Based on the predominant intermolecular forces, which of the...

Based on the predominant intermolecular forces, which of the following pairs of liquids are likely to be miscible? (a) $\mathrm{H}_{2} \mathrm{SO}_{4}$ and $\mathrm{H}_{2} \mathrm{O}$ (b) $\mathrm{C}_{8} \mathrm{H}_{18}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$ (c) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$ (d) $\mathrm{CS}_{2}$ and $\mathrm{CCl}_{4}$

Based on the predominant intermolecular forces, which of the following pairs of liquids are likely to be miscible?
(a) $\mathrm{H}_{2} \mathrm{SO}_{4}$ and $\mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{C}_{8} \mathrm{H}_{18}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$
(c) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$
(d) $\mathrm{CS}_{2}$ and $\mathrm{CCl}_{4}$

Key Concepts

Like Dissolves Like Principle

The 'like dissolves like' principle states that substances with similar polarities and types of intermolecular forces are more likely to be miscible. This concept is fundamental in predicting solubility, as polar solvents tend to dissolve polar substances, and non-polar solvents tend to dissolve non-polar substances.

London Dispersion Forces

London dispersion forces are weak, transient forces that arise from momentary fluctuations in electron density in molecules, affecting all molecules regardless of their polarity. They are the predominant interactions in non-polar substances and play a crucial role in the miscibility of non-polar liquids.

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules, including hydrogen bonding, dipole-dipole interactions, and London dispersion forces. These forces dictate many properties of substances, including their boiling points, viscosity, and miscibility. Understanding these forces is essential for predicting how different liquids interact with one another.

Hydrogen Bonding

Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when a hydrogen atom, which is covalently bonded to an electronegative atom like oxygen or sulfur, interacts with a lone pair on another electronegative atom. This force notably enhances miscibility between substances capable of hydrogen bonding.

Polarity

Polarity refers to the distribution of electrical charge within a molecule, which creates a dipole moment. Polar molecules have distinct ends with partial positive and negative charges, leading to strong intermolecular attractions with other polar molecules. This matching of polarity is a key factor in determining miscibility among liquids.

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