Dilution processes of different aqueous solutions, with water, are given in LIST-L The effects of dilution of the solutions on [H + ] are given in LIST-II.
(Note: Degree of dissociation ( 
) of weak acid and weak base is <<1; degree of hydrolysis of salt <<1; if] 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 value 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 [if] changes to half of its initial value on dilution |
R. (20 mL of 0.1 M HC1 + 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 of 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 times of its initial value on dilution. |
5. the value of [H+] changes of 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
4; Q 
2; R 
3; S 
1
4;Q 
3;R 
2;S 
3
1; Q 
4; R 
5; S 
3
1;Q 
5;R 
4;S 
1
Text Solution
Verified by ExpertsD
(P) is a buffer, so [H + ] does not change on dilution, as [salt] = [acid].
(Q) contains only CH 3 COONa
So CH 3 COO - + H 2 O 
CH 3 COOH + OH -
decreases by 
times
(R) is also salt hydrolysis
So, 
So, C is made 
so, [H + ] becomes 
(S) it is a solubility equilibria
So dilution does not effect [H + ] or [OH - ]
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