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If the solubility products of AgCl and AgBr are 1.2 × 10^–10 and 3.5 × 10^–13 respectively, then the relation between the solubilities (denoted by the symbol ‘S’) of these salts can correctly be represented as

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S of is AgBr greater than that of AgCl

S of is AgBr times greater than that of AgCl

S of is AgBr less than that of AgCl

S of is AgBr equal to that of AgCl

answer is A.

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Detailed Solution

\large \large AgCl\left( s \right) \rightleftharpoons \mathop {AgCl}\limits_{S_1} \left( {aq} \right)\xrightarrow{{}}\mathop {A{g^ + }}\limits_{S_1} \left( {aq} \right) + \mathop {C{l^ - }}\limits_{S_1} \left( {aq} \right)

K_sp = S₁x S₁

⇒ 1.2 x10^-10 = $s_{1}^{2}$

\large \large \large AgBr\left( s \right) \rightleftharpoons \mathop {AgBr}\limits_{S_2} \left( {aq} \right)\xrightarrow{{}}\mathop {A{g^ + }}\limits_{S_2} \left( {aq} \right) + \mathop {B{r^ - }}\limits_{S_2} \left( {aq} \right)

K_sp = S₂ x S₂

⇒ 3.5 x10^-13 = $s_{2}^{2}$

By observation, S₁ > S₂

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