The pH of a 0.1 M solution of cyanic acid (HCNO) is 2.34. The ionization constant of the acid will be:
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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
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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 |
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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 |
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A mixture of 10 mL of 0.2 M Ca(OH)2 and 25 mL of 0.1 M HCl is prepared. The pH of the resultant mixture would be:
1. | 1.90 | 2. | 13.42 |
3. | 1.47 | 4. | 12.63 |
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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).
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The salt solution that is basic in nature is:
1. Ammonium chloride.
2. Ammonium sulphate.
3. Ammonium nitrate.
4. Sodium acetate.
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The solubility product for a salt of type AB is . The molarity of its standard solution will be:
1.
2.
3.
4.
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At 298 K, the solubility of Sr(OH)2 is 19.23 g/L. The pH of the solution will be:
1. | 1.50 | 2. | 13.50 |
3. | 0.50 | 4. | 12.45 |
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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 |
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