Acids and Bases Flashcards
acids
produce hydrogen ions in aqueous solution (proton doners)
bases
Substances that produce hydroxide ions in aqueous solution; proton acceptors
Arrhenius concept of acids and bases
A concept postulating that acids produce hydrogen ions in aqueous solutions, whereas bases produce hydroxide ions
Brønsted–Lowry model
suggested by the Danish chemist Johannes Brønsted and the English chemist Thomas Lowry
A model proposing that an acid is a proton donor and that a base is a proton acceptor
conjugate acid
The species formed when a proton is added to a base
conjugate base
What remains of an acid molecule after a proton is lost
conjugate acid–base pair
Two species related to each other by the donating and accepting of a single proton
hydronium ion
The H3O+ ion; a hydrated proton
strong acid.
completely ionized or completely dissociated.
A strong acid is one for which the forward reaction predominates
A strong acid contains a relatively weak conjugate base (low attraction for protons)
acid whose conjugate base is a much weaker base than water
weak acid
An acid that dissociates only to a slight extent in aqueous solution
the reverse reaction predominates
A weak acid contains a relatively strong conjugate base
oxyacids
Acids in which the acidic proton is attached to an oxygen atom
Organic acids
Acids with a carbon-atom backbone and a carboxyl group
carboxyl group
The —COOH group in an organic acid
amphoteric substance
said to be amphoteric if it can behave either as an acid or as a base
The fundamental unit of which elements are composed
ex- water
ion-product constant, 𝐾𝑤
The equilibrium constant for the autoionization of water ;
𝐾w=[H+] [OH-]. At 25C° , 𝐾w equals 1.0×10^14
neutral solution
A solution for which [H+]=[OH-]
acidic solution
A solution for which [H+]>[OH-]
basic solution
A log scale based on 10 and equal to log[H+][OH-]
pH scale
10, the pH changes by 1 for every power-of- 10 change in the [𝐻+]
