Assertion (A): Solubility of `AgCN` in acidic solutions is greater than in pure water.
Reason (R) : Solubility equilibrium of `AgCN` is shifted in formwed direction due to the formation of `HCN`.

Assertion (A): Solubility of AgCN in acidic solutions is greater than in pure water. Reason (R) : Solubility equilibrium of AgCN is shifted in forward direction due to the formation of HCN .

This question has statement I and Statement II. Of the four choices given after the Statements, choose the one that best describes the two Statements. Statement-I: Solubility of AgCN in acidic solution is greater than that in pure water. Statement-II: Solubility equilibria of AgCN in water is shifted in forward direction due to formation of HCN.

The solubility of AgI in NaI solutions is less than that in pure water because:

The solubility of AgI in NaI solutions is less than that in pure water because:

The solublity of I_2 in KI solution is more than its solubility in pure water because

Assertion : Solubility of AgCl in NH_(3)(aq) is greater than in pure water. Reason : When AgCl dissolve in NH_(3)(aq) , complex ion [ Ag(NH_(3))_(2)^(+) ] formation takes place and solubility equilibrium of AgCl_(3) shifted in forward direction.

Assertion : Solubility of AgCl in NH_(3)(aq) is greater than in pure water. Reason : When AgCl dissolve in NH_(3)(aq) , complex ion [ Ag(NH_(3))_(2)^(+) ] formation takes place and solubility equilibrium of AgCl_(3) shifted in forward direction.