FormulaSolubility product (K_{sp})AgBrO_32.5 | vedclass

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(A) For a salt of the type $AB$ (where $A$ and $B$ are ions),the solubility $S$ is given by $S = \sqrt{K_{sp}}$.All the given salts are of the $1:1$ e

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$AgBrO_3$

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(A) For a salt of the type $AB$ (where $A$ and $B$ are ions),the solubility $S$ is given by $S = \sqrt{K_{sp}}$.All the given salts are of the $1:1$ electrolyte type $(AB \leftrightarrows A^{+} + B^{-})$.Therefore,the salt with the highest $K_{sp}$ value will have the maximum solubility.Comparing the $K_{sp}$ values:$AgBrO_3: 2.5 	imes 10^{-10}$$MgSO_4: 2.7 	imes 10^{-27}$$CaCO_3: 2.7 	imes 10^{-18}$$FeC_2O_4: 2.4 	imes 10^{-15}$Since $2.5 	imes 10^{-10}$ is the largest value among the given $K_{sp}$ values,$AgBrO_3$ has the maximum solubility.

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

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?

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FormulaSolubility 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?