1)

When 100 mL of 1.0 M  HCl was mixed with 100mL   of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7° C was measured for the beaker and its contents (Expt. I). Because the enthalpy of neutralisation 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), 100mL  of 2.0 M  acetic acid  (Ka = 2.0 x 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° C was measured.

Enthalpy of disscociation (in KJmol-1) of acetiic acid  obtained from the Expt. 2 is 


A) 1.0

B) 10.0

C) 24.5

D) 51.4

Answer:

Option A

Explanation:

Let C JK-1 be the heat energy capacity of the calorimeter.

                        Maa of solution

             =200mL×1gmL1=200g

 Heat evolved  in Exp.I

    =   57×1000×0.1(mol)=5700J

        5700J=(200×4.2+C)×5.7

                 100=200×4.2+C  ......(i)

Let x kJ/mol  is  heat evolved in neutralisation of acetic acid.

 x×1000×0.10=(200×4.2+C)×5.6

             x×1005.6=200×4.2+C         ...........(ii)

From (i)  and (ii): x=56 kJ/mol

           Enthalpy  of ionisation of acetic acid 

                                    = -56-(-57)= 1 kJ/MOL