The heat of dissolution of NaOH is:

$\mathbf{\u2206}{\mathbf{H}}_{\mathbf{dissolution}}\mathbf{=}\mathbf{887}\mathbf{}\raisebox{1ex}{$\mathbf{kJ}$}\!\left/ \!\raisebox{-1ex}{$\mathbf{mol}$}\right.\mathbf{-}\mathbf{932}\mathbf{}\raisebox{1ex}{$\mathbf{kJ}$}\!\left/ \!\raisebox{-1ex}{$\mathbf{mol}$}\right.\phantom{\rule{0ex}{0ex}}\mathbf{\u2206}{\mathbf{H}}_{\mathbf{dissolution}}\mathbf{=}\mathbf{-}\mathbf{45}\mathbf{}\raisebox{1ex}{$\mathbf{kJ}$}\!\left/ \!\raisebox{-1ex}{$\mathbf{mol}$}\right.$

Sodium hydroxide (NaOH) has a lattice energy of -887 kJ/mol and a heat of hydration of -932 kJ/mol.

How much solution could be heated to boiling by the heat evolved by the dissolution of 24.5 g of NaOH? (For the solution, assume a heat capacity of 4.0 J/g^{o}C, an initial temperature of 25.0 ^{o}C, a boiling point of 100.0 ^{o}C, and a density of 1.05 g/mL.)

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