Final answer:
The Ksp for Ca(OH)2, based on its molar solubility of 0.022 M, is calculated to be 4.26 x 10^-5.
Step-by-step explanation:
To calculate the Ksp (solubility product constant) for Ca(OH)2 using its molar solubility, we consider the following dissolution equation:
Ca(OH)2 → Ca2+ + 2OH−
Given that the molar solubility is 0.022 M, we can determine the concentrations of ions in the solution. From the stoichiometry of the reaction, for each mole of Ca(OH)2 that dissolves, it produces one mole of Ca2+ ions and two moles of OH− ions. Therefore, the concentrations in the solution will be:
- [Ca2+] = 0.022 M
- [OH−] = 2 × 0.022 M = 0.044 M
The Ksp expression for Ca(OH)2 is:
Ksp = [Ca2+][OH−]2
Substitute the values we found:
Ksp = (0.022) × (0.044)2
Calculate the Ksp:
Ksp = (0.022) × (0.044) × (0.044) = 4.26 × 10−5