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Acetic acid ( ethanoic acid ) and hydroc...

Acetic acid `(` ethanoic acid `)` and hydrochloric acid react with `KOH` solution. The enthalpy of neutralisation of ethanoic acis is `-55.8kJ mol^(-1)` while that of hydrochloric acid is `-57.3kJ mol^(-1)` . Can you think of how are these different?`

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To understand the difference in the enthalpy of neutralization between acetic acid (ethanoic acid) and hydrochloric acid when they react with KOH, we can break down the solution into several steps: ### Step 1: Define Enthalpy of Neutralization The enthalpy of neutralization is defined as the heat change that occurs when one mole of an acid reacts with one mole of a base to form water and a salt in an aqueous solution. ### Step 2: Identify the Acids - **Acetic Acid (CH₃COOH)**: This is a weak acid. It does not completely dissociate in solution. - **Hydrochloric Acid (HCl)**: This is a strong acid. It completely dissociates in solution. ...
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The enthalpy of neutralisation of HCl by NaOH IS -55.9 kJ and that of HCN by NaOH is -12.1 kJ mol^(-1) . The enthalpy of ionisation of HCN is

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Knowledge Check

  • Which of the following reactions will have the value of enthalpy of neutralisation as -57.1"kJ mol"^(-1) ?

    A
    `CH_(3)COOH+NaOH rarr CH_(3)COONa+H_(2)O`
    B
    `HCl+NaOH rarr NaCl +H_(2)O`
    C
    `HCl+NH_(4)OHrarr NH_(4)Cl+H_(2)O`
    D
    `HCOOH+NaOH rarr HCOONa+H_(2)O`

  • The heat of neutralisation of NaOH and HCl is 57.3 kJ mol^(-1) then the amount of heat liberated if 2 moles each of NaOH and HCl are reacted is

    A
    57.3 kJ mol
    B
    114.6 kJ mol
    C
    28.65 kJ mol
    D
    215.2 kJ mol

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