21 acids and bases
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define acid
proton donor
define base
proton acceptor
define a strong acid
an acid that fully dissociates
define a weak acid
an acid that only partially dissociates
define pH
-log10[H+]
how do you calculate the concentration of H+ ([H+]) from pH?
10^-pH
what does Kw mean?
the ionic product of water
define Kw
[H+][OH-] 1x10^-14
what is a monoprotic acid?
one which only releases one H+ ion
what is a diprotic acid?
one which releases two H+ ions
if the pH is small, what does that mean in terms of concentration of H+ ions?
greater concentration of H+ ions
name 4 strong acids
HCl (hydrochloric acid) H2SO4 (sulfuric acid) HNO3 (nitric acid) H3PO4 (phosphoric acid)
how does HCl dissociate? give an equation
fully dissociates HCl –> H+ + Cl-
where does the equilibrium lie in equations of strong acid dissociations?
entirely to the right
if the concentration of HCl is originally 2moldm-3, what will be the conc of H+ once fully dissociated?
2moldm-3
if the concentration of H2SO4 is originally 2moldm-3, what will be the conc of H+ once fully dissociated?
4moldm-3
how does a weak acid dissociate? give an equation in terms of HA
partially dissociates HA <–> H+ + A-
where does the equilibrium lie in equations of weak acid dissociations?
on the left hand side
write a Ka expression for the dissociation of weak acid HA
Ka = [H+][A-]/[HA]
how would you find the concentration of H+ in a weak acid dissociation?
[H+] = [A-] Ka = [H+]^2/[HA] [H+]^2 = Ka x [HA] [H+] = √Ka x [HA]
how do you calculate pKa?
-log10Ka
how do you find Ka from pKa?
10^-pKa
write an equation for the ionisation of water
H2O <–> H+ + OH-
where does the equilibrium lie in the equations for the ionisation of water?
very far left