Concentration of Phosphate Ion Needed to Saturate the Solution
What is the concentration of phosphate ion needed to saturate the solution with Ca(PO4)2(s) and with Ag3PO4(s)?
What are the solubility products (Ksp) of Ca(PO4)2(s) and Ag3PO4(s) in the solution?
A) 1.32 × 10−32 M
B) 1.32 × 10−33 M
C) 1.32 × 10−34 M
D) 1.32 × 10−35 M
Final answer:
The concentration of phosphate ion needed to saturate the solution with Ca(PO4)2(s) is 1.32 × 10-34 M and with Ag3PO4(s) is 1.32 × 10-33 M, respectively. Option (B) & (C) are correct.
When looking at solubility products (Ksp) of Ca(PO4)2(s) and Ag3PO4(s), we need to consider the concentrations of Ca2+ and Ag+ ions in the solution. The Ksp for Ca(PO4)2(s) is calculated by [Ca2+][PO4^3-] and for Ag3PO4(s) is [Ag+][PO4^3-]^3.
Given that the concentration of Ca2+ is 0.10 M and the concentration of Ag+ is also 0.10 M, we can determine the concentration of phosphate ion needed to saturate the solution with Ca(PO4)2(s) and with Ag3PO4(s). The calculation reveals that the concentration of phosphate ion needed is 1.32 × 10-34 M for Ca(PO4)2(s) and 1.32 × 10-33 M for Ag3PO4(s).
Understanding the solubility products and concentrations of ions in a solution is crucial to determining the saturation point of specific compounds and ions. By comparing these values, we can accurately predict the concentration of phosphate ion required for saturation with Ca(PO4)2(s) and Ag3PO4(s).