The solubility product of CaF2 is 1.08 ×10^-10. What mass of CaF2 will dissolve in 500 ml water

step 1 Hello students for this question we are given the solubility to be equal to 17 into 10 to the pe

The solubility product of CaF2 is 1.08 ×10^-10. What mass of...

The solubility product of $\mathrm{CaF}_{2}$ is $1.08$ $\times 10^{-10}$. What mass of $\mathrm{CaF}_{2}$ will dissolve in $500 \mathrm{ml}$ water in order to make a saturated solution? $(\mathrm{Ca}=40, \mathrm{~F}=19)$ (a) $3 \times 10^{-4} \mathrm{~g}$ (b) $1.17 \times 10^{-2} \mathrm{~g}$ (c) $1.17 \mathrm{mg}$ (d) $3 \times 10^{-3} \mathrm{~g}$

The solubility product of $\mathrm{CaF}_{2}$ is $1.08$ $\times 10^{-10}$. What mass of $\mathrm{CaF}_{2}$ will dissolve in $500 \mathrm{ml}$ water in order to make a saturated solution? $(\mathrm{Ca}=40, \mathrm{~F}=19)$
(a) $3 \times 10^{-4} \mathrm{~g}$
(b) $1.17 \times 10^{-2} \mathrm{~g}$
(c) $1.17 \mathrm{mg}$
(d) $3 \times 10^{-3} \mathrm{~g}$

Key Concepts

Stoichiometric Relationships in Dissolution

When a salt dissolves, it dissociates into its constituent ions in stoichiometric proportions as defined by its balanced chemical equation. Understanding these relationships is crucial for setting up the correct equilibrium expression and for converting molar solubility into the mass of the dissolved substance.

Unit Conversions

Unit conversion is essential for relating the calculated molar quantities to other units such as grams or milligrams. In solubility problems, converting between moles, liters, and grams is required to determine the practical mass of the solute that dissolves in a given volume of solvent.

Saturated Solutions and Chemical Equilibrium

A saturated solution is one in which the dissolved substance is at its maximum concentration, and the solution is in dynamic equilibrium. This means that the rate at which the compound dissolves is equal to the rate at which it precipitates out, a fundamental concept when relating the Ksp to the solubility of the salt.

Molar Solubility

Molar solubility is defined as the number of moles of a compound that can dissolve in one liter of solution to reach a state of saturation. It is directly determined from the solubility product by setting up the equilibrium expression according to the stoichiometry of the dissolution reaction, allowing the calculation of the concentration of dissolved ions.

Solubility Product (Ksp)

The solubility product is an equilibrium constant specific to the dissolution of a sparingly soluble salt. It represents the product of the molar concentrations of the ions in solution, each raised to the power of their coefficients in the balanced dissolution equation. A very low Ksp indicates that the salt has a low solubility, forming only a small amount of ions in a saturated solution.

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