Acids and Bases APChem

pH of pure water is only […] when temp. is 25°C.

7

Acids donate

[H+]

Bases accept

[H+]

The pH of acids are less than

7

pH of bases are greater than

7

equation for solving pH

pH = −log [H+]

equation for solving for [H+]

[H+] = 10−pH

perchloric acid

strong acid

HClO4

strong acid

hydrochloric acid

strong acid

HCl

strong acid

HBr

strong acid

hydrobromic acid

strong acid

hydroiodic acid

strong acid

HI

strong acid

HNO3

strong acid

nitric acid

strong acid

H2SO4

strong acid

LiOH

strong base

lithium hydroxide

strong base

NaOH

strong base

sodium hydroxide

strong base

KOH

strong base

potassium hydroxide

strong base

Ca(OH)2

strong base

calcium hydroxide

strong base

Sr(OH)2

strong base

strontium hydroxide

strong base

Ba(OH)2

strong base

barium hydroxide

strong base

sulfuric acid

strong acid

The stronger the acid

the weaker its conjugate base

acid base favors […] side

strong; if K>1, reactants are stronger

“x” in the ice box calculation is

[H+] for a weak acid, and [OH−] for a weak base.

% Ionization of a weak acid

[H+] /Ma

% ionization increases as

[acid] decreases; Adding more water will increase the amount of ionization.

If a salt contains a conjugate base of a weak acid, the salt will be slightly

basic; CBOWA’s are (-) ions.

If a salt contains a conjugate acid of a weak base, the salt will be slightly

acidic; CAOWB’s are (+) ions.

If a salt contains conjugates of strong acid/bases, the ion is

neutral; KBr is a neutral salt (KOH + HBr)

A larger Ka value means

a stronger acid.

A larger Kb means

a stronger base.

Buffers are created by

a weak acid + CB (salt) or by a weak base + CA (salt)

Adding a common ion to a weak acid (or base) decreases the

% ionization, so the pH gets closer to 7.

This is only true at the equivalence point.

MaVa=MbVb

More buffer capacity =

more moles of weak acid & CB (or weak base and CA).

The larger the “x” value,

the more soluble the salt is.

If Q > Ksp then

a precipitate forms.

Group I cations, NH4+, and NO3- salts are always

soluble in water; Usually spectator ions in a chemical reaction.

Indicators should change color in the

range of the eq. pt.

At the 1⁄2 equivalence point for a “weak + strong” titration

pH = pKa; When pH = pKa, then [HA] = [A−]