Question

Ksp of ag2co3 is 8x10^-12. The molar solubility of ag2co3 in 0.1 molar agno3 is

Answer 1

Answer: Solubility of $Ag_2CO_3$ in 0.1M $AgNO_3$ is $8\times 10^{-10}$ moles/L

Explanation: The equation for the reaction will be as follows:

$Ag_2CO_3\leftrightharpoons 2Ag^++CO_3^{2-}$

1 mole of $Ag_2CO_3$ gives 2 moles of $Ag^{+}$ and 1 mole of $CO_3^{2-}$.

Thus if solubility of $Ag_2CO_3$ is s moles/liter, solubility of  $Ag^{+}$ is 2s moles\liter and solubility of $CO_3^{2-}$ is s moles/liter

$AgNO_3\rightarrow Ag^++NO_3^-$

0.1 mole of $AgNO_3$ gives 0.1 mole of $Ag^{+}$ and 0.1 mole of $NO_3^-$.

Thus solubility of Ag is (2s+0.1) M

Therefore,  

$K_sp=[Ag^+]^2[CO_3^{2-}]$

$8\times 10^{-12}=[2s+0.1]^2[s]$

$s=8\times 10^{-10}moles\liter$

Answer 2

Explanation:

Ag2CO3(s) ⇌2Ag+(aq.)+CO3²-

(0.1 + 2S) M + CO−23(aq)S M

Ksp = [Ag+]²[CO−32]

8×10−12 = (0.1 + 2S)²(S)

S = 8 × 10-10 M