The value of Kw _____________ as temperature increases.
pH + pOH = ?
pKa + pKb = ?
Salts made from a weak acid and strong base are ____________ in solution.
Salts made from a strong acid and weak base are _____________ in solution.
Salts made from a strong acid and strong base are _____________ in solution.
The acidity of salts depends on the _________ and _________ of the cation.
A solution that resists changes in pH when a small amount of strong acid or strong base is added
A buffer consists of a weak acid or base and a(n) ______________ amount of its salt.
The pH is equal to the _________ when the concentration of an acid and its conjugate base are equal.
The dissociation of HA is minimal.
What assumption is made in problems involving weak acid dissociation?
The weaker an acid is, the ___________ the value of the Ka is.
Example of a buffer: ammonia and __________
Example of a buffer: ethanoic acid and ___________
To prepare a buffer, combine equal ___________ of equal _____________ of an acid and its salt.
To prepare a buffer, combine a certain number of moles of a weak acid with ___________ the number of moles of a strong base.
Salts whose cation has a high ______________ will be acidic.
In titrations, the name given to the point at which an equal number of moles of acid/base have been combined
A strong acid titrated with strong base gives a(n) ______________ solution.
A weak acid titrated with strong base gives a(n) _____________ solution.
Strong acid titrated with weak base gives a(n) ______________ solution.
Part of a titration curve where the solution maintains the most constant pH (pKa = pH, the amount of base equal to half the amount required to reach equivalence has been added).
A weak acid or weak base whose salt is a different color; used in titrations
Which indicator should be used for the titration of a strong acid with a strong base?
Which indicator should be used for the titration of a weak acid with a strong base?
Which indicator should be used for the titration of a strong acid with a weak base?
An indicator should be chosen with a pKa as close to the pH of the _____________ as possible (within one pH unit).
Phenolphthalein is _________ in acid and __________ in base.
Methyl orange is _________ in acid and __________ in base.
The symbol used to represent an indicator is _______.
1.00 x 10 ^ -14
Kw = [H+][OH-] = ?
For the dissociation of a weak acid (HA (aq) <----> H+ (aq) + A- (aq)), Ka = ?
A substance that can accept a proton
A substance that can donate a proton
An electron pair acceptor
An electron pair donor
HCl, HNO3, H2SO4
Three examples of strong acids
NaOH, KOH, Ba(OH)2
Three examples of strong bases
Two examples of weak acids
Two examples of weak bases
Acids participate in _____________ reactions with bases.
Acids react with carbonates and hydrogen carbonates to produce __________ and __________.
Acids react with metals above hydrogen in the reactivity series to produce __________ and a ___________.
An acid is ____________ if it dissociates to give 2 mol of hydrogen ions in solution (for a strong one of these, [H+] will be twice the concentration of the acid).
H3O+ (aq) + A- (aq)
HA (aq) + H2O (aq) <----> ?
Ka x Kb = ?
aluminum, iron (III)
Two examples of ions with a high charge density that form acidic salts
BH+ (aq) + OH- (aq)
B (aq) + H2O (aq) <----> ?
For the dissociation of a weak base, Kb = ?
The weaker an acid is, the _____________ the pKa is.
Ka x ([HA]/[A-])
The [H+] of a buffer solution = ?