chem unit 2 ai 1

Ksp

The solubility product constant, representing the equilibrium between a solid salt and its dissolved ions.

Molar Solubility

The amount of solute that dissolves in a solvent to form a saturated solution at equilibrium.

Net Ionic Equation

An equation that shows only the ions involved in the reaction, excluding spectator ions.

Spectator Ion

An ion that doesn't participate in the chemical reaction and is present in the same form on both sides of the equation.

Arrhenius Acid

A substance that increases the concentration of H+ ions in an aqueous solution.

Arrhenius Base

A substance that increases the concentration of OH− ions in an aqueous solution.

Brønsted–Lowry Acid

A proton (H+) donor.

Brønsted–Lowry Base

A proton (H+) acceptor.

Lewis Acid

A substance that accepts an electron pair.

Lewis Base

A substance that donates an electron pair.

pH of Strong Acid

The pH of a strong acid is calculated using the formula pH = -log[H+].

pH of Strong Base

The pH of a strong base is calculated using the formula pOH = -log[OH−], then pH = 14 - pOH.

Buffer

A solution that resists changes in pH upon the addition of small amounts of an acid or base.

Buffer Capacity

The amount of acid or base a buffer solution can neutralize before the pH changes significantly.

Polyprotic Acid

An acid that can donate more than one proton (H+), such as H2SO4 or H3PO4.

Titration

A technique used to determine the concentration of a solution by reacting it with a solution of known concentration.

Equivalence Point in Titration

The point at which the amount of titrant added is stoichiometrically equivalent to the amount of substance present in the sample.

pKa

The negative logarithm of the acid dissociation constant (Ka), used to express the strength of an acid.

Ka

The acid dissociation constant, which represents the equilibrium constant for the dissociation of a weak acid.

Kb

The base dissociation constant, which represents the equilibrium constant for the dissociation of a weak base.

pKa1, pKa2

The first and second dissociation constants for polyprotic acids, indicating the strength of each proton donation.

Titration of Weak Acid with Strong Base

In this titration, the pH at equivalence point is greater than 7 because the conjugate base of the weak acid is present.

Titration of Weak Base with Strong Acid

In this titration, the pH at equivalence point is less than 7 because the conjugate acid of the weak base is present.

Alpha Diagram

A diagram showing the distribution of species in a polyprotic acid system as a function of pH.

Selective Precipitation

The process of precipitating one ion from a solution while leaving others in solution, based on differences in solubility.