The substance being dissolved

The substance doing the dissolving

The ability of a solute to dissolve in a solvent

A solution in which water is the solvent

A molecule in which the electrons are shared unevenly, resulting in one end of the molecule being positive and the other being negative

An aqueous solution that conducts electricity

An aqueous solution that does not conduct electricity

A solution that contains the maximum amount of solute at a given temperature

A solution that contains more than the maximum amount of solute at a given temperature

A solution that contains less than the maximum amount of solute at a given temperature

Uneven distribution of a charge on a molecule, allows water to dissolve many substances

Weak bonds that form between the positive hydrogens and negative oxygens of polar water molecules, giving water many of its unique properties

Property of water where water molecules stick to each other

Property of water where hydrogen bonds between water molecules cause a 'film' to develop at the surface; allows bugs to sit on top of water

Property of water where water molecules stick to other surfaces

Property of water where water molecules can "climb" structures; straws in water make use of this property

Water has a high ___ ___ because it requires a great deal of energy to overcome the hydrogen bonding in the liquid phase to change it to a gas

Water is known as the ___ ___ because its unique properties allow it to dissolve more substances than any other solvent

Liquid mercury

Sodium chloride

Air

Brass

Is making a solution a physical or chemical change?

When the temperature of a solvent increases, solubility of ____ increases.

Which salt is least soluble at 50°C?

How many grams of KCl are expected to dissolve in water at 90 °C?

50 g of KNO₃ dissolved into 100 g of water at 60°C.

50 g of KCl dissolved into 100 g of water at 50°C.

25 g of CaCl₂ dissolved into 100 g of water at 10 °C.

45 g of NaCl dissolved into 100 g of water at 100 °C.

30 g of K₂Cr₂O₇ dissolved in 100 g of water at 50 °C.

Use solubility rules to determine if the following is soluble (aq) or insoluble (s) in water: CaSO₄

Use solubility rules to determine if the following is soluble (aq) or insoluble (s) in water: AgNO₃

When KNO₃ dissolves in water, what ions will it form?

When PbI₂ dissolves in water, into what ions will it dissociate?

When Al₂O₃ dissolves in water, what ions will it dissociate into?

Use solubility rules to determine which of the following will produce a precipitate (s).

3NaBr(aq) + AlNO₃(aq) → NaNO₃(___) + AlBr₃(___)

Predict whether the following compound is soluble or insoluble in water: Methane (CH₄) (nonpolar)

Predict whether the following compound is soluble or insoluble in water: Ammonia (NH₃) (polar)

Predict whether the following compound is soluble or insoluble in water: Fe₂O₃ (ionic)

Identify the following aqueous solution as a strong electrolyte, weak electrolyte, or nonelectrolyte: Sr(OH)₂

Identify the following aqueous solution as a strong electrolyte, weak electrolyte, or nonelectrolyte: H₂CO₃

Identify the following aqueous solution as a strong electrolyte, weak electrolyte, or nonelectrolyte: C₁₂H₂₂O₁₁

Identify the following aqueous solution as a strong electrolyte, weak electrolyte, or nonelectrolyte: HNO₃

Identify the following aqueous solution as a strong electrolyte, weak electrolyte, or nonelectrolyte: CH₄

When the pressure on a solvent increases, solubility of ____ increases.