Solubility product constant (Ksp) of salts of types MX, MX2 and M3 X at temperature, T are 4.0 ×

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Solubility product constant (Ksp) of salts of types MX, MX2...

Solubility product constant $\left(K_{\mathrm{sp}}\right)$ of salts of types $\mathrm{MX}, \mathrm{MX}_{2}$ and $\mathrm{M}_{3} \mathrm{X}$ at temperature, $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$, respectively. Solubilities (in $\mathrm{M}$ ) of the salts at temperature, $T$, are in the order (a) $\mathrm{MX}>\mathrm{MX}_{2}>\mathrm{M}_{3} \mathrm{X}$ (b) $\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}_{2}>\mathrm{MX}$ (c) $\mathrm{MX}_{2}>\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}$ (d) $\mathrm{MX}>\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}_{2}$

Solubility product constant $\left(K_{\mathrm{sp}}\right)$ of salts of types $\mathrm{MX}, \mathrm{MX}_{2}$ and $\mathrm{M}_{3} \mathrm{X}$ at temperature, $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$
and $2.7 \times 10^{-15}$, respectively. Solubilities (in $\mathrm{M}$ ) of the salts at temperature, $T$, are in the order
(a) $\mathrm{MX}>\mathrm{MX}_{2}>\mathrm{M}_{3} \mathrm{X}$
(b) $\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}_{2}>\mathrm{MX}$
(c) $\mathrm{MX}_{2}>\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}$
(d) $\mathrm{MX}>\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}_{2}$

Key Concepts

Solubility Product Constant (Ksp)

Ksp is the equilibrium constant for the dissolution of a sparingly soluble salt into its constituent ions in water. It quantifies how much of the salt can dissolve before the solution becomes saturated, and is dependent on the concentrations of the individual ions raised to the power of their stoichiometric coefficients in the dissolution reaction.

Molar Solubility

Molar solubility is the maximum number of moles of a solute that can dissolve in one liter of solution to form a saturated solution. It is directly related to the Ksp of the salt and varies depending on the stoichiometry of the ions produced during dissolution, leading to different solubility values even for salts with similar Ksp values.

Stoichiometry in Dissolution Reactions

The stoichiometry of the dissolution reaction dictates how many moles of ions are produced from one mole of the salt and significantly affects the relationship between the salt's molar solubility and its Ksp. When a salt dissolves, the number of ions formed (and their respective concentrations) is determined by the balanced chemical equation, which must be considered to accurately calculate the solubility.

Equilibrium Expressions

Equilibrium expressions are formulated based on the balanced dissolution equation of a salt, where the Ksp is expressed as the product of the concentrations of the ions each raised to the power of its coefficient. This method connects the solubility of a salt with its Ksp and helps in comparing different salts with varying stoichiometries.

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