Question:
For which of the following liquid mixtures \(\Delta_\text{mix} H = 0\) and \(\Delta_\text{mix} V = 0\)?
For which of the following liquid mixtures \(\Delta_\text{mix} H = 0\) and \(\Delta_\text{mix} V = 0\)?
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Ideal liquid mixtures are those where intermolecular forces of the components are similar, leading to zero enthalpy and volume changes on mixing.
Updated On: Jun 26, 2026
- ethyl chloride, ethyl bromide
- ethanol, acetone
- phenol, aniline
- chloroform, acetone
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The Correct Option is A
Solution and Explanation
Step 1: Recall definitions.
For an ideal mixture, the enthalpy of mixing (\(\Delta_\text{mix} H\)) and the volume change on mixing (\(\Delta_\text{mix} V\)) are zero.
Step 2: Identify ideal behaviour.
Ideal behaviour occurs when molecules are similar in size and intermolecular interactions (e.g., dispersion forces) are comparable.
Step 3: Analyze each mixture.
- Ethyl chloride + ethyl bromide: Both are similar in molecular size and non-polar → ideal mixture.
- Ethanol + acetone: Strong hydrogen bonding → non-ideal, \(\Delta_\text{mix} H \neq 0\).
- Phenol + aniline: Strong hydrogen bonding → non-ideal.
- Chloroform + acetone: Dipole-dipole and hydrogen bonding → non-ideal.
Step 4: Conclusion.
Only ethyl chloride and ethyl bromide form an ideal mixture with \[ \Delta_\text{mix} H = 0 \text{ and } \Delta_\text{mix} V = 0 \]
For an ideal mixture, the enthalpy of mixing (\(\Delta_\text{mix} H\)) and the volume change on mixing (\(\Delta_\text{mix} V\)) are zero.
Step 2: Identify ideal behaviour.
Ideal behaviour occurs when molecules are similar in size and intermolecular interactions (e.g., dispersion forces) are comparable.
Step 3: Analyze each mixture.
- Ethyl chloride + ethyl bromide: Both are similar in molecular size and non-polar → ideal mixture.
- Ethanol + acetone: Strong hydrogen bonding → non-ideal, \(\Delta_\text{mix} H \neq 0\).
- Phenol + aniline: Strong hydrogen bonding → non-ideal.
- Chloroform + acetone: Dipole-dipole and hydrogen bonding → non-ideal.
Step 4: Conclusion.
Only ethyl chloride and ethyl bromide form an ideal mixture with \[ \Delta_\text{mix} H = 0 \text{ and } \Delta_\text{mix} V = 0 \]
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