_{3(g)}+ )
( boldsymbol{C l}_{2(boldsymbol{g})} ) and ( boldsymbol{C O C l}_{2(boldsymbol{g})} rightleftharpoons boldsymbol{C O}_{(g)}+boldsymbol{C l}_{2(boldsymbol{g})} )
are simultaneously in equilibrium in a vessel at constant volume. If some ( C O )
is introduced into the vessel then at the
new equilibrium, the concentration of :
A . ( P C l_{5} ) is increased
B. ( P C l_{3} ) remains unchanged
c. ( P C l_{5} ) is decreased
D. ( C l_{2} ) is increased
11
6960.01 mol of ( A g N O_{3} ) is added to 1 L of a
solution which is ( 0.1 M N a_{2} C r O_{4} ) and
( 0.005 M ) in ( N a I O_{3} . ) Calculate
( left[boldsymbol{A} boldsymbol{g}^{oplus}right],left[boldsymbol{I} boldsymbol{O}_{3}^{ominus}right] ) and ( left[boldsymbol{C r} boldsymbol{O}_{4}^{2-}right] )
( K_{s p} A g_{2} C r O_{4} ) and ( A g I O_{3} ) are ( 10^{-8} ) and ( 10^{-13} ) respectively
( mathbf{A} cdotleft[A g^{oplus}right]=0.316 times 10^{-4} M,left[I O_{3}^{ominus}right]=0.31 times )
( 10^{-10} M,left[C r O_{2}^{2-}right]=0.0975 M )
B ( cdotleft[A g^{oplus}right]=3.16 times 10^{-4} M,left[I O_{3}^{ominus}right]=3.1 times )
( 10^{-10} M,left[C r O_{2}^{2-}right]=0.975 M )
C ( cdotleft[A g^{oplus}right]=31.6 times 10^{-4} M,left[I O_{3}^{odot}right]=31 times )
( 10^{-10} M,left[C r O_{2}^{2-}right]=9.75 M )
D. None of these
11
697Given the reaction ( boldsymbol{A} rightarrow boldsymbol{B}+boldsymbol{C}, ) when
( triangle boldsymbol{H}_{text {reaction}} ) is negative, what effect
would increase in temperature (at constant pressure) have on the system at equilibrium?
A. No change
B. Cannot be determined
c. Shift to the right
D. Shift to left for ( K1 )
E. Shift to the left
11
698The equilibrium constant for the reaction
( boldsymbol{P C l}_{5(g)} rightleftharpoons boldsymbol{P} C l_{3(g)}+boldsymbol{C l}_{2(g)} ) is ( 2.4 times )
( 10^{-3} . ) Determine the equilibrium
constant for the reverse reaction at
same temperature
11
699Q3. Ata certain temperature and total pressure of 10° Pa, iodine vapours contain 40% by volume
of iodine atoms in the equilibrium I.(g) = 21 (g). Calculate K, for the equilibrium.
11
700The acid present in tea is:
A . citric
B. tannic
c. formic
D. lactic
11
701Gaseous ( N_{2} O_{4} ) dissociates into
gaseous ( N O_{2} ) according to the reaction
( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) at ( 300 mathrm{K} ) and 1
atm pressure, the degree of
dissociation of ( N_{2} O_{4} ) is ( 0.2 . ) If one mole
of ( N_{2} O_{4} ) gas is contained in a vessel then the density of the equilibrium mixture is :
A. ( 3.11 mathrm{g} / mathrm{L} )
B. 4.56 g/L
c. ( 1.56 g / L )
D. ( 6.22 mathrm{g} / mathrm{L} )
11
702Calculate the equilibrium concentration ratio of ( boldsymbol{C} ) to ( boldsymbol{A} ) if
equimolar ratio of ( A ) and ( B ) were
allowed to come to equilibrium at ( 300 K )
( boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}) leftrightharpoons boldsymbol{C}(boldsymbol{g})+ )
( boldsymbol{D}(boldsymbol{g}) ; quad boldsymbol{Delta} boldsymbol{G}^{o}=-boldsymbol{8} boldsymbol{3} boldsymbol{0} boldsymbol{c a l} )
11
703The ( left[boldsymbol{H}_{3} boldsymbol{O}^{+}right] ) in a solution having ( left[boldsymbol{O H}^{-}right]=mathbf{5} times mathbf{1 0}^{-mathbf{3}} boldsymbol{M} ) is:
A ( cdot 2 times 10^{-3} )
B. ( 2 times 10^{-12} )
c. ( 5 times 10^{-3} )
D. none of these
11
704LV-
5101 –
Q68. The solubility product constants of Ag, Cro, and AgBr are 1.1 X 10and 5.0 * 10
respectively. Calculate the ratio of molarities of their saturated solutions.
