The solubility of Li3 Na3(AlF6)2 is 0.0744 g per 100 ml at 298 K. Calculate the solubility pro

step 1 So this question asks us to calculate the solubility product constant, KSP of 2 compound. The fi

The solubility of Li3 Na3(AlF6)2 is 0.0744 g per 100 ml at...

The solubility of $\mathrm{Li}_{3} \mathrm{Na}_{3}\left(\mathrm{AlF}_{6}\right)_{2}$ is $0.0744 \mathrm{~g}$ per $100 \mathrm{ml}$ at $298 \mathrm{~K}$. Calculate the solubility product of the salt. (Atomic masses: $\mathrm{Li}=7, \mathrm{Na}=23, \mathrm{Al}=27, \mathrm{~F}=19)$ (a) $2.56 \times 10^{-22}$ (b) $2 \times 10^{-3}$ (c) $7.46 \times 10^{-19}$ (d) $3.46 \times 10^{-12}$

The solubility of $\mathrm{Li}_{3} \mathrm{Na}_{3}\left(\mathrm{AlF}_{6}\right)_{2}$ is
$0.0744 \mathrm{~g}$ per $100 \mathrm{ml}$ at $298 \mathrm{~K}$. Calculate the solubility product of the salt. (Atomic masses: $\mathrm{Li}=7, \mathrm{Na}=23, \mathrm{Al}=27, \mathrm{~F}=19)$
(a) $2.56 \times 10^{-22}$
(b) $2 \times 10^{-3}$
(c) $7.46 \times 10^{-19}$
(d) $3.46 \times 10^{-12}$

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Key Concepts

Solubility Product (Ksp)

The solubility product is an equilibrium constant that quantifies the maximum concentration of ions in a saturated solution of a sparingly soluble salt. It is defined as the product of the molar concentrations of the dissociated ions, each raised to the power of its stoichiometric coefficient in the dissolution equation.

Dissolution Equilibrium

This concept refers to the dynamic equilibrium established when a salt dissolves in water and dissociates into its constituent ions. At equilibrium, the rates of the dissolution and precipitation processes are equal, and the ion concentrations remain constant, which is expressed through the Ksp.

Molar Mass Calculation

Determining the molar mass of a compound is essential for converting solubility provided in mass per volume into molar concentration. This conversion is critical for linking the measured solubility to the concentrations used in the solubility product (Ksp) expression.

Stoichiometry of Dissociation

This involves understanding the ratio in which an ionic compound dissociates into its respective ions. Knowing the stoichiometric coefficients enables the proper formulation of the Ksp expression by relating the molar solubility of the compound to the individual concentrations of the dissolved ions.

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