12.1 Flashcards
an acid is a proton…
donor
a base is a proton…
acceptor
when does a molecule which contains hydrogen act as an acid
if the hydrogen carries a slightly positive charge
what makes a molecule a base
it must contain a lone pair in order to form a dative covalent bond
what is a conjugated acid-base pair
consists of either a base and its conjugate acid or an acid and its conjugated base
state the conjugated pairs for this reaction
HCl + H2O <=> H3O+ + Cl-
Cl- & HCl
H2O & H3O+
what is meant by monoprotic
a species that can donate 1 proton
what is meant by diprotic
a species that can donate 2 protons
what is an amphoteric substance
one that can act both as an acid and as a base
how do you define a strong acid
one that almost completely dissociates in aqueous solutions
how do you define a weak acid
one that only partially dissociates in aqueous solutions
what is the equation for pH
pH = -log[H+]
what does Ka stand for
acid dissociation constant
what is the general equation for Ka
Ka = [H+(aq)] [A-(aq)] / [HA(aq)]
what is the equation for Ka in strong acids
Ka = [H+(aq)] / [HA(aq)]
what is the equation for pKa
pKa = -logKa
How does pKa and Ka effect the pH of an acid
as Ka increases pH decreases
as pKa decreases pH decreases
what is the equation for self-ionization of water
Kw = [H+(aq)] [OH-(aq) / [H2O(l)]
How is the equation for ionisation of water simplified at a stated temperature
Kw = [H+(aq)] [OH-(aq)]
what does Kw stand for
the ionic product of water
how do you define a neutral solution
one in which the hydrogen ion concentration is equal to the hydroxide ion concentration
what is the equation for pKw
pKw = -log Kw
why do even the most alkaline solutions still contain some hydrogen ions
because of the fact that water self-ionises
how can the relative strengths of different acids or bases be determined
by measuring the pH of equimolar aqueous solutions of the acids/bases, at the same temperature