For a sparingly soluble salt Ap Bq, the relationship of its solubility product (Ls) with its sol

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For a sparingly soluble salt Ap Bq, the relationship of its...

For a sparingly soluble salt $\mathrm{A}_{\mathrm{p}} \mathrm{B}_{\mathrm{q}}$, the relationship of its solubility product $\left(L_{\mathrm{s}}\right)$ with its solubility $(S)$ is (a) $L_{\mathrm{s}}=S^{p+q} \cdot p^{p} \cdot q^{q}$ (b) $L_{\mathrm{s}}=S^{p+q} \cdot p^{q} \cdot q^{p}$ (c) $L_{\mathrm{S}}=S^{p q} \cdot p^{p} \cdot q^{q}$ (d) $L_{\mathrm{s}}=S^{p q} \cdot(p q)^{p+q}$

For a sparingly soluble salt $\mathrm{A}_{\mathrm{p}} \mathrm{B}_{\mathrm{q}}$, the relationship of its solubility product $\left(L_{\mathrm{s}}\right)$ with its solubility $(S)$ is
(a) $L_{\mathrm{s}}=S^{p+q} \cdot p^{p} \cdot q^{q}$
(b) $L_{\mathrm{s}}=S^{p+q} \cdot p^{q} \cdot q^{p}$
(c) $L_{\mathrm{S}}=S^{p q} \cdot p^{p} \cdot q^{q}$
(d) $L_{\mathrm{s}}=S^{p q} \cdot(p q)^{p+q}$

Key Concepts

Solubility Product Constant

The solubility product (Ksp) is an equilibrium constant that applies to the dissolution of a sparingly soluble salt. It is defined as the product of the molar concentrations of the resulting ions, each raised to the power of its coefficient in the balanced equilibrium equation. This concept is used to describe the extent to which a salt can dissolve in solution before reaching saturation.

Dissolution Reaction Stoichiometry

Dissolution reaction stoichiometry pertains to the way in which a sparingly soluble salt dissociates into its constituent ions. For example, a salt with the formula A?B_q dissolves according to the reaction A?B_q(s) ? p A^(n+) (aq) + q B^(m-) (aq). The stoichiometric coefficients (p and q) are crucial because they determine the exponents in the solubility product expression, reflecting the molar relationship between the salt and the ions produced.

Relationship Between Solubility and Solubility Product

The relationship between the solubility (S) of a sparingly soluble salt and its solubility product is derived from the stoichiometry of its dissolution reaction. When the salt dissociates, the ion concentrations are typically proportional to S multiplied by their respective stoichiometric numbers. Therefore, the Ksp is expressed as a power function of S, where the exponents on S are the sum of the stoichiometric coefficients, effectively linking the measurable solubility of the salt to its equilibrium constant.

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