Three hypothetical sparingly soluble salts, \(\text{MX}(s)\), \(\text{MX}_2(s)\), and \(\text{M}_2\text{X}_3(s)\), each have an identical solubility product constant of \(K_{sp} = 1.0 \times 10^{-10}\) at \(298 \text{ K}\). Which of the following correctly ranks the molar solubility, \(s\), of the three salts in pure water at \(298 \text{ K}\) from greatest to least, and provides the correct justification?