SOLUTIONS CHEMISTRY QUIZ

Colligative properties depend only on the number of particles of solute in a solution and not on their identity. Vapor pressure lowering, boiling point elevation, and freezing point depression are colligative properties, while mixture composition is not.

An abnormal colligative property refers to a deviation from what is predicted by Raoult's Law. This can include unexpected changes in boiling point, freezing point, or vapor pressure of the solution due to specific solute-solvent interactions.

Raoult's Law is used to explain the vapor pressure of solutions and the colligative properties of solutes. It relates the vapor pressure of a solution to the mole fraction of the solvent and the vapor pressure of the pure solvent.

1 part per million (ppm) of fluoride ions in water prevents tooth decay. It also notes that higher concentrations can cause the tooth to become mottled and that extremely high concentrations are poisonous.

Brass, which is a mixture of copper and zinc, is an example of a solid solution because it is a homogeneous mixture of two or more solid metals.

Ideal solutions obey Raoult's law, while non-ideal solutions do not. This distinction is based on the interactions between particles in the solution; ideal solutions have similar interactions between all particles, while non-ideal solutions have varying interactions which cause deviations from Raoult's law.

An abnormal colligative property is one that deviates from the predictions made by Raoult's law. This could be due to the formation of associations or dissociations in the solution, which alters the number of particles in the solution compared to what would be expected from the amount of solute dissolved.

Colligative properties are those properties of solutions that depend on the ratio of the number of solute particles to the number of solvent molecules in a solution and not on the nature of the chemical species present.

Henry's law states that at a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.

Concentration of solutions can be expressed in various units including moles per liter (molarity), grams per milliliter (mass/volume percentage), and parts per million (ppm), all of which are valid units for expressing the concentration of a solution.

Ideal solutions follow Raoult's law, which states that the partial vapor pressure of each component is directly proportional to its mole fraction in the solution. Non-ideal solutions deviate from this law due to interactions between the molecules that are different from those in the pure substances.

a solution composed of a gas dissolved in a liquid is classified as a liquid solution.

Air is a mixture of oxygen and nitrogen gases, among others, which makes it an example of a gas dissolved in a gas.

The mass percentage is calculated by the formula the mass of the component divided by the total mass of the solution, multiplied by 100.