The solubility product for a salt of type AB is . The molarity of its standard solution will be:
1.
2.
3.
4.
The salt solution that is basic in nature is:
1. Ammonium chloride.
2. Ammonium sulphate.
3. Ammonium nitrate.
4. Sodium acetate.
The pKb of dimethylamine and pka of acetic acid are 3.27 and 4.77 respectively at T (K).
The correct option for the pH of dimethylammonium acetate solution is:
1. 7.75
2. 6.25
3. 8.50
4. 5.50
Given that the ionic product of is 2 × .
The solubility of in 0.1 M NaOH is ;
1. | 2 × M
|
2. | 1 × M
|
3. | 1 × M
|
4. | 2 × 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. \(2.4 \times 10^{31} \)
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. \(1.0 \times 10^{-8} M\)
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 |
1. | 3 | 2. | 2 |
3. | 4 | 4. | 1 |
1. | 0.36 | 2. | 3.6 × 10–2 |
3. | 3.6 × 10–3 | 4. | 3.6 |