Question

If $H^{+}+O{H}^{-}\leftrightharpoons H_{2}O+13.7Kcal$, then heat of complete neutralisation of one gram mole of $H_{2}S{O}_4$ with strong base will be:

• A. 13.7 Kcal
• B. 27.4 Kcal
• C. 6.85 Kcal
• D. 3.425 Kcal

Answer 1

The correct option is B 27.4 Kcal

If $H^{+}+O{H}^{-}\leftrightharpoons H_{2}O+13.7Kcal$, then heat of complete neutralisation of one gram mole of $H_{2}S{O}_4$ with strong base will be 27.4 Kcal.

$H_{2}S{O}_4\leftrightharpoons 2H^{+}+S{O}_4^{2-}$

$2H^{+}+2O{H}^{-}\leftrightharpoons 2H_{2}O+27.4Kcal$

$13.7\times 2=27.4$

Note: Complete neutralisation of one gram mole of $H_{2}S{O}_4$ with strong base corresponds to reaction of 2 protons with 2 hydroxide ions.