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Ionic Equilibrium question

2015 · Shift 2 · Q6

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JEE Advanced
Chemistry
Ionic Equilibrium
2015 · Shift 2 · Q6

Ionic Equilibrium question

2015 · Shift 2 · Q6

JEE AdvancedChemistryIonic EquilibriumMultiple correct+4 / −2

Paragraph 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 5.7o 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 constant (-57.0 kJ/mol), this 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

\times

10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6o C was measured. (Consider heat capacity of all solutions as 4.2 J/gK and density of all solutions as 1.0 g m/L) Question Enthalpy of dissociation (in kJ/mol) of acetic acid obtained from the Expt. 2 is

A
1.0
B
10.0
C
24.5
D
51.4

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