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The enthalpy of neutralization is about ...

The enthalpy of neutralization is about 57.3 kJ for the pair

A

`HCl and NH_(4)OH`

B

`NH_(4)OH and HNO_(3)`

C

HCl and NaOH

D

`CH_(3)COOH and NaOH`

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the enthalpy of neutralization, we need to understand the concept of enthalpy changes during neutralization reactions. Here is a step-by-step solution: ### Step-by-Step Solution: 1. **Understanding Enthalpy of Neutralization**: The enthalpy of neutralization is the heat change that occurs when an acid and a base react to form water and a salt. For strong acids and strong bases, this value is typically around -57.3 kJ/mol. 2. **Identifying Strong and Weak Acids/Bases**: - Strong acids (like HCl) completely dissociate in water. - Strong bases (like NaOH) also completely dissociate in water. - Weak acids (like CH3COOH) and weak bases (like NH4OH) do not completely dissociate. 3. **Analyzing the Given Pairs**: - If both the acid and base are strong, the enthalpy of neutralization will be approximately -57.3 kJ. - If one of the reactants is a weak acid or a weak base, some of the heat released during the reaction is used for the ionization of the weak component, resulting in a lower enthalpy of neutralization. 4. **Applying to the Given Example**: - In the case of HCl (strong acid) and NH4OH (weak base), the enthalpy of neutralization will be less than -57.3 kJ because NH4OH does not completely ionize. - Similarly, if we consider other pairs like CH3OH (weak acid) and NH4OH (weak base), the enthalpy will also be less than -57.3 kJ. 5. **Conclusion**: - For strong acid and strong base pairs, the enthalpy of neutralization is around -57.3 kJ. - For weak acid or weak base combinations, the enthalpy will be lower than -57.3 kJ. ### Final Answer: The enthalpy of neutralization for combinations where at least one component is weak will be less than -57.3 kJ.
To solve the question regarding the enthalpy of neutralization, we need to understand the concept of enthalpy changes during neutralization reactions. Here is a step-by-step solution: ### Step-by-Step Solution: 1. **Understanding Enthalpy of Neutralization**: The enthalpy of neutralization is the heat change that occurs when an acid and a base react to form water and a salt. For strong acids and strong bases, this value is typically around -57.3 kJ/mol. 2. **Identifying Strong and Weak Acids/Bases**: ...
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Acetic acid (ethanoic acid) and hydrochloric acid react withh KOH solution. The enthalpy of neutralization of ethanoic acid is -55.8 kJ mol^(-1) while that of hydrochloric acid is -57.3 kJ mol^(-1) . Can you think of how are these different?

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

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 required 1.4 KJ/mol heat for it's comptate ionzatation and enthalpy of netralization of the strong monobasic acid with a strong monoacidic base is -57.3 KJ/mol . What is the % ionzation of the weak acid in molar solution ?

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

  • For salt of strong acid with strong base heat of neutralization is -57.3 kJ . For the formation of 0.9 kg H_(2)O how much heat is liberated?

    A
    2865 kJ
    B
    28.66 kJ
    C
    89.30 kJ
    D
    2800 kJ

  • In which of the following pairs the enthalpy of neutralization is less than or more than the standard value

    A
    `HNO_(3) and NaOH`
    B
    `HCl and NaOH`
    C
    `HCN and NaOH`
    D
    `H_(2)SO_(4) and NaOH`

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    When the aqueous solution of 0.5 mole HNO_(3) is mixed with the 0.3 mole of OH^(-) solution, then what will be the liberated heat (Enthalpy of neutralization is = 57.1 kJ)

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