Exploration of Le Chatelier's Principle and Buffers

Flashcards covering key concepts related to Le Chatelier's Principle and buffers from the lab experiment.

Le Chatelier's Principle

When a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

Ligands

Molecules or ions that can bind to a central metal atom to form a complex (e.g., H₂O, NH₃, Cl⁻, OH⁻).

Buffer

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

Common-Ion Effect

A shift in equilibrium caused by the addition of an ion that is part of the equilibrium.

Qualitative Analysis

The process of determining the presence or absence of a certain substance based on observable changes, such as color shifts.

Reaction Quotient (Q)

A measure of the relative amounts of reactants and products during a reaction at any point in time, used to predict the direction of a reaction.

Endothermic Reaction

A reaction that absorbs heat; a shift to the right occurs when heat is added.

Exothermic Reaction

A reaction that releases heat; a shift to the left occurs when heat is added.

Henderson-Hasselbalch Equation

An equation that relates the pH of a buffer solution to the concentrations of its acid and conjugate base: pH = pKa + log(base/acid).

Complex Ion

A polyatomic ion consisting of a metal ion surrounded by ligands.

Precipitate

An insoluble solid formed from a solution during a chemical reaction.

Solubility Product Constant (Ksp)

An equilibrium constant that applies to the saturated solution of a sparingly soluble ionic compound.

Color Change as an Indicator

A visual sign used to determine the direction of equilibrium shifts in chemical reactions.

Thermal Stressing

The effect of temperature changes on the position of equilibrium in a chemical reaction.

Chemical Formula of Silver-Ammonia Complex

The formula for the silver-ammonia complex formed in this lab is [Ag(NH₃)₂]⁺.