Find delta H for the dissolution of 1.00 g NaOH in water. Find delta H for the d

Question

Find delta H for the dissolution of 1.00 g NaOH in water. Find delta H for the dissolution of 1 mole NaOH in water. Given that NaOH exists as Na^+ and OH^- ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water. Given the following heats of formation, delta H_f in kJ per mole, as obtained from a table of delta H_f, data, calculate delta H for the reaction in Part (f). Compare your answer with the result you obtained in Part (e). NaOH(s), - 425.6; Na^+ (aq), -240.1; OH^-(aq), -230.0

Explanation / Answer

NaOH dissolution is exothermic, so use (-) sign for the values given at d. and e.

At f. write the equation as

NaOH(s)   = Na+(aq) + HO-(aq)

Now the answer at g. is clear:

dH = (-230) + (-240.1) – (- 425.6) = - 44.5 kJ/mol

The experimental results at e. is quite good the error is about 10%.

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