Solutions Mind Map

A solution is a homogeneous mixture of two or more components, usually described using solvent, solute, and concentration terms such as mass percentage, mole fraction, molarity, molality, and parts per million.

Check whether the denominator is solution or solvent before applying the formula. Molarity changes with temperature because volume changes, while molality does not depend on solution volume.

Henry's law relates the solubility of a gas in a liquid to its partial pressure, while Raoult's law relates the vapour pressure of a volatile component in an ideal solution to its mole fraction.

Write the exact form of the law before interpreting K_H. For Raoult's law, check whether the solution is ideal and whether the component is volatile.

Vapour pressure of a solution is the pressure exerted by vapour in equilibrium with the liquid solution; addition of a non-volatile solute lowers the vapour pressure of the solvent, and liquid pairs may show ideal or non-ideal behaviour.

For deviation questions, compare intermolecular attractions first, then predict vapour pressure and boiling point trend.

Colligative properties are solution properties that depend on the number of solute particles present, not on their chemical nature, for dilute solutions.

For numerical answers, always write the selected formula, convert units, substitute values, and interpret whether molar mass or property change is being calculated.

Van't Hoff factor, i, is the ratio of observed colligative property to the calculated colligative property when the solute is assumed to neither associate nor dissociate.

Before applying i, decide whether the solute dissociates or associates. This predicts whether the observed molar mass will appear lower or higher than the normal molar mass.