Chemistry: Solubility, Acids, Bases, and Gas Laws

Comprehensive flashcards covering solubility definitions, the effects of temperature/pressure on solids and gases, acid-base theories, nomenclature, gas laws, and molarity/dilution formulas.

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.

Solvent

The substance doing the dissolving.

Solubility

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 called 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 where more solute is dissolved than normal at a given temperature.

Electrolytes

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

Effect of temperature on solid solubility

Increase in temperature leads to more substance dissolving, while decrease in temperature leads to less substance dissolving.

Effect of air pressure on solid solubility

No effect on solubility.

Effect of temperature on gas solubility

Increase in temperature causes solubility to decrease, while decrease in temperature causes solubility to increase.

Effect of air pressure on gas solubility

Increase in air pressure causes solubility to increase, while decrease in air pressure causes solubility to decrease.

Oxidized element

An element that loses electrons.

Hydronium

$\text{H}_3\text{O}^+$; it is formed when an acid dissolves in water.

Acids (Characteristics)

pH of 0-6.9, turns litmus paper red, tastes sour, feels squeaky, and includes examples like citrus fruits, apples, and tomato sauce.

Bases (Characteristics)

pH of 7.1-14, turns litmus paper blue, tastes bitter, feels slippery, and includes examples like ammonia (Windex), soap, and bleach.

Arrhenius Acid

A substance that donates hydrogen ion ($\text{H}^+$).

Arrhenius Base

A substance that donates hydroxide ion ($\text{OH}^-$).

Bronsted-Lowry Acid

A substance that donates hydrogen ion ($\text{H}^+$).

Bronsted-Lowry Base

A substance that accepts hydrogen ion ($\text{H}^+$).

Strong (Acid/Base)

A substance that completely breaks apart into ions.

Weak (Acid/Base)

A substance that completely stays together.

pH Formula ($\text{H}^+$)

$$pH = -\log[H^+]$$

pH Formula ($\text{OH}^-$)

$-\log[OH^-] = X$ then $14 - X = pH$

Neutralization Reaction

A reaction where the products are always a water and a salt, resulting in a pH of 7.

Binary Acids

Acids made of $\text{H}^+$ and one other element, often a halogen, with no polyatomic ions.

Naming Binary Acids

Start with the prefix hydro-, add the root of the anion, end with the suffix -ic, and add the word "acid" (e.g., $\text{HCl}$ is hydrochloric acid).

Oxyanion Acid

An acid made of $\text{H}^+$ and a polyatomic ion, usually containing hydrogen.

Oxyanion Acid Suffix Rule

If the polyatomic ion ends with -ate, the acid ends with -ic; if it ends with -ite, the acid ends with -ous.

Arrhenius Base Naming

Name the metal ion followed by the anion, which is usually hydroxide (e.g., $\text{KOH}$ is potassium hydroxide).

Conjugates

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

Boyle’s Law

States that volume varies inversely with pressure: $P_1V_1 = P_2V_2$

Charles's Law

States that volume varies directly with temperature ($K$): $\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Gay-Lussac’s Law

States that pressure varies directly with temperature: $\frac{P_1}{T_1} = \frac{P_2}{T_2}$

Avogadro’s Law

States that volume varies directly with moles: $\frac{V_1}{n_1} = \frac{V_2}{n_2}$

Ideal Gas Law

Relates pressure, temperature, volume, and moles through the gas constant ($R$): $PV = nRT$

Combined Gas Law

Combines Boyle’s, Charle’s and Gay-Lussac’s laws into one equation: $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$\n

Dalton’s Law of Partial Pressure

The total pressure of a mixture of gases is the sum of the pressures of each gas: $P_{total} = P_1 + P_2 + P_3 + P_4 \dots$

Concentration

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

Molarity

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

Dilutions

The process of reducing molarity or concentration of a solute in a solution by adding more solvent.

Dilution Equation

$$V_1M_1 = V_2M_2$$