The molar solubility of Ni(OH)2 in a solution containing 0.10 M NaOH, given that the ionic product of Ni(OH)2 is 2.0 × 10–15, is:
1. | 2.0 × 10–13 M | 2. | 2.0 × 10–12 M |
3. | 2.0 × 10–11 M | 4. | 2.0 × 10–16 M |
The values of Ksp of two sparingly soluble salts Ni(OH)2 and AgCN are 2.0 × 10–15 and 6 × 10-17 respectively.
The more soluble salt is:
1. Ni(OH)2 is more soluble than AgCN
2. AgCN is soluble in than Ni(OH)2
3. Both have similar solubility
4. None of the above
The solubility of A2X3 in pure water, assuming that neither kind of ion reacts with water is:
(solubility product of A2X3, Ksp = 1.1 × 10–23)
1. | 5.0 × 10–5 mol/L. | 2. | 1.0 × 10–5 mol/L |
3. | 1.0 × 10–4 mol/L | 4. | 5.0 × 10–4 mol/L. |
The pH after 50.0 mL of 0.10 ammonia solution is treated with 25.0 mL of 0.10M HCl solution is-
(Kb = 1.77 × 10–5 )
1. 5.74
2. 10.12
3. 8.34
4. 9.24
The ionization constant of ammonia is 1.77 × 10–5. The pH of a 0.05M of ammonia solution is-
1. 12
2. 11
3. 10
4. 6
The pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present is:
(pKb of ammonia solution is 4.75)
1. | 12 | 2. | 9 |
3. | 6 | 4. | 11 |
The pH of 0.004M hydrazine solution is 9.7, its ionization constant Kb and pKb are respectively:
1. Kb = 8.96 × 10–7; pKb = 6.04
2. Kb = 7.26 × 10–7 ; pKb = 6.04
3. Kb = 8.96 × 10–7 ; pKb = 7.02
4. Kb = 7.26 × 10–7 ; pKb = 7.02
The ionization constant of the hypochlorous acid is 2.5 × 10–5. The concentration of hypochlorous acid 0.08 M. The percent dissociation of HOCl is:
1. 2.56 %
2. 1.21 %
3. 1.76 %
4. 2.21 %
The pH of 0.1M monobasic acid is 4.50. The value of pKa of the monobasic acid is:
1. 6. 3
2. 7.4
3. 8.0
4. 9.0
The ionization constant of HF is 3.2 × 10–4 and its solution concentration is 0.02 M. The pH of the solution is:
1. 3.45
2. 2.62
3. 4.21
4. 1.89