Properties of Solutions (Acids + Bases + Buffers + titrations) Flashcards
what is the ionic product of water
1 x 10^-14
what is a bronsted-Lowry acid ?
proton (H+) donor
what is a Bronsted-Lowry Base?
proton (H+) acceptor
what does amphoteric mean ?
able to act as both an acid and a base.
what is an Arrhenius acid?
a species which increases the number of H30+ ions when dissolved in water (pH decreases)
what is a Arrhenius base?
a species which increases the number of OH- ions when dissolved in water (pH increases)
what is a lewis acid
electron pair acceptor
what is a lewis base
electron pair donor
the Arrhenius acids are limited to …
aqueous solutions
the equation for strong acid pH =
-log (c H30+/c standard)
in an acid base reaction the equilibrium favours the side with the … this is because…
weaker acid and base, because they are more stable and have lower potential energies.
how do we determine the pH of weak acids/bases
first we find the equilibrium constant - in this case known as the Ka (acid dissociation constant)
Ka of pure liquids =
1
using the Ka we can calculate the …
pKa
for weak acids the equilibrium lies far to the…
left
after finding x in the pH weak acid calculations, how do you find the pH?
pH = -logx
pKa + pKb =
pKw = 14
Ka x Kb =
Kw
what is the inductive effect?
occurs when electron-withdrawing or electron-donating groups in a molecule cause a change in electron density. this causes the pH to change.
inductive effect -
the more electronegative the bonding group the ____ the acid
stronger
inductive effect -
the _____ the bonding group the stronger the acid
closer
inductive effect -
the ____ of the bonding group the stronger the acid
more
the ___ resonance forms the ____ stable the anion and hence the stronger the acid
more, more
what makes up a buffer solution?
mix of either a weak acid or base and its corresponding salt.