Solutions, acids & bases · Topic 12 of 15

Solutions & Concentration

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Chemistry · solutions

A solute dissolves in a solvent; concentration is molarity (mol/L) or percent; dilution keeps the solute constant, so C₁V₁ = C₂V₂.

01 · The partsSolute dissolves in solvent

02 · MolarityM = mol solute ÷ L solution

03 · DilutionC₁V₁ = C₂V₂

Solution = a solute dissolved evenly in a solvent must know

Aqueous (aq) = water is the solvent

Solubility = the most solute that can dissolve under set conditions

Warmer solvent: most solids dissolve more, gases dissolve less

More gas pressure = more gas dissolves (Henry's law)

Like dissolves like: polar in polar, nonpolar in nonpolar

Molarity (M) = moles of solute ÷ liters of solution must know

Dilution: C₁V₁ = C₂V₂ — the amount of solute stays the same must know

Percent = solute ÷ total solution × 100 (m/v %: g per 100 mL) must know

0.60 mol in 250 mL: 0.60 ÷ 0.250 L = 2.4 M

500 mL of 0.50 M from 2.0 M: V₁ = 0.50 × 500 ÷ 2.0 = 125 mL

500 mL of 0.9% saline: 0.9 g per 100 mL × 5 = 4.5 g NaCl

Unsaturated (more fits) · saturated (at the limit) · supersaturated (over it)

Dilute = little solute; concentrated = much (relative terms)

Commonly confused

Molarity uses liters of solution — change mL to L first

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Volume percent (v/v) = mL solute ÷ mL solution × 100

Trace amounts: parts per million (ppm) or billion (ppb)

Miscible liquids mix fully; immiscible ones form layers

Pearl

Dilution changes the volume, never the amount of solute — that is why C₁V₁ = C₂V₂.

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