When `100 ML` of `1.0 M HCl` was mixed `100 MI` of `1.0 M NaOH` in an insulated beakertat constant pressure, a temperature incease of `5.7^(0)C` was measured for the beaker and its contents (Expt.1) Because th enthalpy of neutralization of a c `5.7^(0)C` strong acid with a strong base is constant `(-57.0 kJ moL- I)`, 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 xx 10^(-5))` was mixed with `100 ML` of `1.0 m NaOH` (under identical conditions to Expt. 1) Where a temperature rise of `5.0^(0)C` was measured. (Consider heat capcity of all solution as `4.2 Jg^(-1)` and density of all solution as `1.0 gmL^(-1)`) The `p^(H)` of the solution after Expt.2 isA. `2.8`B. `4.7`C. `5.0`D. `7.0`

When `100 ML` of `1.0 M HCl` was mixed `100 MI` of `1.0 M NaOH` in an

1.	When `100 ML` of `1.0 M HCl` was mixed `100 MI` of `1.0 M NaOH` in an insulated beakertat constant pressure, a temperature incease of `5.7^(0)C` was measured for the beaker and its contents (Expt.1) Because th enthalpy of neutralization of a c `5.7^(0)C` strong acid with a strong base is constant `(-57.0 kJ moL- I)`, 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 xx 10^(-5))` was mixed with `100 ML` of `1.0 m NaOH` (under identical conditions to Expt. 1) Where a temperature rise of `5.0^(0)C` was measured. (Consider heat capcity of all solution as `4.2 Jg^(-1)` and density of all solution as `1.0 gmL^(-1)`) The `p^(H)` of the solution after Expt.2 isA. `2.8`B. `4.7`C. `5.0`D. `7.0`
Answer» Correct Answer - B

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100ml of 0.1M `H_(3)PO_(4)` is titrated with 0.05 M NaOH solution till 2nd equivalent point. Then, resultant solution was mixed with 10 ml of 0.5 MHCI solution `K_(1)=10^(-3)M` `K_(2)=10^(-8)M` `K_(3)=10^(-13)M` pH at 2nd equivalent point will be :A. `5.5`B. `10.5`C. `8`D. `7`
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