Equilibrium · Question 70

What is the [OH-] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)2?

1. 0.40 M
2. 0.0050 M
3. 0.12 M
4. 0.10 M

The dissociation equilibrium of a 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

1. (2Kp/P)1/2
2. (Kp/P)
3. (2Kp/P)
4. (2Kp/P)1/3

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

1. 64 times
2. 4 times
3. 8 times
4. 16 times

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. 3.7 10-3 M
2. 1.11 10-3 M
3. 1.11 10-4 M
4. 3.7 10-4 M

The value of equilibrium constant of the reaction HI(g) 12H2(g) + 12I2(g) is 8.0. The equilibrium constant of the reaction H2(g) + I2(g) 2HI(g) will be

1. 16
2. 1/8
3. 1/16
4. 1/64

The values of Kp for the reactions, X Y + Z ....(i) A 2B ....(ii) are in the ratio 9 : 1. If degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio

1. 36 : 1
2. 1 : 1
3. 3 : 1
4. 1 : 9

Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest pH?

1. MgCl2
2. CaCl2
3. SrCl2
4. BaCl2

Which one of the following ionic species has the greatest proton affinity to form stable compound?

1. NH2-
2. F-
3. I-
4. HS-

The equilibrium constants of the following are N2 + 3H2 2NH3; K1 N2 + O2 2NO; K2 H2 + 12O2 H2O; K3 The equilibrium constant (K) of the reaction: 2NH3 + 52O2 2NO + 3H2O will be

1. K2K33/K1
2. K2K3/K1
3. K23K3/K1
4. K1K33/K2

A weak acid, HA, has a Ka of 1.00 10-5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to

1. 1.00\%
2. 99.9\%
3. 0.100\%
4. 99.0\%