Sodium hydroxide is dissolved in enough water to make up a 20.0 mole% solution.
If the NaOH and water are initially at 77°F (25°C), how much heat (Btu/Ib product solution) must be removed for the solution also to be at 77°F. Assume the process is carried out at constant pressure, so that
- If the dissolution is done adiabatically, estimate the final temperature of the solution. Assume that the heat capacity of the solution is approximately that of pure liquid water.
- If the process of Part (b) were actually carried out, the final temperature would be less than the value calculated. Why? (Neglect errors caused by the assumptions of adiabatic dissolution and a solution heat capacity equal to that of pure water.)
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