When 100 mL of `1.0 M HCl` was mixed with `100` mL of `0.1 M NaOH` in an insulated beaker at constant pressure, a temperature increase of `5.7^(@)C` was measured for the beaker and its contents. Because the enthypy of neutralization of a strong acid with a strong base is a constant `(-57.0" kJ mol"^(-1))`, this experiment could used to measure the calorimeter constant.
In a second experiment `100` mL of `2.0 M` acetic acid `(K_(a)=2.0xx10^(-5))` was mixed with `100` mL of `1.0 M NaOH` (under identical conditions of Expt. 1) where a temperature rise of `5.6^(@)C` was measured.
(Consider heat capacity of all solutions as `4.2 J g^(-1) K^(-1)` and density of all solutions as `1.0 g mL^(-1)`)
Enthalpy of dissociation (in kJ `mol^(-1)`) of acetic acid from the Expt. 2 is
A. `1.0`
B. `10.0`
C. `24.5`
D. `51.4`
