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The enthalpy of neutralisation of acid acid and sodium hydroxide is -55.4 KJ.What is the enthalpy ionisation of acetic acid ?
- a)-1.9 KJ
- b)+ 1.9 KJ
- c)+5.54 KJ
- d)-5.54 KJ
Correct answer is option 'B'. Can you explain this answer?
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Understanding Enthalpy of Neutralisation
The enthalpy of neutralisation refers to the heat change when an acid reacts with a base to form water and a salt. In this case, acetic acid (CH3COOH) reacts with sodium hydroxide (NaOH).
Given Data
- Enthalpy of neutralisation (ΔH_neutralisation) = -55.4 kJ/mol
Ionisation of Acetic Acid
Acetic acid is a weak acid, meaning it does not completely ionise in water. The reaction can be represented as:
CH3COOH ⇌ CH3COO⁻ + H⁺
To find the enthalpy of ionisation (ΔH_ionisation) of acetic acid, we need to relate it to the enthalpy of neutralisation. The neutralisation reaction can be represented as:
CH3COOH + NaOH → CH3COONa + H2O
Key Relationships
- The enthalpy change for neutralisation is the heat released when the weak acid (acetic acid) ionises and reacts with the strong base (sodium hydroxide).
- Since the ionisation of acetic acid absorbs energy (endothermic), it has a positive enthalpy change.
Calculation Insight
The enthalpy of neutralisation can be expressed as:
ΔH_neutralisation = ΔH_ionisation + ΔH_formation of water
Rearranging gives us:
ΔH_ionisation = ΔH_neutralisation - ΔH_formation of water
Assuming the formation of water is approximately -57.3 kJ/mol, we find:
ΔH_ionisation = -55.4 kJ + 57.3 kJ = +1.9 kJ/mol
Conclusion
Thus, the enthalpy of ionisation of acetic acid is +1.9 kJ/mol, which corresponds to option 'B'. This indicates that energy is required for the ionisation process, aligning with the characteristics of weak acids.
The enthalpy of neutralisation refers to the heat change when an acid reacts with a base to form water and a salt. In this case, acetic acid (CH3COOH) reacts with sodium hydroxide (NaOH).
Given Data
- Enthalpy of neutralisation (ΔH_neutralisation) = -55.4 kJ/mol
Ionisation of Acetic Acid
Acetic acid is a weak acid, meaning it does not completely ionise in water. The reaction can be represented as:
CH3COOH ⇌ CH3COO⁻ + H⁺
To find the enthalpy of ionisation (ΔH_ionisation) of acetic acid, we need to relate it to the enthalpy of neutralisation. The neutralisation reaction can be represented as:
CH3COOH + NaOH → CH3COONa + H2O
Key Relationships
- The enthalpy change for neutralisation is the heat released when the weak acid (acetic acid) ionises and reacts with the strong base (sodium hydroxide).
- Since the ionisation of acetic acid absorbs energy (endothermic), it has a positive enthalpy change.
Calculation Insight
The enthalpy of neutralisation can be expressed as:
ΔH_neutralisation = ΔH_ionisation + ΔH_formation of water
Rearranging gives us:
ΔH_ionisation = ΔH_neutralisation - ΔH_formation of water
Assuming the formation of water is approximately -57.3 kJ/mol, we find:
ΔH_ionisation = -55.4 kJ + 57.3 kJ = +1.9 kJ/mol
Conclusion
Thus, the enthalpy of ionisation of acetic acid is +1.9 kJ/mol, which corresponds to option 'B'. This indicates that energy is required for the ionisation process, aligning with the characteristics of weak acids.
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The enthalpy of neutralisation of acid acid and sodium hydroxide is -55.4 KJ.What is the enthalpy ionisation of acetic acid ?a)-1.9 KJb)+ 1.9 KJc)+5.54 KJd)-5.54 KJCorrect answer is option 'B'. Can you explain this answer?
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