11
705Concentrated strong acid is added to a
solid mixture of 0.015 mole samples of
( F e(O H)_{2} ) and ( C a(O H)_{2} ) placed in one litre of water. At what value of ( mathrm{pH} ) will the dissolution of each hydroxide be
complete? (Assume negligible volume change) ( boldsymbol{K}_{s p}left[boldsymbol{F e}(boldsymbol{O H})_{2}right]=mathbf{7 . 9} times mathbf{1 0}^{-15} ) and
( boldsymbol{K}_{s p}left[boldsymbol{C u}(boldsymbol{O} boldsymbol{H})_{2}right]=mathbf{1 . 6} times mathbf{1 0}^{-19} )
A . 6.67
в. 7.86
( c .8 .86 )
D. 7.26
11
706The ( K_{a} ) value of ammonium ion
( left(N H_{4}+right) ) is ( 5.6 times 10^{-10}, ) the ( K_{b} ) value of
( operatorname{ammonia} N H_{3}=1.8 times 10^{-5}, ) then
A. Ammonia is more strongly basic than ammonium is acidic
B. Ammonia is weaker basic than ammonium is acidic
c. Both a and ( b )
D. Data insufficient
11
707Q. 13 What will be the value of pH of 0.01 mol dm-3 CH,COOH
(Ka = 1.74 x 10-5)?
(a) 3.4 ond (6) 3.6 ton (c) 3.9 holland (d) 3.0
-5
11
70816. A buffer solution of pH = 9.00 is made by dissolving
ammonium chloride and ammonia in water. How many
moles of ammonium chloride must be added to 1.0 L of
0.25 M ammonia to prepare this buffer?
NH,(aq) + H2O NH(aq) + OH-(aq); K, = 1.8 x 10-5
(a) 0.25 mol
(b) 0.45 mol
(c) 0.65 mol
(d) 2.2 mol
11
709Which of the following cations is not hydrolyzed in aqueous solution?
(i) ( M g^{2+} )
( (text { ii }) C a^{2+} )
( (text { iii }) N a^{+} )
( (text { iv }) boldsymbol{K}^{+} )
A. (i), (ii)
B. (iii), (iv)
c. (i), (ii), (iii), (iv)
D. (i), (ii), (iii)
11
710The characteristic properties of an acid is due to the presence of
A. hydride ions
B. hydroxyl ions
c. hydronium ions
D. oxide ions
11
711Equilibrium constant for the given reaction is ( K=10^{20} ) at temperature
( mathbf{3 0 0} boldsymbol{K} )
( boldsymbol{A}(s)+mathbf{2} boldsymbol{B}(boldsymbol{a} boldsymbol{q} .) rightleftharpoons mathbf{2} boldsymbol{C}(boldsymbol{s})+boldsymbol{D}(boldsymbol{a} boldsymbol{q} .) )
( boldsymbol{K}=mathbf{1} mathbf{0}^{mathbf{2 0}} )
The equilibrium concentration of B
starting with a mixture of 1 mol ( / ) lit of A and ( 1 / 3 m o l / l i t ) of ( B ) at ( 300 K ) is
в. ( 2 times 10^{-1} )
c. ( 2 times 10^{-11} )
D. ( 10^{-10} )
11
712Find the correct graph regarding
equilibrium state:
( A )
B.
