Kinetics and Acid-Base Equilibrium Experiments

Flashcards covering key concepts, terminology, and definitions related to the Kinetics and Acid-Base Equilibrium experiments.

Rate Law

An equation that relates the rate of a reaction to the concentration of its reactants.

Kinetics

The study of the rates of chemical reactions.

Activation Energy

The minimum amount of energy required for a reaction to occur.

Catalyst

A substance that increases the rate of a chemical reaction without being consumed.

Spectrophotometer

An instrument used to measure the intensity of light absorbed by a solution.

Equilibrium

A state in which the forward and reverse reactions of a chemical process occur at the same rate.

Henderson-Hasselbalch Equation

An equation used to calculate the pH of a buffer solution.

Buffer Capacity

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

Spectrochemical Series

A list of ligands arranged according to their ability to split the d-orbitals of transition metal ions.

Beer-Lambert Law

A linear relationship between absorbance and concentration of an absorbing species.

Titration

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

Complex Ion

A species formed from a metal ion bonded to one or more ligands.

Solubility Product (Ksp)

An equilibrium constant that applies to the solubility of ionic compounds.

Gran Plot

A graphical method used to determine the equivalence point of a titration.

Monoprotic Acid

An acid that can donate only one proton (H+) per molecule in a reaction.

Polyprotic Acid

An acid that can donate more than one proton per molecule in a reaction.

Transition Metal

Elements that have partially filled d-orbitals and can form variable oxidation states.

Infrared Spectroscopy (IR)

A technique used to identify functional groups in organic compounds by measuring the absorption of infrared light.