Q. No.| 1. | \(OH^- \) | 2. | \(NH_3 \) |
| 3. | \(H_2O \) | 4. | \(BF_3 \) |
| 1. | -13.73 cal | 2. | 1372.60 cal |
| 3. | -137.26 cal | 4. | -1381.80 cal |
| 1. | weak acid and it's salt with strong base |
| 2. | equal volumes of equimolar solutions of weak acid and weak base |
| 3. | strong acid and it's salt with strong base |
| 4. | strong acid and it's salt with weak base (The pKa of acid = pKb of the base) |
| 1. | \(1 \times 10^{-4}\) |
| 2. | \(1 \times 10^{-6} \) |
| 3. | \(1 \times 10^{-5} \) |
| 4. | \(1 \times 10^{-3} \) |
| 1. | 2.57 | 2. | 5.57 |
| 3. | 3.57 | 4. | 4.57 |
\(3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g}) \)
For the above reaction at 298 K, \(K_c\) is found to be \(3.0 \times 10^{-59} \). If the concentration of \(O_2\) at equilibrium is 0.040 M, then the concentration of \(O_3 \) in M is:
1. \(1.2 \times 10^{21} \)
2. \(4.38 \times 10^{-32} \)
3. \(1.9 \times 10^{-63} \)
4. \(2.4 \times 10^{31} \)
The solubility product of \(BaSO_4\) in water is \(1.5 \times 10^{-9} \). The molar solubility of \(BaSO_4\) in 0.1 M solution of Ba(NO3)2 in-
1. \(2.0 \times 10^{-8} M\)
2. \(0.5 \times 10^{-8} M\)
3. \(1.5 \times 10^{-8} M\)
4. \(1.0 \times 10^{-8} M\)
Consider the following reaction taking place in 1L capacity container at 300 K.
\(A +B \rightleftharpoons C+D \)
If one mole each of A and B are present initially and at equilibrium 0.7 mol of C is formed, then the equilibrium constant \((K_c) \) for the reaction is
| 1. | 9.7 | 2. | 1.2 |
| 3. | 6.2 | 4. | 5.4 |
| 1. | 3 | 2. | 2 |
| 3. | 4 | 4. | 1 |
\(CO_{2}(g)\,+\,C(s)\rightarrow \,2CO(g)\)
The value of Kc for the reaction at the same temperature is:
(Given - R = 0.083 L bar K-1 mol-1)
| 1. | 0.36 | 2. | 3.6 × 10-2 |
| 3. | 3.6 × 10-3 | 4. | 3.6 |
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