The hydrolysis of the salt of a strong acid and a weak base is called:
1. Anionic hydrolysis
2. Cationic hydrolysis
3. Amphoteric hydrolysis
4. None of the above
The relation for calculating pH of a weak base is:
1. pH =pKw -1/2 pKb + 1/2 logc
2. pH =pKw +1/2 pKb - 1/2 logc
3. pH =pKw -1/2 pKa + 1/2 logc
4. none of the above
A solution of FeCl3 in water acts as acidic due to:
1. Acidic impurities
2. Ionization
3. Hydrolysis of Fe3+
4. Dissociation
pH for the solution of salt undergoing anionic hydrolysis (say CH3COONa) is given by:
1. pH = [pKw + pKa + log c]
2. pH = [pKw + pKa - log c]
3. pH = [pKw + pKb - log c]
4. none of the above
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
The most hydrolyzed salt among the following is-
(Assume that Kb of all weak bases is the same)
1. NH4Cl
2. CuSO4
3. AlCl3
4. All are equally hydrolyzed.
The ionisation constant of ammonium hydroxide is 1.77 x 10-5 at 298 K. Hydrolysis constant of ammonium chloride is
1. 5.65 x 10-10
2. 6.50 x 10-12
3. 5.65 x 10-13
4. 5.65 x 10-12
A certain acid–base indicator is red in acid solution and blue in basic solution 75% of the indicator is presentin the solution in its blue form at pH = 5. Calculate the pH at which the indicator shows 90% red form?
(1) 3.56
(2) 5.47
(3) 2.5
(4) 7.4
Ionisation constant of HA (weak acid) and BOH (weak base) are 3.0 x 10–7 each at 298K. The percent degree of hydrolysis of BA at the dilution of 10L is :
1. 25
2. 50
3. 75
4. 40
Assertion : 0.20 M solution of is more basic than 0.20 M solution of .
Reason : 0.20 M solution of is more basic than 0.20 M solution of