(Solved): 6. Calcium hydroxide has a solubility in water at 25.0C determined by the value Ksp=4.6810 ...

6. Calcium hydroxide has a solubility in water at $25.0^{?}\mathrm{C}$ determined by the value $K_{\mathrm{sp}}=4.68\times 10^{?6}$. (a) Write the equation representing the solubility equilibrium for calcium hydroxide and construct the ICE table using initial conditions $n$ mol of the solid and no ions present. If the volume of solution is exactly $1\mathrm{L}$, what is the relation between the chemical amounts of any ions present and their molar concentrations? (b) Substitute the appropriate expressions from the E row of your ICE table into the expression for $K_{\mathrm{s}}$ and calculate the equilibrium concentrations of each of the ions in solution at $25.0^{?}\mathrm{C}$. (c) If an aqueous solution consists of $1.180\mathrm{g}$ of calcium hydroxide mixed with water to form a solution with a final volume of $1.75\mathrm{L}$, will additional calcium hydroxide dissolve in this solution? If yes, how much more calcium hydroxide (in $\mathrm{g}$ ) can dissolve before the solution reaches saturation? If no, how much solid calcium hydroxide remains undissolved?