Solutions: Vocabulary Flashcards

Flashcards for vocabulary related to solutions, concentration, and colligative properties.

Solutions

Homogeneous mixtures of two or more components with uniform composition and properties throughout.

Solvent

The component present in the largest quantity in a solution.

Solute

One or more components present in the solution other than the solvent.

Binary Solution

A solution consisting of two components.

Concentration

Expressing the amount of solute relative to the amount of solution or solvent.

Mass Percentage (w/w)

The mass of a component in a solution divided by the total mass of the solution, multiplied by 100.

Volume Percentage (V/V)

The volume of a component divided by the total volume of the solution, multiplied by 100.

Mass by Volume Percentage (w/V)

The mass of solute dissolved in 100 mL of solution.

Parts per Million (ppm)

Number of parts of a component per million parts of the solution.

Mole Fraction

The ratio of the number of moles of a component to the total number of moles of all components in the solution.

Molarity (M)

Number of moles of solute dissolved in one liter of solution.

Molality (m)

Number of moles of solute per kilogram of solvent.

Solubility

The maximum amount of a substance that can be dissolved in a specified amount of solvent at a specified temperature.

Crystallization

The process of solute particles in solution colliding with solid solute particles and separating out of the solution.

Saturated Solution

A solution in which no more solute can be dissolved at the same temperature and pressure.

Unsaturated Solution

A solution in which more solute can be dissolved at the same temperature.

Henry's Law

At a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of the liquid or solution.

Raoult's Law

For a solution of volatile liquids, the partial vapor pressure of each component of the solution is directly proportional to its mole fraction present in the solution.

Ideal Solutions

Solutions that obey Raoult's law over the entire range of concentration.

Non-Ideal Solutions

Solutions that do not obey Raoult's law over the entire range of concentration.

Azeotropes

A constant boiling mixture

Colligative Properties

Properties that depend on the number of solute particles, irrespective of their nature, relative to the total number of particles present in the solution.

Relative Lowering of Vapor Pressure

The lowering of vapor pressure divided by the vapor pressure of the pure solvent; equal to the mole fraction of the solute.

Elevation of Boiling Point

The increase in the boiling point of a solution compared to the pure solvent.

Depression of Freezing Point

The decrease in the freezing point of a solution compared to the pure solvent.

Osmotic Pressure

The pressure that must be applied to a solution to prevent osmosis.

Isotonic Solutions

Solutions having the same osmotic pressure at a given temperature.

Hypertonic Solution

A solution having higher osmotic pressure than another solution.

Hypotonic Solution

A solution having lower osmotic pressure than another solution.

Reverse Osmosis

The flow of solvent from a solution through a semipermeable membrane when pressure larger than the osmotic pressure is applied to the solution.

Abnormal Molar Mass

Molar mass that is either lower or higher than the expected or normal value due to association or dissociation of solute.

van't Hoff Factor (i)

A factor introduced to account for the extent of dissociation or association of solutes in solution.