Two solutions initially at `25^(@)C` were mixed in an adiabatic constant pressure calorimeter. One contains 400 ml of 0.2 M weak monoprotic acid solution. The other contain 100 ml of 0.80 M NaOH. After mixing temperature increased to `26.2^(@)C`. How much heat is evolved in the neutralization of 1 mole of acid? Assume density of solution `1.0 g//cm^(3)`, and specific heat of solution 4.2 J/g-K. Neglect heat capacity of the Calorimeter.

Answer

`-31.5` kJ/mole

Explanation

Mass= density `xx` vol. `=1xx500=500` gram
`DeltaT=1.2`
`q=mc.DeltaT=2520`
Heat released by 1 mole of acid `=2520/0.08=-31500 J=-31.5 kJ`