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HL material with some review of SL material

increases

The value of Kw _____________ as temperature increases.

14

pH + pOH = ?

pH

-log[H+]

14

pKa + pKb = ?

alkaline

Salts made from a weak acid and strong base are ____________ in solution.

acidic

Salts made from a strong acid and weak base are _____________ in solution.

neutral

Salts made from a strong acid and strong base are _____________ in solution.

size, charge

The acidity of salts depends on the _________ and _________ of the cation.

buffer

A solution that resists changes in pH when a small amount of strong acid or strong base is added

equimolar

A buffer consists of a weak acid or base and a(n) ______________ amount of its salt.

pKa

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?

lower

The weaker an acid is, the ___________ the value of the Ka is.

ammonium chloride

Example of a buffer: ammonia and __________

sodium ethanoate

Example of a buffer: ethanoic acid and ___________

volumes, concentrations

To prepare a buffer, combine equal ___________ of equal _____________ of an acid and its salt.

one half

To prepare a buffer, combine a certain number of moles of a weak acid with ___________ the number of moles of a strong base.

charge density

Salts whose cation has a high ______________ will be acidic.

equivalence point

In titrations, the name given to the point at which an equal number of moles of acid/base have been combined

neutral

A strong acid titrated with strong base gives a(n) ______________ solution.

basic

A weak acid titrated with strong base gives a(n) _____________ solution.

acidic

Strong acid titrated with weak base gives a(n) ______________ solution.

buffer region

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).

indicator

A weak acid or weak base whose salt is a different color; used in titrations

any

Which indicator should be used for the titration of a strong acid with a strong base?

phenolphthalein

Which indicator should be used for the titration of a weak acid with a strong base?

methyl orange

Which indicator should be used for the titration of a strong acid with a weak base?

equivalence point

An indicator should be chosen with a pKa as close to the pH of the _____________ as possible (within one pH unit).

colorless, pink

Phenolphthalein is _________ in acid and __________ in base.

red, yellow

Methyl orange is _________ in acid and __________ in base.

HIn (aq)

The symbol used to represent an indicator is _______.

1.00 x 10 ^ -14

Kw = [H+][OH-] = ?

[H+][A-]/[HA]

For the dissociation of a weak acid (HA (aq) <----> H+ (aq) + A- (aq)), Ka = ?

Bronsted-Lowry base

A substance that can accept a proton

Bronsted-Lowry acid

A substance that can donate a proton

Lewis acid

An electron pair acceptor

Lewis base

An electron pair donor

HCl, HNO3, H2SO4

Three examples of strong acids

NaOH, KOH, Ba(OH)2

Three examples of strong bases

CH3COOH, H2CO3

Two examples of weak acids

NH3, amines

Two examples of weak bases

neutralization

Acids participate in _____________ reactions with bases.

CO2, H2O

Acids react with carbonates and hydrogen carbonates to produce __________ and __________.

H2, salt

Acids react with metals above hydrogen in the reactivity series to produce __________ and a ___________.

diprotic

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) <----> ?

Kw

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) <----> ?

[BH+][OH-]/[B]

For the dissociation of a weak base, Kb = ?

higher

The weaker an acid is, the _____________ the pKa is.

Ka x ([HA]/[A-])

The [H+] of a buffer solution = ?

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