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 0.7oC 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 (-57.0 kJ mol-1), the experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH. (under identical conditions of Expt.1) where the temperature rise of 5.6oC was measured.

(Consider heat capacity of all solutions as 4.2Jg-1 K-1 and density of all solutions as 1.0 m mL-1)

Enthalpy of dissociation (in kJ mol-1) of acetic acid obtained from Expt. 2 is.

(A) 1.0

(B) 10.0

(C) 24.5

(D) 51.4

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