A saturated solution of calcium fluoride contains 2 ×10^4 moles of the salt per litre of the sol

step 1 Dear students in problem 131 of chapter 7 we have asked that the saturated solution of calcium f

A saturated solution of calcium fluoride contains 2 ×10^4...

A saturated solution of calcium fluoride contains $2 \times$ $10^{4}$ moles of the salt per litre of the solution. Its $K_{w}$ is
(1) $8 \times 10^{-18}$
(2) $3.2 \times 10^{-11}$
(3) $4 \times 10^{-6}$
(4) $1.43 \times 10^{-9}$

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Key Concepts

Dissolution Equilibrium

Dissolution equilibrium refers to the dynamic balance established when a sparingly soluble solid dissolves to form its ions in solution. In this state, the rate at which the solid dissolves equals the rate at which the ions recombine to form the solid, and this equilibrium is expressed by an equilibrium constant.

Solubility Product Constant (Ksp)

The solubility product constant, Ksp, is the equilibrium constant for the dissolution process of a sparingly soluble salt. It is defined by expressing the product of the concentrations of the ions in solution, each raised to the power of their stoichiometric coefficients. Ksp is a measure of the salt's solubility and is essential in predicting precipitation and solubility behavior.

Stoichiometry in Equilibrium Calculations

Stoichiometry in equilibrium calculations involves using the balanced chemical equation to relate the concentration of the dissolved ions to the solubility of the compound. Correct incorporation of the stoichiometric coefficients ensures that the equilibrium expression accurately represents the relationship between the dissolved salt and its ions, which is critical when computing constants like Ksp.

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