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Answer: The standard enthalpies of formation of ions in
Chapter 6, Problem 52P(choose chapter or problem)
The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to \(H^{+}\) ions; that is, \(\Delta H_{f}^{0}\left[H^{+}(a q)\right]=0\).
(a) For the following reaction \(HCI(g)\ \xrightarrow{H_{2}O}\ H^{+} (aq)+Cl^{-}(aq)\)
\(\Delta H^{\circ}=-74.9\ \mathrm{kJ} / \mathrm{mol}\)
calculate \(\Delta H_{f}^{\circ}\) for the \(C l^{-}\) ions.
(b) Given that \(\Delta H_{f}^{\circ}\) for \(\mathrm{OH}^{-}\) ions is - 229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at \(25^{\circ} \mathrm{C}\).
Questions & Answers
QUESTION:
The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to \(H^{+}\) ions; that is, \(\Delta H_{f}^{0}\left[H^{+}(a q)\right]=0\).
(a) For the following reaction \(HCI(g)\ \xrightarrow{H_{2}O}\ H^{+} (aq)+Cl^{-}(aq)\)
\(\Delta H^{\circ}=-74.9\ \mathrm{kJ} / \mathrm{mol}\)
calculate \(\Delta H_{f}^{\circ}\) for the \(C l^{-}\) ions.
(b) Given that \(\Delta H_{f}^{\circ}\) for \(\mathrm{OH}^{-}\) ions is - 229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at \(25^{\circ} \mathrm{C}\).
ANSWER:Step 1 of 4
(a) Here, we are going to determine the standard enthalpies of formation of 
We know that,
The standard enthalpy change , is defined as the difference between the enthalpies of the products and the enthalpies of the reactants.
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