Chapter 14

The ionic substance EJ dissociates to form \(\mathrm{E}^{2+}\) and \(\mathrm{J}^{2-}\) ions. The solubility of EJ is \(8.45 \times 10^{-6} \mathrm{mol} / \mathrm{L}\) . What is the value of the solubility-product constant?

Four lead salts and their solubility products are as follows: \(\mathrm{PbS}, 3.0 \times 10^{-28} ; \mathrm{PbCrO}_{4}, 1.8\) \(\times 10^{-14} ; \mathrm{PbCO}_{3}, 7.4 \times 10^{-14} ;\) and \(\mathrm{PbSO}_{4}, 2.5\) \(\times 10^{-8} .\) Calculate the \(\mathrm{Pb}^{2+}\) concentration in a saturated solution of each of these salts.

What is the concentration of \(\mathrm{F}^{-}\) ions in a saturated solution that is 0.10 \(\mathrm{M}\) in \(\mathrm{Ca}^{2+}\) ? The \(K_{s p}\) of \(\mathrm{CaF}_{2}\) is \(1.6 \times 10^{-10} .\)

Why might an industrial process be operated at high temperature even though the reaction is more favorable at lower temperatures?

How does temperature affect equilibrium constants?

The reaction below has an equilibrium constant of \(4.9 \times 10^{11}\) . $$\mathrm{Fe}(\mathrm{OH})_{2}(s)+2 \mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftarrows \mathrm{Fe}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l)$$ Write the equilibrium constant expression, and determine the concentration of \(\mathrm{Fe}^{2+}\) ions in equilibrium when the hydronium ion concentration is \(1.0 \times 10^{-7} \mathrm{mol} / \mathrm{L}\)

When does a pressure change affect a chemical equilibrium?

What information may be conveyed by the knowledge that the equilibrium constant of a reaction is very small?

Calculate the solubility of a substance MN that ionizes to form \(\mathrm{M}^{2+}\) and \(\mathrm{N}^{2-}\) ions given that \(K_{s p}=8.1 \times 10^{-6} .\)

A student wrote, "The larger the equilibrium constant, the greater the rate at which reactants convert to products." How was he wrong?