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Nitric Acid

HNO₃

Hydrochloric acid

HCL

Sulphuric acid

H₂SO₄

Ethanoic acid

CH₃COOH

Ammonia

NH₃

Sodium hydroxide

NaOH

Sodium carbonate

NA₂CO₃

Amonnium hydroxide

NH₄OH

Hydroxide ion

OH^-

Hydronium ion

H₃O⁺

Acids

• <7

• Red litmus

• Donates protons

• Neutralizes bases

• Corrosive

• Sour

• Dissolve into electrolytes

Bases

• >7

• Blue litmus

• Accepts protons

• Neutralizes acids

• Corrosive

• Bitter

• Slippery

• Electrolyte

• Oxides/hydroxides of metals

• Ionic

• Insoluble (or alkali)

Oxidation

• -e^-

• Oxidation number increases

• Reductant is oxidised

• Anode

Reduction

• +e^-

• Oxidation number decreases

• Oxidant is reduced

• Cathode

Oxidation numbers

• free = 0

• sum of oxidation numbers = molecule charge

Hydroxide

OH^-

Oxide

O^2-

Carbonate

CO₃^2-

Hydrogen carbonate/bicarbonate

HCO₃^-

Half equations

1. Balance everything but O and H

2. Balance O with water

3. Balance H with H⁺

4. Balance charges with e^-

Strong

• Fully reacts →

• Better conductor

• HCL

• HNO₃

• H₂SO₄

• O^2-

• OH^-

Weak

• Reacts partially ><

• CH₃COOH

• H₂CO₃

• NH₃

• NO₃^-