For the equilibrium of the reaction, HgO(s) Hg(g) + O2(g), KP for the reaction at a total pressure of "P" will be:
1. | \(\mathrm{K}_P={2 \over 3^{3/2}}\mathrm P^{3/2}\) | 2. | \(\mathrm{K}_P={2 \over 3^{1/2}}\mathrm P^{1/2}\) |
3. | \(\mathrm{K}_P={1 \over 3^{2/3}}\mathrm P^{3/2}\) | 4. | \(\mathrm{K}_P={1 \over 3^{2/3}}\mathrm P\) |
The Ksp of Ag2CrO4, AgCl, AgBr and Agl are, respectively, 1.1x10-12, 1.8x10-10, 5.0x10-13, and 8.3x10-17. The salt precipitates that last if the AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na2CrO4 is -
1. | Agl | 2. | AgCl |
3. | AgBr | 4. | Ag2CrO4 |
The dissociation of NH4OH can be suppressed by the addition of
1. | NH4Cl | 2. | NH4NO3 |
3. | NaOH | 4. | All of the above |
In the reaction, N2O4(g) 2NO2(g), is that part of N2O4 which dissociates. The number of moles at equilibrium will be:
1.
2.
3.
4.
Inert gas is added to the equilibrium at constant pressure. The degree of dissociation will :
1. Remain unchanged
2. Decrease
3. Increase
4. Decrease or increase but cannot be predicted with certainty
The most hydrolyzed salt among the following is-
(Assume that Kb of all weak bases is the same)
1. NH4Cl
2. CuSO4
3. AlCl3
4. All are equally hydrolyzed.
In an acidic Buffer solution (CH3COOH + CH3COONa), the species mainly present in the solution are:
(Ignore negligible amount)
1. CH3COOH, CH3COO-, CH3COONa, H+
2. CH3COO-, Na+, CH3COOH
3. CH3COONa, CH3COO-, H+
4. CH3COO-, Na+, H+, CH3COONa
The solubility of BaSO4 in water is g/ litre at 298 K. The value of the solubility product will be: (Molar mass of BaSO4 = 233 gmol–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 |
Mark the conditions that favour the maximum product formation in the given reaction.
1. Low temperature and High pressure
2. Low temperature and Low pressure
3. High temperature and High pressure
4. High temperature and Low pressure
At room temperature, MY and NY3, two nearly insoluble salts, have the same Ksp values of 6.2 × 10-13. The true statement regarding MY and NY3 is:
1. | The molar solubility of MY in water is less than that of NY3. |
2. | The salts MY and NY3 are more soluble in 0.5 M KY than in pure water. |
3. | The addition of the salt of KY to a solution of MY and NY3 will have no effect on their solubilities. |
4. | The molar solubilities of MY and NY3 in water are identical. |