Question

Heat of neutralization of oxalic acid is $ - 106.7kJ/mol$ using $NaOH$ hence $\Delta H$ of ${H_2}{C_2}{O_4} \to {C_2}{O_4}^{2 - } + 2{H^ + }$ is,
1) $5.88KJ$
2) $ - 5.88KJ$
3) $ - 13.7kCal$
4) $7.5KJ$

Answer 1

Hint: We know that the Enthalpy of neutralization is consistently steady for a solid acid and a solid base: this is on the grounds that every single solid acid and solid base are totally ionized in a weak arrangement. Enthalpy changes in neutralization are consistently adverse when acid and salt respond, heat is given out.

Complete answer:
We need to remember that the enthalpy of neutralization is the adjustment of enthalpy that happens when one likes acid and a base goes through a neutralization response to shape water and a salt. It is an exceptional instance of the enthalpy of response. It is characterized as the energy delivered with the development of 1 mole of water.
At the point when a response is done under standard conditions at the temperature of \[298K\] and one atm of pressing factor and one mole of water is framed it is known as the standard enthalpy of neutralization.
Oxalic acid has two ionisable ${H^ + }$ . Subsequently, anticipated warmth of neutralization, in the event that it acts as a solid acid. It is given in the data that Heat of neutralization of oxalic acid is \[-{\text{ }}53.35kJ/mol\] utilizing $NaOH$. Consequently $\Delta H$ \[{H_2}{C_2}{O_4} \leftrightharpoons {C_2}{O_2}^{ + 4} + 2{H^ + }\] is \[7.9kJ\].

Consequently the right answer is D.

Note:
We need to know that the warmth is advanced during neutralization of an acid with antacid. The neutralization response of a solid acid with a solid base is basically the mix of one likeness hydrogen particles with one likeness hydroxyl particles.
Enthalpy of neutralization is the warmth advanced when one gram likeness the acid is totally killed by a base in weakened arrangement.
The compound response is given underneath.
\[{H^ + } + O{H^-} \to {H_2}O + 13.7kcal\]
\[{H^ + }\left( {aq} \right) + C{l^-}\left( {aq} \right) + N{a^ + }\left( {aq} \right) + O{H^-}\left( {aq} \right){\text{ }} \to {\text{ }}Na + \left( {aq} \right) + C{l^-}\left( {aq} \right) + {H_2}O + 13.7kcal\]\[13.7kcal\] of warmth is freed out and is the warmth of neutralization for every single solid acid and bases. Hess in \[1840\] acquired a consistent worth of \[13.7kcal\] as the warmth of neutralization in practically every one of the instances of solid acids and solid bases. This consistency of warmth of neutralization of a solid acid and solid base is clarified based on ionic hypothesis.