5 Steps to a 5 AP Chemistry

4. Nitric, HNO 3


5. Chloric, HClO 3


6. