(B) The dissociation of $AgCl$ is represented as: $AgCl(s) \rightleftharpoons Ag^+(aq) + Cl^-(aq)$ Let the solubility be $x \, mol \, L^{-1}$. Then,$[

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$1 \times 10^{-3} \, mol \, L^{-1}$

(B) The dissociation of $AgCl$ is represented as: $AgCl(s) \rightleftharpoons Ag^+(aq) + Cl^-(aq)$ Let the solubility be $x \, mol \, L^{-1}$. Then,$[Ag^+] = x$ and $[Cl^-] = x$. The solubility product expression is: $K_{sp} = [Ag^+][Cl^-] = x \times x = x^2$ Given $K_{sp} = 1 \times 10^{-6}$. Therefore,$x^2 = 1 \times 10^{-6}$ $x = \sqrt{1 \times 10^{-6}} = 1 \times 10^{-3} \, mol \, L^{-1}$.

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

Medium

The solubility product of $AgCl$ is $1 \times 10^{-6}$ at $298 \, K$. Its solubility in $mol \, L^{-1}$ would be:

A
$1 \times 10^{-6} \, mol \, L^{-1}$
B
$1 \times 10^{-3} \, mol \, L^{-1}$
C
$1 \times 10^{-12} \, mol \, L^{-1}$
D
None of these

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solubility product

On adding $0.1 \ M$ solution each of $[Ag^+]$,$[Ba^{2+}]$,and $[Ca^{2+}]$ to a $Na_2SO_4$ solution,which species precipitates first? Given: $K_{sp}(BaSO_4) = 10^{-11}$,$K_{sp}(CaSO_4) = 10^{-6}$,$K_{sp}(Ag_2SO_4) = 10^{-5}$.

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If $0.001435 \ g$ of $AgCl$ is present in $100 \ mL$ of water,calculate the $K_{sp}$.

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$CaSO_3 \downarrow + SO_2 + H_2O \longrightarrow Ca(HSO_3)_2$

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Assign $A, B, C, D$ from the given type of reaction.
$Ca(OH)_2 + 2HF \longrightarrow CaF_2 \downarrow + 2H_2O$

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If the solubility of $AgCl$ (molar mass $= 143 \, g/mol$) in water at $25 \, ^\circ C$ is $1.43 \times 10^{-4} \, g/100 \, mL$ of solution,then the value of $K_{sp}$ is?

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The solubility product of $AgCl$ is $1 \times 10^{-6}$ at $298 \, K$. Its solubility in $mol \, L^{-1}$ would be:

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On adding $0.1 \ M$ solution each of $[Ag^+]$,$[Ba^{2+}]$,and $[Ca^{2+}]$ to a $Na_2SO_4$ solution,which species precipitates first? Given: $K_{sp}(BaSO_4) = 10^{-11}$,$K_{sp}(CaSO_4) = 10^{-6}$,$K_{sp}(Ag_2SO_4) = 10^{-5}$.

If $0.001435 \ g$ of $AgCl$ is present in $100 \ mL$ of water,calculate the $K_{sp}$.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.$CaSO_3 \downarrow + SO_2 + H_2O \longrightarrow Ca(HSO_3)_2$

Assign $A, B, C, D$ from the given type of reaction.$Ca(OH)_2 + 2HF \longrightarrow CaF_2 \downarrow + 2H_2O$

If the solubility of $AgCl$ (molar mass $= 143 \, g/mol$) in water at $25 \, ^\circ C$ is $1.43 \times 10^{-4} \, g/100 \, mL$ of solution,then the value of $K_{sp}$ is?

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$CaSO_3 \downarrow + SO_2 + H_2O \longrightarrow Ca(HSO_3)_2$

Assign $A, B, C, D$ from the given type of reaction.
$Ca(OH)_2 + 2HF \longrightarrow CaF_2 \downarrow + 2H_2O$