For the given reaction, the degree of dissociation of B was found to be 20% at 300 K and 24% at 500K.
\(2 \mathrm{~A}(\mathrm{~s})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{s})+\mathrm{E}(\mathrm{s})\)
The rate of backward reaction:
1. | Increases with increase in pressure and temperature |
2. | Increases with increase in pressure and decrease in temperature |
3. | Depends on temperature only and decreases with increase in temperature |
4. | Increases with increase in concentration of B and increase in the temperature |
The pH of 0.1 M solution of anilium chloride is (Ka of = 10-6)
(1) 3.5
(2) 3
(3) 4.5
(4) none of these
1L of an aqueous solution contains 0.15mole of CH3COOH (pKa = 4.8) and 0.15 mole of CH3COONa. After the addition of 0.05 mole of solid NaOH to this solution, the pH will be
(1) 4.5
(2) 4.8
(3) 5.1
(4) 5.4
In the following reaction
Which are the two Bronsted bases ?
1.
2.
3.
4.
Percentage ionisation of water at certain temperature is 3.6 X 10-7%, Calculate Kw and pH of water.
1. 10-14, pH = 6.7
2. 4 X 10-14, pH=6.7
3. 2X 10-14, pH=7
4. 10-14, pH=7
A 50 ml solution of strong acid of pH = 1 is mixed with a 50 ml solution of strong acid of pH=2. The pH of the mixture will be nearly:
(log 5.5 = 0.74)
1. 0.74
2. 1.26
3. 3.76
4. 4.50
1 litre solution of pH =4 (solution of a strong acid) is added to the 7/3 litre of water. What is the pH of resulting solution. (Log 3 = 0.48)
1. 4
2. 4.48
3. 4.52
4. 5
The pH of a solution obtained by mixing 50ml of 0.4N HCl and 50ml of 0.2M NaOH is:
1. 13
2. 12
3. 1.0
4. 2.0
Kb for a monoacidic base whose 0.10 M solution has a pH of 10.48
1. 9 X 10-6
2. 9 X 10-9
3. 9 X 10-7
4. 3 X 10-7
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