Ionic EquilibriumHard
Question
Degree of hydrolysis for a salt of strong acid and weak base is
Options
A.independent of dilution
B.increases with dilution
C.increases with decrease in Kb of the bases
D.decreases with decrease in temperature.
Solution
Let BA be this salt BA → B+ + A-
A- does not undergo hydrolysis because HA is strong acid. B+ undergoes hydroysis
h =
h = degree of hydrolysis where Kh = Hydrolysis constant = 
h ∝
greater the hydrolysis constant greater the h(degree of hydrolysis).
h ∝
greater the Kb lesser the h.
Hydrolysis is endothermic, Kh increases with temperature and h also increase with temperature.
h ∝ √ V = volume of salt solution hence h increases with dilution. Kh =
Both Kw and Kb change with temperature, hence Kh changes with temperature.
Hence, statement(B) is correct. h increases if Kb decreases, statement(C) correct.
It is found that as temperature increase, Kw and Kb increase but increase in Kw is greater than increase in Kb.
Hence, h increases with increase in temperature. or h decrease in temperature., hence statement.
(D) is correct.
(D) is not correct from explanation of (B).
A- does not undergo hydrolysis because HA is strong acid. B+ undergoes hydroysis
h =
h = degree of hydrolysis where Kh = Hydrolysis constant = h ∝
greater the hydrolysis constant greater the h(degree of hydrolysis).h ∝
greater the Kb lesser the h.Hydrolysis is endothermic, Kh increases with temperature and h also increase with temperature.
h ∝ √ V = volume of salt solution hence h increases with dilution. Kh =
Both Kw and Kb change with temperature, hence Kh changes with temperature.
Hence, statement(B) is correct. h increases if Kb decreases, statement(C) correct.
It is found that as temperature increase, Kw and Kb increase but increase in Kw is greater than increase in Kb.
Hence, h increases with increase in temperature. or h decrease in temperature., hence statement.
(D) is correct.
(D) is not correct from explanation of (B).
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