(C) For $AgBrO_3$ (type $AB$): $K_{sp} = S^2$ $S = \sqrt{K_{sp}} = \sqrt{5.5 \times 10^{-5}} \approx 7.41 \times 10^{-3} \ M$. For $Ag_2SO_4$ (type $A

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(C) For $AgBrO_3$ (type $AB$): $K_{sp} = S^2$ $S = \sqrt{K_{sp}} = \sqrt{5.5 \times 10^{-5}} \approx 7.41 \times 10^{-3} \ M$. For $Ag_2SO_4$ (type $A_2B$): $K_{sp} = 4S^3$ $S = \sqrt[3]{\frac{K_{sp}}{4}} = \sqrt[3]{\frac{2 \times 10^{-5}}{4}} = \sqrt[3]{0.5 \times 10^{-5}} = \sqrt[3]{5 \times 10^{-6}} \approx 1.71 \times 10^{-2} \ M$. Comparing the two values,$S_{Ag_2SO_4} > S_{AgBrO_3}$ or $S_{AgBrO_3} < S_{Ag_2SO_4}$.

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

Medium

If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,what is the relationship between their solubilities?

A
$S_{AgBrO_3} > S_{Ag_2SO_4}$
B
$S_{AgBrO_3} = S_{Ag_2SO_4}$
C
$S_{AgBrO_3} < S_{Ag_2SO_4}$
D
None of the above

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Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.
Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.

MediumAIIMS 2004

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An excess of $Ag_{2}CrO_{4(s)}$ is added to a $5 \times 10^{-3} \ M$ $K_{2}CrO_{4}$ solution. The concentration of $Ag^{+}$ in the solution is closest to
[ Solubility product for $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$ ]

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Calculate the molar solubility of $Ni(OH)_{2}$ in $0.10 \, M$ $NaOH$. The solubility product constant $(K_{sp})$ of $Ni(OH)_{2}$ is $2.0 \times 10^{-15}$.

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If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,what is the relationship between their solubilities?

Similar Questions

The solubility of $PbCl_2$ is given by:

The solubility product of sparingly soluble salt $AX_{2}$ is $3.2 \times 10^{-11}$. Its solubility (in $mol / L$) is

Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.

An excess of $Ag_{2}CrO_{4(s)}$ is added to a $5 \times 10^{-3} \ M$ $K_{2}CrO_{4}$ solution. The concentration of $Ag^{+}$ in the solution is closest to[ Solubility product for $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$ ]

Calculate the molar solubility of $Ni(OH)_{2}$ in $0.10 \, M$ $NaOH$. The solubility product constant $(K_{sp})$ of $Ni(OH)_{2}$ is $2.0 \times 10^{-15}$.

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Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.
Reason : $K_{sp}$ of $AgCl < K_{sp}$ of $AgBr$.

An excess of $Ag_{2}CrO_{4(s)}$ is added to a $5 \times 10^{-3} \ M$ $K_{2}CrO_{4}$ solution. The concentration of $Ag^{+}$ in the solution is closest to
[ Solubility product for $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$ ]