The solubility of AgCl (s) with solubility product 1.6 × 10-10 in 0.1 M NaCl solution would be :

Question

The solubility of AgCl (s) with solubility product 1.6 × 10-10 in 0.1 M NaCl solution would be : (A) 1.26 × 10-5 M (B) 1.6 × 10-9 M (C) 1.6 × 10-11 M (D) 0

Tardigrade Admin · Accepted Answer

AgCl leftharpoons Ag ++ Cl - beginarraylll text a 0 0 endarray a-S S S +0.1 k text sp =1.6 × 10-10=[ Ag +][ Cl -] = S (0.1+ S ) k sp is value seems to be very small S value can be ignored, with respect to 0.1 M 1.6 × 10-10= S × 0.1 S =1.6 × 10-9 M

Q. The solubility of $A g Cl (s)$ with solubility product $1.6 \times 1 0^{- 10}$ in $0.1 M N a Cl$ solution would be :

$1.26 \times 1 0^{- 5} M$

$1.6 \times 1 0^{- 9} M$

$1.6 \times 1 0^{- 11} M$

0

$A g Cl ⇌ A g^{+} + C l^{-}$
$a 00$
a-S $SS + 0.1$
$k_{sp} = 1.6 \times 1 0^{- 10} = [A g^{+}] [C l^{-}]$
$= S (0.1 + S)$
$k_{s p}$ is value seems to be very small
$S$ value can be ignored, with respect to $0.1 M$
$1.6 \times 1 0^{- 10} = S \times 0.1$
$S = 1.6 \times 1 0^{- 9} M$

Q. The solubility of AgCl(s) with solubility product 1.6×10−10 in 0.1MNaCl solution would be :

1.26×10−5M

1.6×10−9M

1.6×10−11M

0

AgCl⇌Ag++Cl− a ​0​0​ a-S SS+0.1 ksp ​=1.6×10−10=[Ag+][Cl−] =S(0.1+S) ksp​ is value seems to be very small S value can be ignored, with respect to 0.1M 1.6×10−10=S×0.1 S=1.6×10−9M

Q. The solubility of $A g Cl (s)$ with solubility product $1.6 \times 1 0^{- 10}$ in $0.1 M N a Cl$ solution would be :

$1.26 \times 1 0^{- 5} M$

$1.6 \times 1 0^{- 9} M$

$1.6 \times 1 0^{- 11} M$

$A g Cl ⇌ A g^{+} + C l^{-}$
$a 00$
a-S $SS + 0.1$
$k_{sp} = 1.6 \times 1 0^{- 10} = [A g^{+}] [C l^{-}]$
$= S (0.1 + S)$
$k_{s p}$ is value seems to be very small
$S$ value can be ignored, with respect to $0.1 M$
$1.6 \times 1 0^{- 10} = S \times 0.1$
$S = 1.6 \times 1 0^{- 9} M$