A student evaluating mineral deposits in a heated water-treatment line studies the hypothetical sparingly soluble salt \(\text{MX(s)}\). At each temperature, excess solid is allowed to reach equilibrium with pure water according to the following equation.

\(\text{MX(s)} \rightleftharpoons \text{M}^{2+}\text{(aq)}+\text{X}^{2-}\text{(aq)}\)

Quantity	Value
\(\Delta H^\circ_{\text{soln}}\)	\(+60.0\text{ kJ mol}^{-1}\)
\(\Delta S^\circ_{\text{soln}}\)	\(+80.0\text{ J mol}^{-1}\text{ K}^{-1}\)

Assume that \(\Delta H^\circ_{\text{soln}}\) and \(\Delta S^\circ_{\text{soln}}\) remain constant from \(298\text{ K}\) to \(318\text{ K}\). Which statement correctly compares the equilibrium molar solubility at \(318\text{ K}\) with that at \(298\text{ K}\) and justifies the comparison?