Solubility, Acids and Bases, and Gas Laws Lecture Notes

This set of vocabulary flashcards covers solubility types, acid-base theories, naming conventions for acids and bases, gas laws, and concentration/dilution formulas based on the lecture notes.

Solution

A homogeneous mixture created when two substances are evenly mixed together.

Aqueous solution

A solution formed when solutes dissolve in water.

Solute

The substance being dissolved in a solution.

Solvent

The substance doing the dissolving in a solution.

Solubility

A measure of how well a substance will dissolve in a solvent.

Precipitation reaction

A reaction that occurs when two aqueous solutions are mixed and form a solid product known as a precipitate.

Saturated solution

A solution where the solvent has dissolved all the solute it can at a certain temperature.

Unsaturated solution

A solution where more solute can still be dissolved at a certain temperature.

Supersaturated solution

A solution containing more dissolved solute than normal at a given temperature.

Electrolytes

Ionic compounds that conduct electricity when dissolved; they must be both ionic and soluble.

Hydronium ($H_3O^+$)

The ion formed when an acid dissolves in water.

Arrhenius Acid

A substance that donates a hydrogen ion ($H^+$).

Arrhenius Base

A substance that donates a hydroxide ion ($OH^-$).

Bronsted-Lowry Acid

A substance that donates a hydrogen ion ($H^+$).

Bronsted-Lowry Base

A substance that accepts a hydrogen ion ($H^+$).

Strong (Acid/Base)

A substance that completely breaks apart into ions.

Weak (Acid/Base)

A substance that completely stays together rather than ionizing.

Neutralization Reaction

A reaction between an acid and a base where the products are always a water and a salt, resulting in a pH of $7$.

Binary Acid

An acid made of $H^+$ and one other element, often a halogen, containing no polyatomic ions.

Oxyanion Acid

An acid made of $H^+$ and a polyatomic ion; the name is derived from the polyatomic ion suffix (ate goes to -ic, ite goes to -ous).

Conjugate acid and base

Two substances that transform into each other by the gain and loss of a proton ($H^+$).

Boyle’s Law

The principle that volume varies inversely with pressure, expressed as $P_1V_1 = P_2V_2$.

Charles's Law

The principle that volume varies directly with temperature in Kelvin, expressed as $\frac{V_1}{T_1} = \frac{V_2}{T_2}$.

Gay-Lussac’s Law

The principle that pressure varies directly with temperature, expressed as $\frac{P_1}{T_1} = \frac{P_2}{T_2}$.

Avogadro’s Law

The principle that volume varies directly with the number of moles, expressed as $\frac{V_1}{n_1} = \frac{V_2}{n_2}$.

Ideal Gas Law

The law relating pressure, temperature, volume, and moles through the gas constant ($R$), expressed as $PV = nRT$.

Combined Gas Law

An equation combining Boyle’s, Charles’s, and Gay-Lussac’s laws: $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$.

Dalton’s Law of Partial Pressure

The law stating the total pressure of a gas mixture is the sum of the partial pressures of each gas: $P_{\text{total}} = P_1 + P_2 + P_3 + P_4...$

Concentration

The amount of solute that has been dissolved in a certain amount of solvent.

Molarity

The units in which concentrations are measured, calculated as $M = \frac{\text{mol}}{\text{L}}$.

Dilutions

The process of reducing the molarity of a solute in a solution by adding more solvent, calculated as $V_1M_1 = V_2M_2$.