NEETChemistryIonic Equilibrium
The dilution processes 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: The degree of dissociation α of a weak acid and a weak base is < < 1 ; the degree of hydrolysis of salt is < < 1 ; [ H + ] represents the concentration of H + ions) ( array |l|l|l|l| & List-I & & List-II A) & array l 10 ~mL of 0.1 ~M NaOH +20 ~mL of 0.1
Options
- Aa-q;b-t;c-p;d-r;
- Ba-p;b-t;c-s;d-p;
- Ca-s;b-t;c-p;d-r;
- Da-s;b-q;c-p;d-t;
Correct answer
B. a-p;b-t;c-s;d-p;
Step-by-step solution
( A ) pH = pKa ⇒ H + will not change on dilution. ( B ) OH - = K H C = k w k a C H + 1 = k w k a C H + 2 H + 1 = C 1 C 2 = 0 .05 0 .025 = 2 ( C ) H + = K H C H + 2 H + 1 = C 2 C 1 = 1 2 ( D ) Because of dilution, the solubility does not change. So, H + = constant .