Exam 2 Topics for Analytical Chemistry

Ksp

A solubility product constant used to calculate solubility for compounds with stoichiometry other than 1:1.

Common Ion Effect

A general rule about solubility that states the solubility of a salt decreases in a solution that already contains one of its constituent ions.

Complex Ion Formation

The process of forming complex ions explained in terms of Lewis acids and bases.

Bronsted-Lowry Acids and Bases

Acids are proton donors, and bases are proton acceptors.

Conjugate Acid-Base Pairs

Pairs of acids and bases that differ by the presence or absence of a proton.

Autoprotolysis of Water

The self-ionization of water, represented by the equilibrium constant Kw.

Kw

The ion product of water at 25°C, equal to 1.0 x 10^-14.

pH

A measure of the acidity or basicity of a solution, calculated as -log[H+].

pOH

A measure of the hydroxide ion concentration in a solution, calculated as -log[OH-].

Strong Acids

Acids that completely dissociate in solution; examples include HCl, HBr, and HI.

Strong Bases

Bases that completely dissociate in solution; examples include NaOH and KOH.

Weak Acids

Acids that do not fully dissociate in solution; one class includes acetic acid.

Weak Bases

Bases that do not fully dissociate in solution; one class includes ammonia.

Ka and Kb

The acid dissociation constant and base dissociation constant, respectively, used to express the strength of acids and bases.

Titration

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

Fajans Titration

A type of titration that involves a color change at the endpoint, indicating the completion of the reaction.

Primary Standards

Highly pure substances used to determine the concentration of a titrant in titrations.

Purity Grades of Chemicals

Levels of purity for chemicals, including analytical grade, reagent grade, and others.

pMe

The negative logarithm of the molar concentration of metal ions in a precipitation titration curve.

Buffer Solution

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

Henderson-Hasselbalch Equation

An equation used to calculate the pH of a buffer solution based on the concentration of its acidic and basic components.