Acids + Bases Flashcards
Acid
Substance capable of donating a hydrogen ion (proton)
Acid rain
Rainwater that has reacted with acidic emissions from industry and has a pH less than 5.5
Acidic oxide
An oxide, generally of a non-metal, that either reacts with water to form an acid or reacts with a base
Acidic solution
A aqueous solution in which [H+] > [OH−]. At 25°C, the pH < 7
Alkali
A soluble base
Amphiprotic
The ability to act as an acid or a base
Base
A substance capable of accepting a hydrogen ion (proton)
Basic oxide
An oxide of a metal which either reacts with water to form hydroxide ions or reacts with H3O+ ions
Basic solution
A solution where [H+] < [OH−]. At 25°C, the pH > 7
Brønsted-Lowry theory
A theory that defines an acid as a proton (hydrogen ion) donor and a base as a proton acceptor
Conjugate acid
The conjugate acid of a base contains one more hydrogen ion (proton) than the acid
Conjugate base
The conjugate base of an acid contains one less hydrogen ion (proton) than the acid
Diprotic
A diprotic acid is capable of donating two hydrogen ions (protons), e.g. H₂SO₄
Hydronium ion
The H3O+ ion
Indicator
A substance that has different colours in its acid and base forms
Ionic equation
An equation that includes only ions involved in the reaction
Ionic product of water
The product of the hydrogen ion concentration and hydroxide ion equation
Neutralise
To react an acid with a base to form a solution of a salt and water
Salt
A substance formed from a metal (or ammonium) cation and an anion
Monoprotic
An acid only capable of donating one hydrogen ion (proton)
Neutral solution
A solution in which the concentration of H3O+ (aq) ions equals the concentration of OH− (aq) ions
pH
A measure of acidity; pH = - log10[H3O+(aq)]
Polyprotic
An acid capable of donating more than one hydrogen ion (proton) to form a base
Strong acid
An acid that readily donates a hydrogen ion to water acting as a base
