The solubility product for a salt of type AB is . The molarity of its standard solution will be:
1.
2.
3.
4.
The salt solution that is basic in nature is:
1. Ammonium chloride.
2. Ammonium sulphate.
3. Ammonium nitrate.
4. Sodium acetate.
The maximum concentration of equimolar solutions, of ferrous sulphate and sodium sulphide, so that when mixed in equal volumes, there is no precipitation of iron sulphide, will be:
(For iron sulphide, Ksp = 6.3 × 10–18).
1. | 1.90 | 2. | 13.42 |
3. | 1.47 | 4. | 12.63 |
The ionic product of water at 310 K is 2.7 × 10–14.
The pH of neutral water at this temperature will be:
1. | 2.56
|
2. | 6.78
|
3. | 7.32
|
4. | 11.41 |
The ionization constant of chloroacetic acid is 1.35 × 10–3. The pH of a 0.1 M acid solution will be:
1. | 1.94
|
2. | 6.14
|
3. | 3.23
|
4. | 5.64 |
The ionization constant of nitrous acid is 4.5 × 10–4. The pH of a 0.04 M sodium nitrite solution will be:
1. | 2.56 | 2. | 6.14 |
3. | 7.96 | 4. | 11.74 |
The pH of a 0.1 M solution of cyanic acid (HCNO) is 2.34. The ionization constant of the acid will be:
1. | 1.50 | 2. | 13.50 |
3. | 0.50 | 4. | 12.45 |
0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. The pH of the solution will be
1. | 12.70 | 2. | 1.30 |
3. | 3.14 | 4. | 11.70 |