(Solved): 2. Calcium hydroxide is only slightly soluble in water. The reaction by which it goes into solution ...

2. Calcium hydroxide is only slightly soluble in water. The reaction by which it goes into solution is: $$\mathrm{Ca}(\mathrm{OH}{)}_2(\mathrm{s})={\mathrm{Ca}}^{2+}(\mathrm{aq})+2{\mathrm{OH}}^{?}(\mathrm{aq})$$ a. Formulate the expression for the equilibrium constant, $$K_{ip}$$, for the above reaction. b. It is possible to dissolve significant amounts of $$\mathrm{Ca}(\mathrm{OH}{)}_2$$ in solutions in which the concentration of either $${\mathrm{Ca}}^{2+}$$ or $${\mathrm{OH}}^{?}$$is kept very small. Explain, using $$K_{\text{sp }}$$ why this is the case. c. Explain why $$\mathrm{Ca}(\mathrm{OH}{)}_2$$ might have very appreciable solubility in $$1.0\mathrm{M}\mathrm{HCl}$$. [Hint: Consider the effect of Reaction 3 on the $$\mathrm{Ca}(\mathrm{OH}{)}_2$$ dissolution reaction.]