( c )
D. All of these
11
713When ( N O ) and ( N O_{2} ) are mixed, the
following equilibrium are readily obtained, ( 2 N O_{2} rightleftharpoons N_{2} O_{4}, K_{p}= )
( 6.8 a t m^{-1} ) and ( N O+N O_{2} rightleftharpoons N_{2} O_{3} . ) In
an experiment when ( N O ) and ( N O_{2} ) are
mixed in the ratio of ( 1: 2, ) the final total
pressure was 5.05 at ( m ) and the partial
pressure of ( N_{2} O_{4} ) was ( 1.7 a t m )
Calculate
(a) the equilibrium partial pressure of ( N O,(b) K_{p} ) for: ( N O+ )
( N O_{2} rightleftharpoons N_{2} O_{3} )
A ( .3 .43 a t m^{-1} )
B. ( 5.63 a t m^{-1} )
c. ( 7.43 a t m^{-1} )
D. None of these
11
714The plot of ( log _{10} K_{p} ) against ( 1 / T ) for the reaction:
[
boldsymbol{S O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g})
]
is a straight line with slope ( =4.95 times )
( 10^{3} . ) If the ( K_{p} ) at 25 if standard
entropies for ( boldsymbol{S O}_{2}(boldsymbol{g}), boldsymbol{O}_{2}(boldsymbol{g}) ) and
[
boldsymbol{S O}_{3}(boldsymbol{g}) text { are } mathbf{2 4 8 . 2}, mathbf{2 0 5 . 1} text { and }
]
( 256.8 J K^{-1} m o l^{-1} ) at 25 respectively is
[
boldsymbol{K}_{boldsymbol{p}}=boldsymbol{X} times mathbf{1 0}^{11} text { then } mathbf{1 0} boldsymbol{X}
]
is
11
715Q5. (i) Define Le Chatelier’s principle.
(ii) Following reactions occur in a Blast furnace.
Fe,O3(s) + 3CO(g) 2Fe(s) + 3C02(8)
use Le chatelier’s principle to predict the direction of reaction when equilibrium mixture is
disturbed by
(a) adding Fe,0, (b) removing CO,
(c) removing Co.
TAY
.
.
11
716The equilibrium constant for the given
reaction: ( boldsymbol{S O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+ )
( frac{1}{2} O_{2}(g) ; K_{c}=4.9 times )
( 10^{-2} m o l^{1 / 2} l i t r e^{-1 / 2} )
What is the value of ( K_{c} ) for the reaction:
( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons 2 S O_{3}(g) ? )
A. 416 litre ( m o l^{-1} )
B . ( 2.40 times 10^{-3} ) litre ( mathrm{mol}^{-1} )
c. ( 9.8 times 10^{-2} ) litre mole( ^{-1} )
D. ( 4.9 times 10^{-2} ) litre ( m o l^{-1} )
11
717When ( 0.2 M ) acetic acid is neutralised
with ( 0.1 M ) NaOH in 0.5 litre of water
the resulting solution is slightly alkaline. Calculate the pH of the
resulting solution. ( boldsymbol{K}_{boldsymbol{a}} ) for
( boldsymbol{C H}_{3} boldsymbol{C O O H}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}} )
11
718The solubility curve of ( mathrm{KNO}_{3} ) as a
function of temperature is given above
The amount of ( mathrm{KNO}_{3} ) that will crystallize
when a saturated solution of ( mathrm{KNO}_{3} ) in
( 100 mathrm{ml} ) of water is cooled from ( 90^{circ} mathrm{C} ) to
( 30^{circ} mathrm{C}, ) is
( A cdot 16 g )
B. 100 g
( c cdot 56 g )
D. 160 g
11
719Which acid is present in the stinging hair of nettle leafs?11
720The ionisation constants of formic acid
and ammonium hydroxide are ( 2 times 10^{-4} )
and ( 2 times 10^{-5} ) respectively. The pH of
aqueous solution of ammonium formate is :
( A cdot 7 )
