Acids and Bases

strong acid

HCl (hydrochloric acid)

strong acid

H2SO4 (sulfuric acid)

strong acid

HNO3 (nitric acid)

weak acid

CH3COOH (acetic acid)

weak acid

H2CO3 (carbonic acid)

weak acid

H3PO4 (phosphoric acid)

strong base

NaOH (sodium hydroxide)

strong base

KOH (potassium hydroxide)

strong base

LiOH (lithium hydroxide)

strong base

Mg(OH)2 (magnesium hydroxide)

strong base

Ca(OH)2 (calcium hydroxide)

weak base

NH3 (ammonia)

weak base

Cu(OH)2 (copper 2 hydroxide)

weak base

Al(OH)2 (Aluminum Hydroxide)

weak base

Fe(OH)2 (Iron 2 hydroxide)

Bronsted-Lowry acid

* H+ donor
* Typically start with Hydrogen, then donate it
* Form a conjugate base

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Bronsted-Lowry base

* H+ acceptor
* OH -> hydroxide
* Ammonia -> NH3
* Metal Oxide
* Form a conjugate acid

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Conjugate Pair

A pair of substances that differ by a proton.

Neutralization Reaction

acid + base -\> salt + water

acid + metal --\>

H2(g) + salt

acid + carbonate --\>

CO2(g) + water + salt

salt

made from the anion of the acid and the cation of the base

acid + metal oxide --\>

salt + water

acid + metal hydroxide --\>

salt + water

Neutralization reaction with ammonia

acid + NH3 --\> only one product

Acid + metal carbonate --\>

salt + water + carbon dioxide

acid + active metal --\>

salt + H2

active metal

metals above hydrogen on the activity series

anion hydrolysis

when an acid is weak, the conjugate base is strong enough to hydrolize water

anion (A-)

is a conjugate base of the parent acid

cation hydrolysis

when the base is weak and this conjugate is a nonmetal, the conjugate acid is strong enough to hydrolyze water

hydrolysis

A chemical process that splits a molecule by adding water.

cation (M+)

is a conjugate acid of the parent base

cation hydrolysis produces

H+ ions

anion hydrolysis produces

OH- ions

H+ ions in a substance indicate:

acidity

OH- ions in a substance indicate:

basic-ness

all strong bases...

are hydroxides with metals from groups 1 or 2

Lewis Acid

electron pair acceptor

Lewis base

electron pair donor

Weak acid definition

A proton donor that does NOT completely dissociate in water

Weak base definition

A proton acceptor that does NOT completely dissociate in water

pH definition

measure of hydrogen ion concentration

explain conductivity's role in determining strength of an acid

The stronger the acid, the more percent of the acid is dissociated in water. The more dissociation occurs to ionic compounds, the more conductive they are.

three methods to distinguish between strong and weak acids and bases

* measure electrical conductivity (the higher the conductivity the stronger the acid or base)
* react an acid with an active metal or metal carbonate (violent reactions indicate stronger acids)
* check the pH, lower pH= stronger acid, higher pH=stronger base

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strong acid --\>

weak conjugate base

weak acid --\>

strong conjugate base

strong base --\>

weak conjugate acid

weak base --\>

strong conjugate acid

strong parent acid --\>

no anion hydrolysis

strong parent base --\>

no cation hydrolysis

the bond between lewis acids and bases

covalent, because both electrons are provided by only one of the atoms

choosing an indicator for titrations

choose one within the same pH range as the reaction

strong acid + strong base --\>

salt has a neutral pH

strong acid + weak base --\>

salt is slightly acidic

weak acid + strong base --\>

salt is slightly basic

weak acid + weak base --\>

pH depends on relative strength of reactants

Kw Constant

1.0x10^-14 (in the IB booklet)

Equilibrium constant Kc

(conc. H+ X conc. OH-) / (conc. H2O)

Kw equation

Kw\=[H+][OH-] at 298K

pH range of [H+] \= [OH-]

neutral; 7

pH range of [H+] \> [OH-]

acidic

pH range of [H+] < [OH-]

basic

pH changes rapidly at the equivalence point because...

a change of a factor of 10 occurs very quickly, which is why the graph is extremely steep at this point. As the H+ concentration becomes very low, it will require more base to increase the H+ concentration by 10 fold to change the pH significantly

n\=cV

moles \= concentration / volume(in LITERS)