Heat of neutralisation of H2C2O4 (oxalic acid) is -26 kcal mol- 1 . Hence, dissociation energy of H2C2O4leftharpoons2H++C2O42 - is :

Question

Heat of neutralisation of H2C2O4 (oxalic acid) is -26 kcal mol- 1 . Hence, dissociation energy of H2C2O4leftharpoons2H++C2O42 - is : (A) 12.3 kcal mol- 1 (B) 1.4 kcal mol- 1 (C) -13.7 kcal mol- 1 (D) -1.4 kcal mol- 1

Tardigrade Admin · Accepted Answer

H++OH- arrow H2O;Δ H=-13.7 kcal/mole Oxalic acid has two ionisable H+ ions. Hence, the expected heat of neutralization, if it behaves strong acid would have been = -13.7× 2=-27.4 kcal mol- 1 But experimental value = -26 kcal mol- 1 So dissociation enery = 1.4 kcal mol- 1 .

Q. Heat of neutralisation of $H_{2} C_{2} O_{4}$ (oxalic acid) is $- 26 k c a l m o l^{- 1}$ . Hence, dissociation energy of $H_{2} C_{2} O_{4} ⇌ 2 H^{+} + C_{2} O_{4}^{2 -}$ is :

$12.3 k c a l m o l^{- 1}$

$1.4 k c a l m o l^{- 1}$

$- 13.7 k c a l m o l^{- 1}$

$- 1.4 k c a l m o l^{- 1}$

Q. Heat of neutralisation of H2​C2​O4​ (oxalic acid) is −26kcalmol−1 . Hence, dissociation energy of H2​C2​O4​⇌2H++C2​O42−​ is :

12.3kcalmol−1

1.4kcalmol−1

−13.7kcalmol−1

−1.4kcalmol−1

H++OH−→H2​O;ΔH=−13.7kcal/mole Oxalic acid has two ionisable H+ ions. Hence, the expected heat of neutralization, if it behaves strong acid would have been = −13.7×2=−27.4kcalmol−1 But experimental value = −26kcalmol−1 So dissociation enery = 1.4kcalmol−1 .

Q. Heat of neutralisation of $H_{2} C_{2} O_{4}$ (oxalic acid) is $- 26 k c a l m o l^{- 1}$ . Hence, dissociation energy of $H_{2} C_{2} O_{4} ⇌ 2 H^{+} + C_{2} O_{4}^{2 -}$ is :

$12.3 k c a l m o l^{- 1}$

$1.4 k c a l m o l^{- 1}$

$- 13.7 k c a l m o l^{- 1}$

$- 1.4 k c a l m o l^{- 1}$