B. 6.
c. 11.5
D. 8
11
7211. Given that K, for HClO and HCN are 3.0 x 10-8 and
4.8 x 10-10, respectively, the equilibrium constant for
the reaction
HCIO(aq) + CN-(aq) C10 (aq) + HCN(aq), is
(a) 6.3 x 101
(C) 1.6 x 1012
(6) 1.6 x 10-2
(d) 1.4 x 10-17
11
722Which of the following is the most
acidic compound?
A. ( C H_{2}=C H_{2} )
в. ( C H equiv C H )
c.
D.
11
723( 0.25 mathrm{M} ) solution of pyridine chloride
( C_{5} H_{6} N^{+} C l^{-} ) was found to have a pH of
2.699. What is ( boldsymbol{K}_{boldsymbol{b}} ) for pyridine, ( boldsymbol{C}_{boldsymbol{5}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{N} ) ?
( (log 2=0.3010) )
11
724The reactions ( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P C l}_{3}(boldsymbol{g})+ )
( C l_{2}(g) ) and ( C O C l_{2}(g) rightleftharpoons C O(g)+ )
( C l_{2}(g) ) are simultaneously in
equilibrium in an equilibrium box at constant volume. A few moles of ( C O(g) ) are later introduced into the vessel.
After some time, the new equilibrium concentration of
A. ( P C l_{5} ) will remain unchanged
B. ( C l_{2} ) will be greater
c. ( P C l_{5} ) will become less
D. ( P C l_{5} ) will become greater
11
725Which of the following is a Lewis acid?
A ( . H_{2} O )
в. ( C l^{circ} )
( mathrm{c} cdot B F_{3} )
D. ( N H_{3} )
11
726For the reaction ( C O(g)+2 H_{2}(g) leftrightharpoons )
( boldsymbol{C H}_{2} boldsymbol{O H}(boldsymbol{g}) . ) If active mass of ( boldsymbol{C O} ) is
kept constant and active mass of ( boldsymbol{H}_{2} ) is tripled, the rate of forward reaction will
become:
A. three times
B. six times
c. eight times
D. nine times
11
727Which among following is electron pair acceptor?
A. Arrhenius acid
B. Arrhenius base
c. Lewis acid
D. Lewis base
E. Bronsted-Lowry acid
11
728Assertion
( K_{p} ) can be equal to or less than or even
greater than the value of ( boldsymbol{K}_{c} )
Reason
( boldsymbol{K}_{boldsymbol{p}}=boldsymbol{K}_{boldsymbol{c}}(boldsymbol{R} boldsymbol{T})^{boldsymbol{Delta} boldsymbol{n}} )
the relation between ( boldsymbol{K}_{boldsymbol{p}} ) and ( boldsymbol{K}_{boldsymbol{c}} )
depends on the change in the number of moles of gaseous reactants and
products.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
729Find the ( p H ) of the resulting solution and then mark the option in which ( p H ) exists between color transition range of an indicator.
