Equilibrium · Question 18

0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :

1. 1
2. 3
3. 2
4. 4

Kp for the following reaction is 3.0 at 1000 K. CO2(g) + C(s) 2CO(g) What will be the value of Kc for the reaction at the same temperature? (Given : R = 0.083 L bar K-1 mol-1)

1. 3.6
2. 0.36
3. 3.6 10-2
4. 3.6 10-3

The pKb of dimethyl amine and pKa of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethyl ammonium acetate solution is :

1. 6.25
2. 8.50
3. 5.50
4. 7.75

Hydrolysis of sucrose is given by the following reaction. Sucrose + H2O Glucose + Fructose If the equilibrium constant (Kc) is 2 1013 at 300 K, the value of r G at the same temperature will be :

1. 8.314 J mol-1 K-1 300 K (2 1013)
2. 8.314 J mol-1 K-1 300 K (3 1013)
3. -8.314 J mol-1 K-1 300 K (4 1013)
4. -8.314 J mol-1 K-1 300 K (2 1013)

Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 10-15.

1. 2 10-8 M
2. 1 10-13 M
3. 1 108 M
4. 2 10-13 M

Conjugate base for Brönsted acids H2O and HF are :

1. OH- and F-, respectively
2. H3O+ and H2F+, respectively
3. OH- and H2F+, respectively
4. H3O+ and F-, respectively

pH of a saturated solution of Ca(OH)2 is 9. The solubility product ( Ksp) of Ca(OH)2 is :

1. 0.125 10-15
2. 0.5 10-10
3. 0.5 10-15
4. 0.25 10-10

Which will make basic buffer?

1. 100 mL of 0.1 M HCl + 200 mL of 0.1 M NH4OH
2. 100 mL of 0.1 M HCl + 100 mL of 0.1 M NH4OH
3. 50 mL of 0.1 M NaOH + 25 mL of 0.1 M CH3COOH
4. 100 mL of 0.1 M CH3COOH + 100 mL of 0.1 M NaOH

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations : pH of which one of them will be equal to 1?

1. B
2. A
3. D
4. C

The solubility of BaSO4 in water is 2.42 10-3 g L-1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO4 = 233 g mol-1)

1. 1.08 10-10 mol2 L-2
2. 1.08 10-12 mol2 L-2
3. 1.08 10-14 mol2 L-2
4. 1.08 10-8 mol2 L-2