When 100 mL of 1.0 M HCl was mixed 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase 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 kJmol^(-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)=2.0xx10^(-5)) was mixed with 100 mL of 1.0 M NaOH (under indentical conditions to Expt. 1) where a temperature rise of 5.6^(@)C was measured (Consider heat capacity of all solutions as 4.2 Jg^(-1)K^(-1) and density of al solutions as 1.0 gmL^(-1))The pH of the solution after Expt. 2 is

When 100 mL of 1.0 M HCl was mixed 100 mL of 1.0 M NaOH in an insulate

1.	When 100 mL of 1.0 M HCl was mixed 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase 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 kJmol^(-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)=2.0xx10^(-5)) was mixed with 100 mL of 1.0 M NaOH (under indentical conditions to Expt. 1) where a temperature rise of 5.6^(@)C was measured (Consider heat capacity of all solutions as 4.2 Jg^(-1)K^(-1) and density of al solutions as 1.0 gmL^(-1))The pH of the solution after Expt. 2 is
Answer» `2.8` `4.7` `5.0` `7.0` Solution :Final solution contain 0.1 mole of `CH_(3)COOH` and `CH_(3)COONA` each HENCE it is BUFFER solution `pH=pK_(a)+log.([CH_(3)COO^(-)])/([CH_(3)COOH])=5-log2+log.(0.1)/(0.1)=4.7`