Q. No.Which one of the following is true for any diprotic acid, H2X?
1. Ka2 = Ka1
2. Ka1 > Ka2
3. Ka1 < Ka2
4. \(K_{a1}=\frac{1}{K_{a2}}\)
1. Ka2 = Ka1
2. Ka1 > Ka2
3. Ka1 < Ka2
4. \(K_{a1}=\frac{1}{K_{a2}}\)
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 |
The dissociation of NH4OH can be suppressed by the addition of:
| 1. | NH4Cl | 2. | NH4NO3 |
| 3. | NaOH | 4. | All of the above |
For the equilibrium of the reaction,\(\mathrm{HgO}(\mathrm{~s}) \rightleftharpoons \mathrm{Hg}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_ 2(\mathrm{~g}), \mathrm{K_P}\) 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. | \(\mathrm{K}_P={1 \over 3^{2/3}}\mathrm P\) |
Based on the given equilibrium constants:
\( \begin{array}{lc} \mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3 & \mathrm{~K}_1 \\ \mathrm{~N}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO} & \mathrm{K}_2 \\ \mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightleftharpoons \mathrm{H}_2 \mathrm{O} & \mathrm{K}_3 \end{array} \)
The equilibrium constant (K) of the following reaction will be:
\(2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \stackrel{\mathrm{~K}}{\rightleftharpoons} 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O}\)
| 1. | \( \dfrac{K_{2}K_{3}^{3}}{K_{1}}\) | 2. | \( \dfrac{K_{2}K_{3}}{K_{1}}\) |
| 3. | \( \dfrac{K_{2}^{3}K_{3}}{K_{1}}\) | 4. | \( \dfrac{K_{3}^{3}K_{1}}{K_{2}}\) |
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5N+H) In A 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10–9) is?
1. 0.0060%
2. 0.013%
3. 0.77%
4. 1.6%
The solubility of AgCl (s) with solubility product 1.6×10–10 in 0.1 M NaCl solution would be?
| 1. | 1.26 × 10–5 M | 2. | 1.6 × 10–9 M |
| 3. | 1.6 × 10–11 M | 4. | zero |
A 20-litre container at 400 K contains CO2 (g) at pressure 0.4 atm and an excess of SrO (neglecting the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container.
The maximum volume of the container, when the pressure of CO2 attains its maximum value will be:
(Given that: SrCO3(s) ⇋ SrO(s) + CO2(g) , Kp = 1.6 atm)
| 1. | 10 litre | 2. | 2 litre |
| 3. | 4 litre | 4. | 5 litre |
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 |
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