(C) The solubility product constant $(K_{sp})$ values at $25^{\circ}C$ are approximately $K_{sp}(AgCl) \approx 1.8 \times 10^{-10}$ and $K_{sp}(AgBr)

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(C) The solubility product constant $(K_{sp})$ values at $25^{\circ}C$ are approximately $K_{sp}(AgCl) \approx 1.8 \times 10^{-10}$ and $K_{sp}(AgBr) \approx 5.0 \times 10^{-13}$.Since $K_{sp}(AgBr) Therefore,$AgBr$ will precipitate first.The Assertion is correct,but the Reason is incorrect because it states $K_{sp}(AgCl) < K_{sp}(AgBr)$,which is false.

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

Medium

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 $AgBr$.

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A
If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
B
If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
C
If the Assertion is correct but Reason is incorrect.
D
If both the Assertion and Reason are incorrect.

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6-2.Equilibrium-II (Ionic Equilibrium)

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Solubility product

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What would be the concentration of $H_2SO_4$ necessary to precipitate $BaSO_4$ from a solution of $0.01 \ M \ Ba^{2+}$ ions $(K_{sp} = 1.0 \times 10^{-9})$?

Medium

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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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For $Cr(OH)_3$,the $K_{sp} = 1.6 \times 10^{-30}$. What is the molar solubility of this compound in water?

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Solubility of a binary sparingly soluble salt is $1.12 \times 10^{-4} \ g \ dm^{-3}$. Calculate its solubility product $(K_{sp})$ if the molar mass of the salt is $112 \ g \ mol^{-1}$.

MediumMHT CET 2025

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Up to what $pH$ must a solution containing a precipitate of $Cr(OH)_3$ be adjusted so that the precipitate just dissolves? (Given: $[Cr^{3+}] = 0.1 \ mol/L$,$K_{sp} = 6 \times 10^{-31}$)

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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 $AgBr$.

Similar Questions

What would be the concentration of $H_2SO_4$ necessary to precipitate $BaSO_4$ from a solution of $0.01 \ M \ Ba^{2+}$ ions $(K_{sp} = 1.0 \times 10^{-9})$?

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: $\log 2 = 0.3010$)

For $Cr(OH)_3$,the $K_{sp} = 1.6 \times 10^{-30}$. What is the molar solubility of this compound in water?

Solubility of a binary sparingly soluble salt is $1.12 \times 10^{-4} \ g \ dm^{-3}$. Calculate its solubility product $(K_{sp})$ if the molar mass of the salt is $112 \ g \ mol^{-1}$.

Up to what $pH$ must a solution containing a precipitate of $Cr(OH)_3$ be adjusted so that the precipitate just dissolves? (Given: $[Cr^{3+}] = 0.1 \ mol/L$,$K_{sp} = 6 \times 10^{-31}$)

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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 $AgBr$.

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: $\log 2 = 0.3010$)