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 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 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 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