Chemistry - Ionic Equilibrium Question with Solution | TestHub

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${5.7}^{\mathrm{o}}\mathrm{C}$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$(-57.0\mathrm{ }\mathrm{k}\mathrm{J}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1})$, this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid$({\mathrm{K}}_{\mathrm{a}}=2.0\times {10}^{-5})$was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of${5.6}^{\mathrm{o}}\mathrm{C}$was measured. (Consider heat capacity of all solutions as$4.2\mathrm{ }\mathrm{J}\mathrm{ }{\mathrm{g}}^{-1}\mathrm{ }{\mathrm{K}}^{-1}$and density of all solutions as$1.0\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{m}{\mathrm{L}}^{-1}$)