(B) $1$. Calculate the molar solubility $(S)$ of $Ag_2CrO_4$ in $mol/L$: $S = \frac{\text{solubility in } g/L}{\text{molar mass in } g/mol} = \frac{1.

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(B) $1$. Calculate the molar solubility $(S)$ of $Ag_2CrO_4$ in $mol/L$: $S = \frac{\text{solubility in } g/L}{\text{molar mass in } g/mol} = \frac{1.992 \times 10^{-2}}{332} = 6 \times 10^{-5} \ mol/L$. $2$. The dissociation of silver chromate is: $Ag_2CrO_4(s) \rightleftharpoons 2Ag^{+}(aq) + CrO_4^{2-}(aq)$. $3$. From the stoichiometry,the concentration of $Ag^{+}$ is $2 \times S$. $4$. $[Ag^{+}] = 2 \times (6 \times 10^{-5} \ M) = 1.2 \times 10^{-4} \ M$.

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

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The solubility of silver chromate is $1.992 \times 10^{-2} \ g/L$. The molar mass of $Ag_2CrO_4$ is $332 \ g/mol$. What is the molar concentration of $Ag^{+}$ in a saturated solution of $Ag_2CrO_4$?

A
$3.2 \times 10^{-5} \ M$
B
$1.2 \times 10^{-4} \ M$
C
$6 \times 10^{-5} \ M$
D
$1.2 \times 10^{-5} \ M$

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Solubility product

At $25^{\circ} C$,the solubility product of $MCl$ is $1 \times 10^{-10}$. What is its molar solubility in $0.1 \ M \ NaCl$ solution at the same temperature?

MediumAP EAMCET 2022

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If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.
[Given $\sqrt{2} = 1.41$]

MediumJEE MAIN 2022

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The solubility of $AgCN$ in a buffer solution of $pH = 3$ is $x$. The value of $x$ is [Assume : No cyano complex is formed; $K_{sp}(AgCN) = 2.2 \times 10^{-16}$ and $K_{a}(HCN) = 6.2 \times 10^{-10}$]

DifficultJEE MAIN 2021

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The molar solubility (in $mol \cdot L^{-1}$) of a sparingly soluble salt $MX_4$ is $S$. The corresponding solubility product is $K_{sp}$. $S$ in terms of $K_{sp}$ is given by the relation:

DifficultWBJEE 2016

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In a qualitative analysis, $Bi^{3+}$ is detected by the appearance of a precipitate of $BiO(OH)(s)$. Calculate the $pH$ when the following equilibrium exists at $298 \text{ K}$:
$BiO(OH)(s) \rightleftharpoons BiO^{+}(aq) + OH^{-}(aq)$,
$K = 4 \times 10^{-10}$
(Given: $\log 2 = 0.3010$)

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The solubility of silver chromate is $1.992 \times 10^{-2} \ g/L$. The molar mass of $Ag_2CrO_4$ is $332 \ g/mol$. What is the molar concentration of $Ag^{+}$ in a saturated solution of $Ag_2CrO_4$?

Similar Questions

At $25^{\circ} C$,the solubility product of $MCl$ is $1 \times 10^{-10}$. What is its molar solubility in $0.1 \ M \ NaCl$ solution at the same temperature?

If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.[Given $\sqrt{2} = 1.41$]

The solubility of $AgCN$ in a buffer solution of $pH = 3$ is $x$. The value of $x$ is [Assume : No cyano complex is formed; $K_{sp}(AgCN) = 2.2 \times 10^{-16}$ and $K_{a}(HCN) = 6.2 \times 10^{-10}$]

The molar solubility (in $mol \cdot L^{-1}$) of a sparingly soluble salt $MX_4$ is $S$. The corresponding solubility product is $K_{sp}$. $S$ in terms of $K_{sp}$ is given by the relation:

In a qualitative analysis, $Bi^{3+}$ is detected by the appearance of a precipitate of $BiO(OH)(s)$. Calculate the $pH$ when the following equilibrium exists at $298 \text{ K}$:$BiO(OH)(s) \rightleftharpoons BiO^{+}(aq) + OH^{-}(aq)$,$K = 4 \times 10^{-10}$(Given: $\log 2 = 0.3010$)

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If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.
[Given $\sqrt{2} = 1.41$]

In a qualitative analysis, $Bi^{3+}$ is detected by the appearance of a precipitate of $BiO(OH)(s)$. Calculate the $pH$ when the following equilibrium exists at $298 \text{ K}$:
$BiO(OH)(s) \rightleftharpoons BiO^{+}(aq) + OH^{-}(aq)$,
$K = 4 \times 10^{-10}$
(Given: $\log 2 = 0.3010$)