Buffer Solutions and pH Calculations in Chemistry-Unit 25

HCl

Strong acid used in neutralization reactions.

NaOH

Strong base that neutralizes acids.

Limiting reactant

Substance that is completely consumed in reaction.

Molarity (M)

Concentration measured in moles per liter.

pH

Measure of acidity or basicity of a solution.

Buffer solution

Resists pH changes upon addition of acids or bases.

Conjugate base

Species formed when an acid donates a proton.

Conjugate acid

Species formed when a base accepts a proton.

Equilibrium

State where reactants and products are balanced.

Le Chatelier's Principle

System shifts to counteract changes in equilibrium.

Weak acid

Partially dissociates in solution, establishing equilibrium.

Strong acid

Completely dissociates in solution.

Acidic buffer

Contains weak acid and its conjugate base.

Basic buffer

Contains weak base and its conjugate acid.

Henderson-Hasselbalch equation

Calculates pH of buffer solutions.

Ka

Acid dissociation constant, measures strength of acid.

Kb

Base dissociation constant, measures strength of base.

Neutralization reaction

Reaction between acid and base producing salt and water.

pKa

Negative logarithm of the acid dissociation constant.

pKb

Negative logarithm of the base dissociation constant.

HF

Weak acid used in buffer solutions.

NH3

Weak base often used in buffer solutions.

F-

Conjugate base of HF.

NH4+

Conjugate acid of NH3.

OH-

Hydroxide ion, a strong base.

Reaction method

Technique to create buffers by partial neutralization.

Moles

Unit measuring amount of substance.

Volume

Amount of space occupied by a substance.

Dilution

Process of reducing concentration by adding solvent.