Solubility and Solution Formation Quiz

Water is known as the universal solvent due to its ability to dissolve a wide range of substances.

Dissolution is the process where a solid substance mixes evenly with a liquid to form a solution.

Condensation is the transition of a gas phase into a liquid phase.

A saturated solution is in equilibrium with undissolved solute at a given temperature.

A concentrated solution contains a relatively high amount of solute compared to the amount of solvent.

Pressure has a direct impact on the solubility of gases in liquids; increasing pressure typically increases solubility.

'Like dissolves like' refers to the tendency of substances with similar polarity to dissolve in each other.

A saturated solution contains the maximum amount of solute that can dissolve at a given temperature.

Pressure generally has minimal effect on the solubility of solid solutes in liquid solvents.

Molarity is calculated by dividing the moles of solute by the volume of solution in liters.

The size of gas particles does not significantly influence their solubility in liquids.

Decreasing temperature usually slows down dissolution processes.

Miscible liquids can dissolve completely in each other to form a single phase.

According to Henry's law, solubility of gases in liquids is directly proportional to the pressure exerted on the gas.

Henry's law explains how the concentration of a gas in a liquid is directly proportional to the partial pressure of that gas.

Colligative properties such as boiling point elevation and freezing point depression depend on the number of solute particles in solution, not their identity.

C6H14 is a nonpolar molecule and is least likely to dissolve in water, which is a polar solvent.