Solubility

What is solubility?

• The ability of a solute to change its state.

• The amount of solute that can dissolve in a solvent at a given temperature and pressure.

• The process of mixing two liquids together.

• The temperature at which a solute can no longer dissolve.

Which solute does not increase in solubility as temperature rises?

• Sodium chloride (NaCl)

• Sugar (C12H22O11)

• Ammonia (NH3)

• Calcium carbonate (CaCO3)

What is the effect of pressure on the solubility of gases?

• Increasing pressure decreases the solubility of gases in liquids.

• Increasing pressure has no effect on the solubility of gases in liquids.

• Increasing pressure increases the solubility of gases in liquids.

• Increasing pressure only affects the solubility of solids, not gases.

What is the significance of the solubility product constant (Ksp)?

• Ksp indicates the boiling point of a solution.

• Ksp is a constant that indicates the solubility of a sparingly soluble ionic compound in a saturated solution.

• Ksp measures the pH level of a solution.

• Ksp determines the color of a solution.

What is a saturated solution?

• A solution that contains more solute than can be dissolved at a given temperature.

• A solution in which no more solute can dissolve at a given temperature.

• A solution that has reached its boiling point.

• A solution that contains only one type of solute.

What is a solution?

• A heterogeneous mixture of different substances.

• A homogeneous mixture made up of solutes and solvents.

• A pure substance with a fixed composition.

• A mixture that cannot be separated by physical means.

What is the difference between ionic and covalent solutes?

• Ionic solutes do not dissociate into ions in solution, while covalent solutes do.

• Ionic solutes dissociate into ions in solution, while covalent solutes do not.

• Both ionic and covalent solutes dissociate into ions in solution.

• Covalent solutes are always soluble in water, while ionic solutes are not.

What factors affect the rate of solubility?

• Temperature, surface area of the solute, and agitation (stirring)

• Concentration of the solute, pressure, and color

• Type of solvent, size of the container, and light exposure

• pH level, electrical conductivity, and viscosity

What are hydrogen bonds?

• Weak attractions between a slightly positive hydrogen atom in a polar molecule and a negatively charged atom.

• Strong attractions between hydrogen atoms in non-polar molecules.

• Covalent bonds formed between hydrogen and oxygen atoms.

• Ionic bonds between hydrogen and other elements.

What is an example of a polar solvent?

• Water

• Oil

• Hexane

• Chloroform