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

The pH of the solution after Expt.2 is

Question

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.1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant $(- 57.0 k J m o l^{- 1})$ , this experiment could be used to measure the calorimeter constant.

In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid $(K_{a} = 2.0 \times 10^{- 5})$ was mixed with 100mL of 1.0 M NaOH(under identical conditions to Expt.1) where a temperature rise of 5.6°C was measured.

(Consider heat capacity of all solutions as $4.2 J g^{- 1} K^{- 1}$ and density of all solutions as $1.0 g m L^{- 1}$

The pH of the solution after Expt.2 is

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