Chapter 17, Problem 115IE

\Interpretation: The solubility product constant, $K_{sp}$ for a saturated solution of $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ that is titrated against the given concentration of $\text{HCl}$ is to be calculated and the reason for any deviation in this value is to be determined.

Interpretation Introduction

Concept introduction: Double the number of moles of base than the acid is required for titration when the acid is monoprotic and base is dibasic to reach the equivalence point. Moreover the value of $K_{sp}$ depends on the temperature at which titration takes place.

To determine: The $K_{sp}$ for $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ in its given saturated sample that is titrated with $\text{HCl}$ and the reason for difference in calculated $K_{sp}$ and that given in Appendix D.