The standard enthalpy of neutralization of with is -51.46 kJ/mol, while that of with is -55.90 kJ/mo — Thermodynamics and Thermochemistry Chemistry Question
Question
The standard enthalpy of neutralization of $NH_4OH$ with $HCl$ is -51.46 kJ/mol, while that of $NaOH$ with $HCl$ is -55.90 kJ/mol. Determine the exact standard enthalpy of ionization of $NH_4OH$ in aqueous medium.
Answer: A
💡 Solution & Explanation
Neutralization of strong acids and bases inherently releases 55.90 kJ/mol. For a weak base like $NH_4OH$, a fraction of this energy is strictly consumed to ionize it prior to neutralization. $\Delta H_{ionization} = \Delta H_{neut}(weak) - \Delta H_{neut}(strong) = -51.46 - (-55.90) = +4.44$ kJ/mol.
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