Heat of Neutralization of a Strong Dibasic Acid in Dilute Solution by NaOH

Introduction
Heat of neutralization is the amount of heat evolved or absorbed when one equivalent of an acid and one equivalent of a base undergo a neutralization reaction to form water and a salt. In this context, we will discuss the heat of neutralization of a strong dibasic acid in dilute solution by NaOH.

Explanation
The heat of neutralization for a strong dibasic acid in dilute solution by NaOH is nearly -13.7 kcal/eq. This means that when one equivalent of a strong dibasic acid is neutralized by one equivalent of NaOH, heat is evolved to the extent of -13.7 kcal.

The reason for the evolution of heat is due to the exothermic nature of the neutralization reaction. When an acid and a base react, the hydrogen ions from the acid combine with the hydroxide ions from the base to form water. This reaction is highly exothermic and releases energy in the form of heat.

In the case of a strong dibasic acid, two equivalents of hydrogen ions are present per molecule of acid. Therefore, when one equivalent of the acid is neutralized by one equivalent of NaOH, two moles of water are formed. This leads to a higher heat of neutralization as compared to a monobasic acid.

The heat of neutralization can be measured experimentally by using a calorimeter. The reactants are mixed in the calorimeter and the temperature change is recorded. From the temperature change and the heat capacity of the calorimeter, the heat of neutralization can be calculated.

Conclusion
In conclusion, the heat of neutralization of a strong dibasic acid in dilute solution by NaOH is nearly -13.7 kcal/eq. This is due to the exothermic nature of the neutralization reaction and the formation of two moles of water per equivalent of acid. The heat of neutralization can be experimentally determined using a calorimeter.

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