( 100 mathrm{ml} ) of ( 0.8 mathrm{M} mathrm{HCO}_{3}^{-}+100 mathrm{ml} ) of ( 0.4 mathrm{M} )
( boldsymbol{C O}_{3}^{2-} )
[For ( boldsymbol{H}_{2} boldsymbol{C O}_{3}: boldsymbol{K}_{boldsymbol{a}_{1}}=boldsymbol{4} times mathbf{1 0}^{-boldsymbol{7}} boldsymbol{&} boldsymbol{K}_{boldsymbol{a}_{2}}= )
( left.4 times 10^{-11}right] )
A. phenol red ( (6.8 text { to } 8.4) )
B. propyl red ( (4.6 text { to } 6.4) )
c. phenolphthalein ( (8.3 text { to } 10.1) )
D. Malachite green (11.4 to 13)
11
730Oxidation number of ( C l ) in ( C a O C l_{2} )
(bleaching powder) is:
A . zero, since it contains ( C l_{2} )
B. -1 , since it contains ( C l^{-} )
c. ( -1, ) since it contains ( C l O^{-} )
D. +1 and -1 since it contains ( C l O^{-} ) and ( C l^{-} )
11
731Simultaneous solubility of ( boldsymbol{A} boldsymbol{g} boldsymbol{C} boldsymbol{N} boldsymbol{S}(boldsymbol{a}) )
and ( A g B r(b) ) in a solution of water will
be
( boldsymbol{K}_{s p_{(A g B r)}}=mathbf{5} times mathbf{1 0}^{-13} ) and ( boldsymbol{K}_{s p_{(A g C N S)}}= )
( 10^{-12} )
A ( cdot a=4.08 times 10^{-7} ) mol litre ( ^{-1} ; b=8.16 times 10^{-7} ) mollitre ( ^{-1} )
В . ( a=4.08 times 10^{-7} ) mol litre ( ^{-1} ; b=4.08 times 10^{-7} ) mollitre ( ^{-1} )
( mathbf{c} cdot a=8.16 times 10^{-7} )mollitre( ^{-1} ; b=4.08 times 10^{-7} )mollitre( ^{-1} )
D. None of these
11
732Q4. PC15, PCl, and Cl, are at equilibrium at 500 K and having concentration 1.59M PCI, 1.59M
Cl, and 1.41M PCI. Calculate Kc for the reaction PCI, = PC1, + Cl2
11
733Assertion: A mixture of ( C H_{3} ) COOH
and ( C H_{3} C O O N H_{4} ) is not a buffer
solution.

Reason: An acidic buffer contains
the mixture of a weak acid and its salt
with a strong base.
A. Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
c. Assertion is correct but Reason is not correct
D. Assertion is not correct but Reason is correct
E. Both Assertion and Reason are not correct

11
734What would be the ionisation constant
( left(boldsymbol{K}_{boldsymbol{a}}right) ) of ( boldsymbol{C H}_{3} boldsymbol{C O O H} ? )
A ( cdot 2 times 10^{-5} )
B ( cdot 10^{-5} )
C ( .2 times 10^{-6} )
D. ( 5 times 10^{-6} )
11
735A closed vessel contains helium and
ozone at a pressure of ( mathrm{P} ) atm. The ratio of He and oxygen atoms is 1: 1 . If helium is
removed from the vessel, the pressure of the sytem will reduced to:
( A cdot 0.5 P ) atm
B. 0.75 P atm
c. ( 0.25 mathrm{P} ) atm
D. 0.33 P atm
11
736The solubility product of a sparingly soluble salt ( A X_{2} ) is ( 3.2 times 10^{11} ). Its
solubility (moles/litre) is:
A ( .3 .1 times 10^{-4} )
B. ( 2 times 10^{3} )
c. ( 4 times 10^{-4} )
D. ( 5.6 times 10^{-6} )
11
737( 0.02 M ) solution of ( N H_{4} O H ) is ( 3 % )
dissociated. Calculate the dissociation
constant of ( boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{O} boldsymbol{H} )
11
738The precipitate of ( boldsymbol{C a} boldsymbol{F}_{2}left(boldsymbol{K}_{s p}=mathbf{1 . 7} timesright. )
( left.10^{-10}right) ) is obtained when equal volumes
of the following are mixed
( mathbf{A} cdot 10^{-4} M C a^{2+}+10^{-4} M F^{-} )
B. ( 10^{-2} M C a^{2+}+10^{-3} M F^{-} )
c. Both A and B
D. None of these
11
739Useful buffer range of weak acid
( boldsymbol{H} boldsymbol{A}left(boldsymbol{K}_{a}=mathbf{1 0}^{-5}right) ) is:
( mathbf{A} cdot 5 ) to 7
B. 4 to 6
c. 3 to 5
D. none of these
11
740The function of ‘buffer solution’ is:
A. to increase the pH value in chemical reaction
B. to decrease the pH value on chemical reaction
C. to increase or decrease the pH value of according the need
D. to keep the pH value constante in chemical reaction
11
741Which of the following is not a mineral acid?
