Using the Thermodynamic Data Provided Below, Calculate the Standard Change

Multiple Choice

Using the thermodynamic data provided below, calculate the standard change in entropy when one mole of sodium sulfate is dissolved in water. $\begin{array}{|l|c|}\hline & \mathrm{S}^{\circ}(\mathrm{J} / \mathrm{K} \cdot \mathrm{~mol}) \\\hline \mathrm{Na}_{2} \mathrm{SO}_{4}(s) & 149.49 \\\hline \mathrm{Na}^{+}(a q) & 60.25 \\\hline \mathrm{SO}_{4}{ }^{2-}(a q) & 17.15 \\\hline\end{array}$ Will the solubility of sodium nitrate increase or decrease if the temperature of the system is increased

A) -11.84 J/K·mol; solubility decreases with increasing temperature
B) -11.84 J/K·mol; solubility increases with increasing temperature
C) 11.84 J/K·mol; solubility decreases with increasing temperature
D) 11.84 J/K·mol; solubility increases with increasing temperature
E) None of the above