The enthalpy of formation of is $H_{2} O (l)$ is -290 kJ/mol and enthalpy of neutralization of strong acid with strong alkali is -56 kJ/equiv. what is the enthalpy of formation of $O H^{-} (a q) ?$ Given $Δ_{form} H (H^{+}, aq) = 0$

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-234 kJ/mol

-334 kJ/mol

-178 kJ/mol

-346 kJ/mol

answer is B.

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Detailed Solution

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); {ΔH}_{1} = - 290 kJ - - - - (1) H^{+} + {OH}^{-} \to H_{2} O; {ΔH}_{2} = - 56 kJ - - - - - (2) substracting eq . 2 from eq . 1 \frac{1}{2} H_{2} \to H^{+} (aq); ΔH = 0 ∴ \frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) \to {OH}^{-} (aq); Δ_{r} H Δ_{r} H = - 290 + 56 = - 234 kJ / mol$