CBSE
Multiple Choice QuestionsThe value of KP1 and Kp2 for the reactions
X ⇌ Y +Z ... (i)
A ⇌ 2B ... (ii)
are in the ratio of 9:1. if the degree of dissociation of X and A be equal, then the total pressure at equilibrium (i) and (ii) are in the ratio
3:1
1:9
36:1
36:1
Calculate the pOH of a solution at 250C that contains 1 x 10-10 M of hydronium ions.
7
4
9
9
The value of equilibrium constant of the reaction HI (g) ⇌ H2(g)/2 + I2/2 is 8.0
The equilibrium constant of the reaction H2(g) + I2(g) ⇌ 2 HI (g) will be
1/16
1/64
16
16
Equimolar solutions of the following were prepared in water separately which one of the solutions will record the highest pH?
SrCl2
BaCl2
MgCl2
MgCl2
A Weak acid, HA has a Ka of 1.00 x 10-5. If 0.100 mole of this percentage of acid dissociated at equilibrium is closest to:
99.0%
1.00%
99.9 %
99.9 %
Base strength of 
is in the order of
(2) > (1) > (3)
(3) > (2) > (1)
(1) > (3)> (2)
(1) > (3)> (2)
Equal volumes of three acid solutions of pH 3.4 and 5 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
1.11 x 10-4 M
3.7 x 10-4 M
3.7 x 10-3 M
3.7 x 10-3 M
If the concentration of OH- ions in the reaction Fe(OH)3 (s) ⇌ Fe3+ (aq) + 3OH-(aq) is decreased by 1/4 times, then equilibrium concentration of Fe3+ will increase by
8 times
16 times
64 times
64 times
The dissociation equilibrium of gas AB2 can be represented as
2AB2 (g) ⇌ 2AB (g) + B2 (g)
The degree of dissociation is 'x' and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant Kp and total pressure p is
(2Kp / p)
(2Kp/p)1/3
(2Kp/p)1/2
(2Kp/p)1/2
The dissociation constants for acetic acid and HCN at 25o C are 1.5 X 10-5 and 4.5 x 10-10 respectively. The equilibrium constant for the equilibrium,
CN- + CH3COOH and HCN + CH3COO-
would be
3 x 105
3.0 x 10-5
3.0 x 10-4
3.0 x 10-4
