The concentration of KI and KCl in a solution | vedclass

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(B) The concentration of $I^-$ and $Cl^-$ ions in the final mixture becomes $0.0005 \ M$ each due to dilution ($20 \ mL$ added to $20 \ mL$ makes $40

Vedclass · Accepted Answer

$AgI$ will be precipitated

Vedclass · Answer

(B) The concentration of $I^-$ and $Cl^-$ ions in the final mixture becomes $0.0005 \ M$ each due to dilution ($20 \ mL$ added to $20 \ mL$ makes $40 \ mL$ total volume).In a saturated solution of $AgI$,the concentration of $Ag^+$ ions is $[Ag^+] = K_{sp}(AgI) / [I^-]_{sat}$.When the solutions are mixed,the ionic product of $AgI$ is $Q_{sp} = [Ag^+][I^-]_{mix}$.Since $[I^-]_{mix} > [I^-]_{sat}$,the ionic product $Q_{sp}$ exceeds the solubility product $K_{sp}$ of $AgI$.Therefore,$AgI$ will be precipitated.

Formula	Solubility product $(K_{sp})$
$AgBrO_3$	$2.5 \times 10^{-10}$
$MgSO_4$	$2.7 \times 10^{-27}$
$CaCO_3$	$2.7 \times 10^{-18}$
$FeC_2O_4$	$2.4 \times 10^{-15}$

The concentration of $KI$ and $KCl$ in a solution containing both is $0.001 \ M$ each. If $20 \ mL$ of this solution is added to $20 \ mL$ of a saturated solution of $AgI$ in water,what will happen?

Similar Questions

Formula Solubility product $(K_{sp})$
$AgBrO_3$ $2.5 \times 10^{-10}$
$MgSO_4$ $2.7 \times 10^{-27}$
$CaCO_3$ $2.7 \times 10^{-18}$
$FeC_2O_4$ $2.4 \times 10^{-15}$
Which of the following salts has the maximum solubility?

Solid $Ba(NO_3)_2$ is gradually dissolved in $1.0 \times 10^{-4} \, M \, Na_2CO_3$ solution. At which concentration of $Ba^{2+}$ will the precipitation begin? $(K_{sp} \, BaCO_3 = 5.1 \times 10^{-9})$

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Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4} \ M$ $Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will a precipitate begin to form? ($K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

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