Acids And Bases

A substance that produces hydrogen ions (H+)/ hydronium ion (H3O+) when it dissolves in water

A substance that produces hydroxide ions (OH-) in water

An acid is a proton (H + ion) donor

A base is a proton acceptor (H + ion)

A substance that ionises completely in water to form a high concentration of hydronium ions

A substance that ionises impartially to form a low concentration of hydronium ions

Strong bases dissociate completely to form a high concentration of OH- hydroxide ions

A substance that dissociates incompletely to form a low concentration of hydroxide ions (OH-)

Substance with a large number of moles of acid/ base in proportion to the volume of water

Substances that contain a small amount of moles of acid/ base in proportion to the volume of water

A substance that can act as a base in one reaction and a acid in another

A substance that can accept protons in one reaction and donate protons in another

An acid that has more than proton to donate

A solution whose exact concentration is known

The reaction of a salt with water

The point at which the acid/ base had completely reacted with the other base/acid

The point at which the indicator changes colour

Bromothymol Blue It’s yellow in acids It’s blue in bases Green at its end point pH range is 6 - 7,6

Phenolphthalein It’s clear in acids It’s pink in bases It’s a faint pink when it reaches end point It’s pH range is 8,3- 10

Methyl orange It’s red in acids It’s yellow in bases It’s pH range is 2,5 - 4,4

The extra O atoms delocalize negative charge on the conjugate base (via resonance), making it more stable and the acid more willing to donate H⁺. Hence why the strength of an acid increases with the amount of O atoms in the compound

Oxacids

A Lewis base donates a pair of electrons, while a Lewis acid accepts a pair of electrons

Lewis acid accepts a pair of electrons