Question

Dilution process of different aqueous solutions; with water, are given in LIST-I. The effects of dilution of the solutions on [H⁺] are given in LIST-II.
(Note : Degree of dissociation (α) of weak acid and weak base is << 1; degree of hydrolysis of salt <<1; [H⁺] represents the concentration of H⁺ ions)

LIST-I	List-II
P. (10 mL of 0.1 M NaOH+ 20 mL of 0.1 M acetic acid) diluted to 60 mL	1. the vale of [H+] does not change on dilution
Q. (20 mL of 0.1 M NaOH + 20 mL of 0.1 M acetic acid) diluted to 80 mL	2. the value of [H+] change to half of its initial value on dilution
R. (20 mL of 0.1 M HCl + 20 mL of 0.1 M ammonia solution) diluted to 80 mL	3. the value of [H+] changes to two times of its initial value on dilution
S. 10 mL saturated solution of Ni(OH)2 in equilibrium with excess solid Ni(OH)2 is diluted to 20 mL (solid Ni(OH)2 is still present after dilution).	4. the value of [H+] changes to 1/√2 times
	5. the value of [H+] changes to √2 times of its initial value on dilution

Match each process given in LIST-I with one or more effect(s) in LIST-II. The correct option is

Answer 1

Answer:D

Solution:

(P) is a buffer, so [H⁺] does not change on dilution, as [salt] = [acid].
(Q) contains only CH₃COONa

(S) it is a solubility equilibria
So dilution does not effect [H⁺] or [OH^–]