Ionic Equilibrium

Paragraph for next 2 Questions
When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7ºC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (−57.0kJmol−1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0M acetic acid (Ka=2.0×10−5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6ºC was measured. (Consider heat capacity of all solutions as 4.2Jg−1K−1 and density of all solutions as 1.0‌gmL−1)