Chem- Equilibrum, Acids and Bases

Acid

Substance that donates H+ ions or increases H+ concentration in water.

Activation Energy

Minimum energy needed for a reaction to occur.

Amphoteric

Substance that can act as both an acid and a base.

Arrhenius

Acid produces H+ in water; base produces OH- in water.

Base

Substance that accepts H+ ions or increases OH- concentration in water.

Bronsted-Lowry

Acid donates protons (H+); base accepts protons.

Catalyst

Substance that speeds up a reaction by lowering activation energy without being used up.

Collisions

Reacting particles must collide with enough energy and correct orientation for a reaction to happen.

Conjugates

Acid/base pairs that differ by one H+ ion.

Electrolytes

Substances that conduct electricity when dissolved in water because they form ions.

Equilibrium

State where forward and reverse reactions occur at equal rates.

Equilibrium Constant (K)

Ratio of products to reactants at equilibrium.

Indicator

Substance that changes color depending on pH.

Kinetics

Study of reaction rates.

LeChatelier’s Principle

If stress is applied to a system at equilibrium, the system shifts to reduce the stress.

Neutralization

Reaction between acid and base producing water and a salt.

pH

Scale measuring acidity/basicity of a solution.

Reaction Rate

Speed at which reactants turn into products.

Reversibility

Ability of a reaction to proceed forward and backward.

Titration

Method used to determine concentration using neutralization.