In each of the following pairs of compounds, which compound...

In each of the following pairs of compounds, which compound is likely to be more soluble in water?
a. $\mathrm{CCl}_{4}$ or $\mathrm{CHCl}_{3}$
b. $\mathrm{CH}_{3} \mathrm{OH}$ or $\mathrm{C}_{6} \mathrm{H}_{11} \mathrm{OH}$
c. NaF or MgO
d. $\mathrm{CaF}_{2}$ or $\mathrm{BaF}_{2}$

Key Concepts

Like Dissolves Like Principle

This principle states that solvents tend to dissolve solutes that share similar polarity characteristics. Polar compounds are more soluble in polar solvents, while nonpolar compounds are more soluble in nonpolar solvents. It is a fundamental concept used to predict solubility behavior in various chemical contexts.

Molecular Polarity

Molecular polarity arises from differences in electronegativity between atoms and the geometry of the molecule. The overall polarity influences how molecules interact with water, a polar solvent, with more polar molecules generally exhibiting better solubility due to stronger electrostatic interactions.

Hydrogen Bonding

Hydrogen bonding is an intermolecular force where a hydrogen atom bonded to a highly electronegative atom interacts with a lone pair of electrons on another electronegative atom. In aqueous solutions, compounds capable of forming hydrogen bonds can interact strongly with water molecules, enhancing their solubility.

Ionic Lattice Energy and Hydration Energy

For ionic compounds, solubility in water depends on the balance between lattice energy (the energy holding the ions together in the solid state) and hydration energy (the energy released when ions interact with water). A lower lattice energy or a higher hydration energy will typically result in greater solubility, guiding predictions about the dissolution of ionic solids.

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