If $H^{+} + O H^{-} \to H_{2} O . Δ H = - 57.3 k J,$ then the heat of neutralisation for complete neutralisation of 1 mole $H_{2} S O_{4}$ by a base is:

-57.3 KJ

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-114.6 KJ

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-28.65 KJ

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-14.3 KJ

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Solution

The correct option is A -114.6 KJ
$H_{2} S O_{4} \to 2 H^{+} + S O {_{4}}^{2 -}$
for 2 moles of $H^{+}$ 2 x (-57.3) kJ heat i.e. -114.6 KJ heat
Thus 114.6 KJ heat will be evolved

Option B is correct.

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