Summary of Acid, Base, Concentration, and Titration Concepts

Units of Concentration

• Solution: Homogeneous mixture of solute and solvent.

• Concentration: Ratio of solute amount to solvent amount.

  • % (w/w), % (w/v), % (v/v) formulas:

  • % (w/w) = (mass solute/mass solution) x 100

  • % (w/v) = (mass solute/volume solution) x 100

  • % (v/v) = (volume solute/volume solution) x 100

ppm and ppb

• ppm: parts per million = (mass solute/volume solution) x 10^6

• ppb: parts per billion = (mass solute/volume solution) x 10^9

Molarity and Molar Mass

• Molarity (M): moles of solute per liter of solution.

• Mole: SI unit for amount of substance.

• Molar mass: Calculated from individual elements.

Making Solutions

• Stock solution: g = M x L x molar mass.

• Dilution formula: C1V1 = C2V2.

Acids and Bases

• Arrhenius: Acid increases [H3O+], base increases [OH-].

• Bronsted-Lowry: Acid donates protons, base accepts protons.

• Lewis: Acid accepts electron pairs, base donates electron pairs.

Strong vs Weak Acids/Bases

• Strong acids/bases ionize completely; weak ones only partially.

• pH: -log[H+].

• pOH: -log[OH-].

• Kw: [H3O+][OH-] = 1.0 x 10^-14 at 25°C.

Titration

• Method to determine concentration of an unknown acid/base using neutralization reaction.

• Equivalence point: Stoichiometric amount of acid and base.

Acid-Base Properties of Salts

• Salts can produce neutral, acidic, or basic solutions depending on the strengths of the acids and bases from which they originate.