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NEET CHEMISTRYSolutionsEasy

Question

Which one is not equal to zero for an ideal solution?

A

ΔHmix\Delta H_{\text{mix}}

B

ΔSmix\Delta S_{\text{mix}}

C

ΔVmix\Delta V_{\text{mix}}

D

ΔP=PObserved−PRaoult\Delta P = P_{\text{Observed}} - P_{\text{Raoult}}

Step-by-Step Solution

For an ideal solution, it perfectly obeys Raoult's law over the entire range of concentrations, meaning the observed vapour pressure matches the pressure calculated by Raoult's law (ΔP=0\Delta P = 0). Furthermore, the intermolecular attractive forces between the components (A-B) are nearly equal to those in the pure components (A-A and B-B). This results in zero enthalpy of mixing (ΔHmix=0\Delta H_{\text{mix}} = 0) and zero volume of mixing (ΔVmix=0\Delta V_{\text{mix}} = 0). However, the mixing of two miscible liquids is a spontaneous process that leads to an increase in the randomness or disorder of the system. Therefore, the entropy of mixing is always positive (ΔSmix>0\Delta S_{\text{mix}} > 0) and is never equal to zero.

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Solutions. Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

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