Chapter 11 Chemistry: Solutions, Electrolytes, and Reaction Types

Solution

solute (what's dissolved) + solvent (does the dissolving). Example: salt water → salt = solute, water = solvent.

Electrolytes

substances that form ions when dissolved in water.

Strong electrolytes

completely ionize (e.g. NaCl, HCl).

Weak electrolytes

partially ionize (e.g. CH₃COOH, NH₃).

Non-electrolytes

do not ionize (e.g. sugar, ethanol).

Solubility Rules

Used to predict if a precipitate (solid) will form in a reaction.

Solubility Example

Most nitrates (NO₃⁻) and alkali metals (Na⁺, K⁺) are soluble.

Insoluble Carbonates and Phosphates

Carbonates (CO₃²⁻) and phosphates (PO₄³⁻) are insoluble unless with alkali metals or NH₄⁺.

Molarity (M)

moles of solute / liters of solution.

Finding Moles

moles = M × L.

Finding Volume

L = moles / M.

Mass percent

(mass solute / mass solution) × 100.

Dilution formula

M₁V₁ = M₂V₂.

Double-Displacement Reactions

Two ionic compounds exchange ions: AB + CD → AD + CB.

Driving forces of reactions

formation of a precipitate, gas, or water.

Precipitation Reactions

Two soluble solutions mix → insoluble solid forms.

Acid-Base Reactions

Acid + Base → Salt + Water.

Acid-Base Reaction Example

HCl + NaOH → NaCl + H₂O.