1. | \(\text{OH}^- \) | 2. | \(\text{NH}_3 \) |
3. | \(\text H_2 \text O \) | 4. | \(\text{BF}_3 \) |
1. | –13.73 cal | 2. | 1372.60 cal |
3. | –137.26 cal | 4. | –1381.80 cal |
1. | Weak acid and it's salt with a strong base. |
2. | Equal volumes of equimolar solutions of weak acid and weak base. |
3. | Strong acid and its salt with a strong base. |
4. | Strong acid and its salt with a 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. | 0.36 | 2. | 3.6 × 10–2 |
3. | 3.6 × 10–3 | 4. | 3.6 |
1. | 3 | 2. | 2 |
3. | 4 | 4. | 1 |
Consider the following reaction taking place in 1L capacity container at 300 K.
\(\mathrm{A +B \rightleftharpoons C+D }\)
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 |
The solubility product of \(\mathrm{BaSO_4}\) in water is \(1.5 \times 10^{-9} \). The molar solubility of \(\mathrm{BaSO_4}\) 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. \(1.0 \times 10^{-8} M\)
\(3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g}) \)
For the above reaction at 298 K, \(\text K_c\) is found to be \(3.0 \times 10^{-59} \). If the concentration of \(\text O_2\) at equilibrium is 0.040 M, then the concentration of \(\text O_3 \) in M is:
1. \(1.2 \times 10^{21} \)
2. \(4.38 \times 10^{-32} \)
3. \(1.9 \times 10^{-63} \)
4. \(2.4 \times 10^{31} \)
1. | 2.57 | 2. | 5.57 |
3. | 3.57 | 4. | 4.57 |