Question

the enthalpy of solution of nacl in water is about 3.88 kj/mol. however, the solubility of nacl in water is relatively high. which statement about the entropy of the solution process explains why nacl dissolves in water even though the process is endothermic? the entropy remains the same when nacl dissolves in water entropy has nothing to do with the solution process the entropy increases when nacl dissolves in water the entropy decreases when nacl dissolves in water

Explanation:

Entropy is a measure of disorder. When NaCl dissolves in water, the ions become more dispersed in the solution compared to the solid - state. An increase in disorder means an increase in entropy. For a process to be spontaneous (like the dissolution of NaCl in water), the change in Gibbs free energy ($\Delta G$) must be negative. Since $\Delta G=\Delta H - T\Delta S$ and the process is endothermic ($\Delta H> 0$), a large enough positive $\Delta S$ (increase in entropy) can make $\Delta G < 0$.

Answer:

the entropy increases when NaCl dissolves in water