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
When NH4Cl is added in NH4OH solution, then pH of the solution
1. Increases
2. Decreases
3. Remains unchanged
4. Firstly decreases and more than decreases