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 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.
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
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.
The dissociation of NH4OH can be suppressed by the addition of
1. | NH4Cl | 2. | NH4NO3 |
3. | NaOH | 4. | All of the above |
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 |
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. | \(\mathrm{K}_P={1 \over 3^{2/3}}\mathrm P\) |
HI was heated in a sealed tube at 440C till the equilibrium was reached. At this point, HI was found to be 22 % decomposed. The equilibrium constant for this dissociation is :
1. | 0.28 | 2. | 0.08 |
3. | 0.02 | 4. | 1.99 |
Salting out action of the soap is based on:
1. Complex ion formation
2. Common ion effect
3. Solubility product
4. Acid-base neutralization
In which of the following will the solubility of AgCl be the minimum?
1. | 0.1 M NaNO3 | 2. | Water |
3. | 0.1 M NaCl | 4. | 0.1 M NaBr |