Acids and Bases, Redox reactions

Bronsted-Lowry acid

Proton donor.

Bronsted-Lowry base

Proton acceptor

Acid-base reaction

Reaction involving the transfer of a proton from an acid to a base

Hydrochloric acid (HCl)

Strong acid, formula HCl

Sulfuric acid (H2SO4)

Strong acid, formula H2SO4

Nitric acid (HNO3)

Strong acid, formula HNO3

Ethanoic acid (CH3COOH)

Weak acid, partially ionises in water

Carbonic acid (H2CO3)

Weak acid

Phosphoric acid (H3PO4)

Weak acid, triprotic

Properties of acids

Turn litmus red, sour, corrosive, conduct electricity, react with bases, low pH.

Sodium hydroxide (NaOH) 

Strong base, readily accepts protons

Calcium hydroxide (Ca(OH)2)

Strong base, weaker than NaOH

Ammonia (NH3)

Weak base, partially accepts protons

Magnesium hydroxide (Mg(OH)2)

Weak base, partially ionises

Sodium carbonate (Na2CO3)

Weak base

Properties of bases

Turn litmus blue, bitter, caustic/slippery, conduct electricity, react with acids, high pH.

Conjugate acid-base pair

Reactants and products that differ by a single H⁺ ion.

Reaction type for acids with metal hydroxide

Acid + metal hydroxide → salt + water

Reaction type for acids with metal carbonates

Acid + metal carbonate → salt + water + CO2

Reaction type for acids with metal hydrogen carbonates

Acid + metal hydrogen carbonate → salt + water + CO2

Reaction of acids with active metals

Acid + reactive metal → salt + hydrogen gas

Full ionic equation

Equation showing only the species that change, omitting spectator ions

Monoprotic acid

Acid that can donate only one proton per molecule (e.g., HCl, HF)

Polyprotic acid

Acid that can donate more than one proton per molecule (e.g., H2SO4, H3PO4)

Diprotic acid

Polyprotic acid that donates two protons in two stages (e.g., H2SO4)

Triprotic acid

Polyprotic acid that donates three protons in three stages (e.g., H3PO4)

Strong acid

Acid that fully ionises in water (→)

Weak acid

Acid that partially ionises in water (⇌)

Strong base

Base that readily accepts protons

Weak base

Base that partially accepts protons

Concentrated solution

Solution with a large amount of solute per unit volume

Dilute solution

Solution with a small amount of solute per unit volume

Oxidation

Loss of electrons (OIL → Oxidation Is Loss)

Reduction

Gain of electrons (RIG → Reduction Is Gain)

Redox reaction

Reaction involving both oxidation and reduction

Oxidising agent (oxidant)

Substance that gains electrons and causes oxidation

Reducing agent (reductant)

Substance that loses electrons and causes reduction

Half-equation

Equation showing only the oxidation or reduction half of a redox reaction

Electrochemical cell

Device that converts chemical energy into electrical energy via spontaneous redox reaction

Galvanic cell (Voltaic cell)

Spontaneous electrochemical cell where oxidation occurs at anode and reduction at cathode

Anode

Electrode where oxidation occurs (– in galvanic cell)

Cathode

Electrode where reduction occurs (+ in galvanic cell)

Salt bridge

Device allowing ion flow to maintain charge neutrality in a galvanic cell

Electrochemical series

List of half-equations ordered by ease of reduction

Electron flow

Direction from stronger reductant to stronger oxidant

Applications of redox

Corrosion, combustion, batteries, electrolysis, industrial bleaching, cellular respiration, photosynthesis