Chapter 2, Problem 42P

Interpretation Introduction

Interpretation:

The given solvent capable of dissolving ionic compounds is to be identified.

Concept Introduction:

▸ A general rule of solubility is: like dissolves like.

▸ Polar and ionic solids are dissolved in polar solvents.

▸ Nonpolar solids are dissolved in nonpolar solvents.

▸ If a molecule has dipole moment, it is termed as polar molecule. The symmetrical molecules are non-polar because the dipole moment cancel each other.

▸ The species resistant to water or the species that are incompatible with water are termed as hydrophobic.

▸ The water loving species or the species compatible with water are termed as hydrophilic species.

▸ If the compound contains one hydrophilic group and more than six carbon atoms, then the compound is insoluble in water.

▸ Alkyl chains with high molecular weight are hydrophobic in nature.

▸ The hydroxyl group is hydrophilic in nature because it forms hydrogen bonding with water molecules.

▸ The carbonyl oxygen and hydroxyl group of carboxylic acid are hydrophilic in nature.

▸ A hydrogen bond is a partially electrostatic force of attraction between a hydrogen atom which is bound to more electronegative atom such as nitrogen, oxygen or fluorine and another atom bearing a lone pair of electron.

▸ The liquid ${\text{SO}}_{\text{2}}$ is polar due to presence of a net dipole moment and polar bonds.

▸ The liquid ${\text{NH}}_3$ is polar due to the presence of a net dipole moment and polar bonds.

▸ In benzene, the bonds are polar due to the presence of electronegativity difference between carbon and hydrogen but the dipole moment cancel out due to the symmetrical structure of benzene. The net dipole moment is zero which makes the molecule non-polar.