In 1 L saturated solution of AgCl [Ksp (AgCl) = 1.6 × 10 - 1 0 ], 0.1 mole of CuCl [ K sp = 1.0 × 10 - 6 ] is added. The resultant concentration of Ag+ in the solution is 1.6 × 10 - x The value of 'x' is

Question

In 1 L saturated solution of AgCl [Ksp (AgCl) = 1.6 × 10 - 1 0 ], 0.1 mole of CuCl [ K sp = 1.0 × 10 - 6 ] is added. The resultant concentration of Ag+ in the solution is 1.6 × 10 - x The value of 'x' is (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

It is a case of simultaneous solubility of salts with a common ion. Here, solubility product of

C u Cl

is much greater than that of

A g Cl

, it can be assumed that

Cl -

in solution comes mainly from

C u Cl

[

C l^{-}] = K_{s p} (C u Cl) = 1 0^{- 3}

M
Now, for

A g Cl, K_{s p} = 1.6 \times 1 0^{- 10} = [A g^{+}] [C l^{-}]

=

[A g^{+}] \times 1 0^{- 3}

\Rightarrow [A g^{+}] = 1.6 \times 1 0^{- 7}

Q. In 1L saturated solution of AgCl[Ksp​(AgCl)=1.6×10−10], 0.1 mole of CuCl[Ksp​=1.0×10−6] is added. The resultant concentration of Ag+ in the solution is 1.6×10−x The value of 'x' is

Q. In $1 L$ saturated solution of $A g Cl [K_{s p} (A g Cl) = 1.6 \times 1 0^{- 10}],$
$0.1$ mole of $C u Cl [K_{s p} = 1.0 \times 1 0^{- 6}]$ is added. The resultant concentration of $A g^{+}$ in the solution is $1.6 \times 1 0^{- x}$ The value of ' $x$ ' is