Solutions, Solubility, and Polarity (HMH Chapter 4.3)

Practice vocabulary flashcards covering mixture types, solubility rules, concentration calculations, and chemical equations for solutions based on the HMH Chapter 4.3 lecture notes.

Solvent

The dissolving agent in a homogeneous mixture, such as water, which is known as the universal solvent.

Solute

The substance that is dissolved in a solution, such as salt, ionic compounds, or polar covalent compounds.

Soluble

Substances that are capable of forming a solution in water, such as table salt or sugar.

Insoluble

Substances that do not form a solution in a specific liquid, such as sand in gasoline.

Miscible

Fluids that are soluble in each other, such as water and ethanol or various gases in the atmosphere.

Immiscible

Fluids that do not form a homogeneous mixture when mixed together, such as oil and water.

Electrolytes

Ions in solution that conduct electricity due to their charges; resulting from the dissociation of substances.

Strong Electrolytes

Substances that achieve $100\%$ dissociation in water, such as $HCl$ or $NaOH$.

Weak Electrolytes

Substances that only partially dissociate in water, such as $CH_3COOH$ (acetic acid) or $NH_3$.

Non-electrolytes

Molecular compounds that do not undergo ionization or dissociation in solution.

Solubility

The maximum quantity of a substance that will dissolve in a certain quantity of water (usually $100\,g$) at a specific temperature.

Saturated

A solution that contains the maximum amount of solute that can be dissolved in that solution at a given temperature.

Precipitate

An insoluble solid that forms and separates from a liquid solution, typically following a reaction between two aqueous solutions.

NAGSAG

A mnemonic for soluble compounds: Nitrates, Ammonium, Group 1 elements, Sulfates, Acetate, and Group 17 elements (except fluorine).

CaStroBear

A mnemonic for the exceptions Calcium ($Ca^{2+}$), Strontium ($Sr^{2+}$), and Barium ($Ba^{2+}$), which are insoluble when paired with sulfates.

PMS

A mnemonic for the exceptions Lead ($Pb^{2+}$), Mercury ($Hg$), and Silver ($Ag$), which are insoluble when paired with Sulfates or Group 17 elements.

Net Ionic Equation

An equation that shows only the species actually participating in the chemical reaction by eliminating spectator ions.

Spectator Ions

Ions that are present in a solution but do not participate in the actual chemical reaction.

Unsaturated

A solution that contains less than the maximum amount of solute and is capable of dissolving more.

Supersaturated

A solution that contains more solute than can typically be dissolved in the solvent under normal conditions.

Molarity ($M$)

A common measure of concentration calculated as $\frac{\text{mol}}{\text{L}}$; it represents the number of moles of solute per liter of solution.

Molality ($m$)

A concentration measure calculated as $\frac{\text{moles of solute}}{\text{kg of solvent}}$; it is independent of temperature and pressure because it is based on mass.

Stock Solution

The original, highly concentrated solution used to prepare more diluted solutions.

Dilution Formula

An equation used to calculate concentration or volume changes when adding solvent: $C_1 V_1 = C_2 V_2$.

Parts per million (ppm)

A unit of concentration used for environmental monitoring, such as $CO_2$ levels or water quality.