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The enthalpy of neutralisation of 'NaOH'...

The enthalpy of neutralisation of 'NaOH' with 'HCl' is '57.1 kJ' while with 'CH_3COOH', it is '-55 kJ' This happens because

A

acetic'acid is an organic acid

B

acetic acid is little soluble in water

C

acetic acid is a weak acid and requires lesser sodium hydroxide for neutralisation

D

some heat, is required to ionise acetic acid completely

Text Solution

Verified by Experts

The correct Answer is:
D
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Acetic acid and hydrochloric acid react with KOH solution. The enthalpy of neutralization of acetic acid is -55.8 kJ mol^(-1) while that of hydrochloric acid is -57.3 kJ 'mol^(-1) . Why?

The enthalpy of neutralization of a weak monoprotic acid (HA) in 1 M solution with a strong base -55.95 kJ/mol. If the unionized acid is required. 1.4 kJ/mol heat for it's complete ionization and enthalpy neutralization of the strong monobasic acid.with a strong monoacidic base is -57.3 kJ/mol. What is the ionization of the weak acid in molar solution?

Knowledge Check

  • The enthalpy of neutralization of a weak monoprotic acid (HA) in 1 M solution with a strong base is -55.95 kJ/mol. If the unionized acid is required 1.4 kJ/mol heat for it's complete ionization and enthalpy of neutralization of the strong monobasic acid with a strong monoacidic base is -57.3 kJ/mol. What is the % ionization of the weak acid in molar solution?

    A
    `1 %`
    B
    `3.57 %`
    C
    `35.7%`
    D
    `10%`

  • The standard enthalpy of formation of NH_(2) is -46 kJ mol^(-1). If the enthalpy of formation of H, from its atoms is -436 kJ mol^(-1) and that of N_(2) is - 712 kJ mol^(-1). the average bond enthalpy of N-H bond in NH_(3) is:

    A
    `- 1056 kJ mol ^(-1)`
    B
    `- 1102 kJmol ^(-1) `
    C
    `- 9 64 kJ mol ^(-1)`
    D
    `+ 352 kJ mol ^(-1)`

  • The enthalpy of a reaction at 273K is-3.57 kJ: What will be the enthalpy of reaction at 373 K if Delta C = U

    A
    `-3.57`
    B
    `0`
    C
    `- 3.57 xx (373)/(273)`
    D
    `- 375`

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