Which of the following ionic salts will not increase the solubility in acidic aqueous solution relative to its solubility in pure water?
(a) NaF; (b) LiCl; (c) Ca(ClO4)2; (d) NH4CH3COO; (e) KNO2; (f) Cu(NO3)2
The correct answer is : (b) LiCl , (c) Ca(ClO4)2, (f) Cu(NO3)2
Explanation
Salts of weak acids dissociate in acidic aqueous solutions and the conjugate base reacts with water molecule to give acid and OH- ion
For example, when NaF is dissolved in acidic aqueous solution, it completely dissociates into Na+ and F- ions
F- (aq) + H2O (l) HF (aq) + OH- (aq)
Decrease in concentration of F- causes more NaF to dissolve in solution to maintain concentration of F-
Hence solubility of NaF increases in acidic aqueous solution
This does not happen with salts of strong acids.
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