A. Hydrochloric acid
B. Citric acid
c. Sulphuric acid
D. Nitric acid
11
742( 30 g m ) of ethanoic acid present in 100 ( g m ) of water, determine molality of ethanoic acid in water?11
743The element which is not common between the compounds called baking
soda and soda ash is:
A. nitrogen
B. hydrogen
c. oxygen
D. sulphur
11
744What concentration of ( boldsymbol{F}- )
( boldsymbol{C H}_{2} boldsymbol{C O O H},left(boldsymbol{K}_{boldsymbol{a}}=boldsymbol{2} boldsymbol{6} times mathbf{1 0}^{-boldsymbol{3}}right) ) is
needed so that ( left[boldsymbol{H}^{+}right]=mathbf{2} times mathbf{1 0}^{-mathbf{3}} ) ?
A ( cdot 1.53 times 10^{-3} M )
В. ( 2.6 times 10^{-3} M )
c. ( 5.2 times 10^{-3} M )
D. ( 3.53 times 10^{-3} ) М
11
745Bleaching powder is used:
This question has multiple correct options
A. for bleaching cotton, wood pulp
B. as a disinfectant and germicide
C. for the manufacture of chloroform
D. as a reducing agent in industries
11
746From the give options, which of the following compound will make best buffer solution?
A. ( H_{2} O, 1 M ) NaOH, 1 M ( H_{2} ) SO ( _{4} ),
в. ( H_{2} O, ) 1 ( M C H_{3} C O O H, 1 M N a^{+} C H_{3} C O O^{-} )
c. ( H_{2} O, 1 M C H_{3} C O O H, 6 M N a^{+} C H_{3} C O O^{-} )
D. ( H_{2} O, 1 M C H_{3} C O O H, 1 M N a O H )
11
747( boldsymbol{K}_{boldsymbol{p}} ) for the reaction ( boldsymbol{N}_{mathbf{2}}(boldsymbol{g})+mathbf{3} boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons )
( 2 N H_{3}(g), ) at ( 298 K ) is ( 5.2 times 10^{-5} . ) What
is the value of ( K_{c} ) at ( 298 K ), for the
reaction ( frac{1}{2} N_{2}(g)+frac{3}{2} H_{2}(g) rightleftharpoons N H_{3}(g) )
11
748LLLLLLLLL LLCCC
Q22. Bromine monochloride (BrCl) decomposes into bromine and chlorine and reaches the equilibrium:
2BrCl(3) – Br.(g) + C1,(g)
The value of K is 32 at 500 K. If initially pure BrCl is present at a concentration of
3.3 10 mol L”, what is its molar concentration in the mixture at equilibrium?

1
11
749Two equilibria, ( A B rightleftharpoons A^{+}+B^{-} . ) are
simultaneously maintained in a solution with equilibrium constants,
( K_{1} ) and ( K_{2} ) respectively. The ratio of
( left[boldsymbol{A}^{+}right] ) to ( left[boldsymbol{A B}_{2}^{-}right] ) in the solution is:
A. directly proportional to ( left[B^{-}right] )
B . inversely proportional to [ ( B^{-} )
C. directly proportional to the square of ( left[B^{-}right] )
D. inversely proportional to the square of ( left[B^{-}right] )
E. independent of ( left[B^{-}right] )
11
750