Practice Problem: Solubility Product Constant Calculations

The video tutorial explains how to use solubility product constants with fluorite as an example. It covers the dissolution of fluorite into calcium and fluoride ions, and how to calculate their concentrations in a saturated solution. The tutorial then guides viewers through writing the KSP expression and calculating the solubility product value for fluorite using stoichiometry and equilibrium principles.

What is the chemical formula for fluorite?

• CaSO4

• CaF2

• CaCO3

• CaCl2

If the calcium ion concentration in a saturated solution is 2.1 * 10^-4 M, what is the fluoride ion concentration?

• 8.4 * 10^-4 M

• 1.05 * 10^-4 M

• 4.2 * 10^-4 M

• 2.1 * 10^-4 M

How many fluoride ions are produced for each calcium ion when fluorite dissolves?

• Two

• Three

• One

• Four

What is the KSP expression for fluorite?

• [Ca^2+][F^-]

• [Ca^2+]^2[F^-]

• [Ca^2+]^2[F^-]^2

• [Ca^2+][F^-]^2

What is the calculated KSP value for fluorite?

• 3.7 * 10^-10

• 3.7 * 10^-11

• 3.7 * 10^-12

• 3.7 * 10^-13