Questions: Using the value of -56.3 kJ as the standard enthalpy change for the reaction H^+(aq) + OH^-(aq) -> H2O(l) Calculate the standard enthalpy of change for the reaction HF(aq) -> H^+(aq) + F^-(aq) Be sure your answer has the correct number of significant digits. kJ/mol

Solution Steps

We are given the standard enthalpy change for the reaction: \[ \mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l) \] which is \(-56.3 \, \text{kJ/mol}\).

We need to calculate the standard enthalpy change for the reaction: \[ \mathrm{HF}(a q) \rightarrow \mathrm{H}^{+}(a q) + \mathrm{F}^{-}(a q) \]

Hess's Law states that the total enthalpy change for a reaction is the sum of the enthalpy changes for the individual steps of the reaction. However, we need additional information such as the enthalpy of formation for HF and the enthalpy of formation for the ions involved to proceed with the calculation.

Since we do not have the necessary additional data (enthalpy of formation for HF and the ions), we cannot calculate the standard enthalpy change for the given reaction with the provided information alone.

Final Answer