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The enthalpy of neutralization of a weak monoprotic acid, HA in 1M solution with a strong base is -55.95KJ/mol. If the unionized acid requires 1.4 KJ/mol heat for its complete ionization and enthalpy of neutralization of the strong monobasic acid with a strong monoacidic base is -57.3 kJ/mol. Then % ionization of the weak acid in molar solution is

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1.2%

3.57%

6.07%

12.01%

answer is C.

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Detailed Solution

$Δ H (neutralization) = Δ H (ionization) + Δ H_{r} (H^{+} + O H^{-} \to H_{2} O)$

$- 55.95 = Δ H_{1} - 57.3$

$- 55.95 = Δ H_{i o n i s a t i o n} = 1.35 K J / m o l$

$1.4 K J / m o l$ heat is required for ionization so, % of heat utilized by 1 M acid for

$ionization = \frac{1.35}{1.4} \times 100 = 96.43 %$

So % of ionization =100-96.43 =3.57%

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