The concentration of Ag+ ion in a given saturated solution of AgCl at 25° C is 1.06× 10-5g- ion per litre. Thus, the solubility product of AgCl is

Question

The concentration of Ag+ ion in a given saturated solution of AgCl at 25° C is 1.06× 10-5g- ion per litre. Thus, the solubility product of AgCl is (A)  0.353× 10-10  (B)  0.530× 10-10  (C)  1.12× 10-10  (D)  2.12× 10-10

Tardigrade Admin · Accepted Answer

[Ag+] = 1.06 × 10-5 g - ion/L = 1.06 × 10-5 mol/L = [Cl-] AgCl(s) leftharpoons Ag+ + Cl- Ksp = [Ag+][Cl-] = (1.06 × 10-5)2 = 1.12 × 10-10

Q. The concentration of $A g^{+}$ ion in a given saturated solution of $A g Cl$ at $25^{\circ} C$ is $1.06 \times 10^{- 5} g -$ ion per litre. Thus, the solubility product of $A g Cl$ is

$0.353 \times 10^{- 10}$

$0.530 \times 10^{- 10}$

$1.12 \times 10^{- 10}$

$2.12 \times 10^{- 10}$

$[A g^{+}] = 1.06 \times 1 0^{- 5} g - i o n / L$
$= 1.06 \times 1 0^{- 5} m o l / L = [C l^{-}]$
$A g Cl (s) ⇌ A g^{+} + C l^{-}$
$K_{s p} = [A g^{+}] [C l^{-}]$
$= (1.06 \times 1 0^{- 5})^{2}$
$= 1.12 \times 1 0^{- 10}$

Q. The concentration of Ag+ ion in a given saturated solution of AgCl at 25∘C is 1.06×10−5g− ion per litre. Thus, the solubility product of AgCl is

0.353×10−10

0.530×10−10

1.12×10−10

2.12×10−10