Buffer Practice Problems and Titration Concepts

These flashcards cover important terms and concepts related to buffer solutions, pH calculations, titration processes, and acid-base chemistry as presented in the lecture notes.

Buffer Solution

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

pH Calculation for Buffers

Use the formula: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the weak acid.

Weak Acid

An acid that partially dissociates in solution, characterized by a low Ka value.

Conjugate Base

The species that remains after an acid donates a proton; it can accept a proton in reverse reactions.

Titration

A laboratory method for determining the concentration of an acid or a base by reacting it with a base or an acid of known concentration.

Equivalence Point

The point in a titration at which the amount of titrant added is stoichiometrically equivalent to the amount of analyte in the sample.

Acid-Base Neutralization Reaction

A chemical reaction between an acid and a base that produces a salt and water.

Indicator in Titrations

A substance that changes color at a particular pH range to indicate the endpoint of a titration.

Hydronium Ion

The ion formed when a water molecule gains an H+ ion, represented as H3O+.

Ka (Acid Dissociation Constant)

A quantitative measure of the strength of an acid in solution; higher Ka values indicate stronger acids.

Ksp (Solubility Product Constant)

An equilibrium constant used to describe the solubility of sparingly soluble ionic compounds.

Henderson-Hasselbalch Equation

A formula used to calculate the pH of a buffer solution: pH = pKa + log([A-]/[HA]).

Titration Curve

A graph plotting pH against the volume of titrant added, illustrating changes in pH during a titration.

Buffer Capacity

The ability of a buffer solution to resist changes in pH upon the addition of an acid or base.

Chloroacetic Acid (Ka)

A strong weak acid with a Ka value of 1.35 x 10^-3, used as an example in buffer calculations.

Weak Base

A base that does not completely ionize in solution; characterized by low Kb value.

Hydroxide Ion (OH-)

The ion formed when a water molecule loses a hydrogen ion, commonly produced by bases.

Saturated Solution

A solution in which the maximum amount of solute has been dissolved at a given temperature.