(C) The molar mass of $AgCl = 107.9 + 35.5 = 143.4 \ g \ mol^{-1}$.Solubility in $mol \ L^{-1}$ $(S)$ = $\frac{1.434 \times 10^{-3} \ g \ L^{-1}}{143.

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(C) The molar mass of $AgCl = 107.9 + 35.5 = 143.4 \ g \ mol^{-1}$.Solubility in $mol \ L^{-1}$ $(S)$ = $\frac{1.434 \times 10^{-3} \ g \ L^{-1}}{143.4 \ g \ mol^{-1}} = 10^{-5} \ mol \ L^{-1}$.For $AgCl_{(s)} \rightleftharpoons Ag^{+}_{(aq)} + Cl^{-}_{(aq)}$,the solubility product $K_{sp} = [Ag^{+}][Cl^{-}] = S^2$.$K_{sp} = (10^{-5})^2 = 10^{-10}$.Therefore,$-\log K_{sp} = -\log(10^{-10}) = 10$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Solubility product

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At $298 \ K$,the solubility of silver chloride in water is $1.434 \times 10^{-3} \ g \ L^{-1}$. The value of $-\log K_{sp}$ for silver chloride is $........$ (Given: molar mass of $Ag = 107.9 \ g \ mol^{-1}$ and $Cl = 35.5 \ g \ mol^{-1}$)

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A
$9$
B
$8$
C
$10$
D
$7$

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6-2.Equilibrium-II (Ionic Equilibrium)

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At $298 \ K$,the solubility of silver chloride in water is $1.434 \times 10^{-3} \ g \ L^{-1}$. The value of $-\log K_{sp}$ for silver chloride is $........$ (Given: molar mass of $Ag = 107.9 \ g \ mol^{-1}$ and $Cl = 35.5 \ g \ mol^{-1}$)

Similar Questions

What mass of $AgI$ will dissolve in $1.0 \ L$ of its saturated solution? [Given $: K_{sp}(AgI) = 1.0 \times 10^{-16} ; (At. \ wt. \ Ag = 108; I = 127)$]

If the ${K_{sp}}$ for $HgSO_4$ is $6.4 \times 10^{-5}$,then the solubility of the salt is:

Which of the following pairs of ions would be expected to form a precipitate when their dilute solutions are mixed?

For the precipitation of $AgCl$ by $Ag^{+}$ ions and $HCl$,which of the following is true?

The value of $K_{sp}$ for $B_2CO_3$ is $3.2 \times 10^{-5}$. The concentration of $B^{+}$ in its saturated solution is :-

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