The dissociation constants for acetic acid and HCN at 25 °C are 1.5 x 10-5 and 4.5 x 10-10, respectively. The equilibrium constant for the equilibrium,
CN- + CH3COOH ⇌ HCN + CH3COO-
would be:
1.
2.
3.
4.
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.
2.
3.
4.
If the concentration of OH ' ions in the reaction
1. 8 times
2. 16 times
3. 64 times
4. 4 times
1. SrCI2
2. BaCl2
3. MgCl2
4. CaCl2
The dissociation equilibrium of a gas AB2 can be represented as
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)
2. (2Kp /p)1/3
3. (2KP/p)1/2
4. (KP/P)
The value of KP1 and Kp2 for the reactions
are in the ratio of 9 : 1. If the degree of dissociation of X and A is equal, then the total pressure at equilibrium(i) and (ii) are in the ratio:
1. 3 : 1
2. 1 : 9
3. 36 : 1
4. 1 : 1
The value of the equilibrium constant of the reaction
is 8.0.
The equilibrium constant of the reaction
will be-
1. | \(1 \over 16\) | 2. | \(1 \over 64\) |
3. | 16 | 4. | \(1 \over 8\) |
The pOH of a solution at 25 °C that contains 1×10-10 M of hydronium ions is:
1. | 7.00 | 2. | 4.00 |
3. | 9.00 | 4. | 1.00 |
A weak acid, HA, has a Ka of 1.00×10-5. If 0.100 mole of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to:
1. 99.0%
2. 1%
3. 99.9%
4. 0.100%
The following equilibrium constants are given:
N2 + 3H2 ⇌ 2NH3; K1
N2 + O2 ⇌ 2NO; K2
H2 + 1/2O2 ⇌ H2O; K3
The equilibrium constant for the oxidation of NH3 by oxygen to give NO is:
1.
2.
3.
4.