CHM 1220: Laboratory Exam Review Guide

A collection of flashcards summarizing key concepts from the CHM 1220 Laboratory Exam Review Guide.

Molarity

The number of moles of solute per liter of solution.

M = mol/L

Molality

The number of moles of solute per kilogram of solvent.

m = mol solute/kilograms SOLVENT

Freezing Point Depression

The decrease in the freezing point of a solvent caused by the addition of a solute.

Molar Mass Calculation

The process of determining the mass of one mole of a given substance.

ΔT = K_fm

Titration

A technique used to determine the concentration of a solute in a solution by adding a titrant of known concentration.

M₁V₁ = M₂V₂

pKa

The negative logarithm of the acid dissociation constant; a measure of the strength of an acid.

Buffer Solution

A solution that resists changes in pH when small amounts of acid or base are added.

Solubility Product (Ksp)

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

Common Ion Effect

The decrease in solubility of a salt when a common ion is added.

Le Chatelier’s Principle

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

Electrochemical Cell

A device that generates electrical energy from chemical reactions.

Cell Voltage

The potential difference between the two electrodes in an electrochemical cell.

E_cathode - E_anode

Shifts to the RIGHT (towards products)

Reactants are added, increase in temperature

Shifts to the LEFT (towards reactants)

Products are added, decrease in temperature

Shifts to side w/ fewer moles

An increase in pressure or decrease in volume

Shifts to side w/ more moles

Increase in volume or a decrease in pressure