How to Determine the Ksp of Calcium Phosphate in a Saturated Solution

What is the Ksp of Ca3(PO4)2 in a saturated solution with a PO4^3- ions concentration of 3.3 × 10^(-7)?

A. 1.32 × 10^(-31) B. 1.32 × 10^(-32) C. 1.32 × 10^(-33) D. 1.32 × 10^(-34)

Answer:

The Ksp of Calcium Phosphate can be determined by raising the concentration of PO4^-3 ions and Ca^2+ ions, as per their stoichiometry in the balanced dissolution equation, to their respective coefficients, and multiplying the results. With a given PO4^-3 ions concentration of 3.3 x 10^(-7), the Ksp will be approximately 1.32 x 10^(-32).

Calcium Phosphate (Ca3(PO4)2) is a compound with a specific solubility product constant (Ksp) that determines its maximum solubility in a solution. In a saturated solution where the concentration of PO4^3- ions is 3.3 × 10^(-7), we can calculate the Ksp of Calcium Phosphate based on the balanced dissolution equation and stoichiometry.

The balanced dissolution equation for Calcium Phosphate is: Ca3(PO4)2(s) ⇌ 3Ca^2+(aq) + 2PO4^3-(aq). This equation shows the molar ratios between the ions in the solution.

Since the stoichiometry indicates that the concentration of Ca^2+ ions is 3 times that of the PO4^3- ions and 3^2 = 9 times, we can use this information to calculate the Ksp. By raising the concentrations of Ca^2+ and PO4^3- ions to their respective coefficients and multiplying the results, we arrive at a Ksp value of approximately 1.32 x 10^(-32).

Understanding how to determine the Ksp of Calcium Phosphate in a saturated solution provides valuable insight into the compound's solubility characteristics and helps in predicting its behavior in different chemical environments.