Chapter 10 Acids and Bases Flashcards
What is an Arrhenius acid?
Dissociate to form an excess of H+ in solution
What is an Arrhenius base?
Dissociate to form an excess of OH− in solution
What is a Bronsted-Lowry acid?
species that donates hydrogen ions (H+)
What is Bronsted-Lowry base?
species that accepts hydrogen ions (H+),
What is a Lewis acid?
electron pair acceptor
What is a Lewis base?
electron pair donor
What is an amphoteric species?
Reacts like an acid in a basic
environment and like a base in an acidic environment.
What is an amphiprotic species?
Amphoteric species that specifically can behave as a Brønsted–Lowry acid or Brønsted–Lowry base.
What is the water dissociation constant?
Kw, is 10^−14 at 298 K. Like other equilibrium constants, only affected by changes in temperature
*pH = 7 = neutral is only valid at 25 C
What is pH + pOH?
14 at 298 K
What happens to strong acid and bases in solution?
Completely dissociate
What signifies weak acids and bases not dissociating completely?
dissociation constants (Ka and Kb)
How are the conjugates produced from strong acids/bases and weak acids/bases?
All the conjugates are weak
What is the scale for conjugates?
The stronger the acid/base the weaker its conjugate
What do neutralization rxns form?
salts and (sometimes) water
What is an equivalent?
one mole of the species of interest
What is the titrant?
Has a known concentration and is added slowly to the titrand to reach the equivalence point.
What is the titrand?
titrant added to it.
has an unknown concentration but a known volume.
What is the half-equivalence point?
the midpoint of the buffering region, in which half of the titrant has been protonated (or deprotonated); thus, [HA] = [A−] and a buffer is formed.
What is the equivalence point?
Indicated by the steepest slope in a titration curve.
When acid and base are equal
What is the equivalence point for strong acid and strong base?
pH =7
What is the equivalence point for weak acid and strong base?
pH >7
What is the equivalence point for strong acid and weak base?
pH < 7
What is the equivalence point for weak acid and weak base?
can have equivalence points above or below 7
What is the endpoint of titration?
when the indicator reaches its final color
*indicator is always a weaker acid or base
What are found in polyvalent acid and base titrations?
Multiple buffering regions and equivalence points
What do buffer solutions consist of?
a mixture of a weak acid and its conjugate salt or a weak base and its conjugate salt
*optimally buffered means
pH = pKa and pOH = pKb
What is the product of a rxn between strong acid and a weak base?
salt, but no water is formed
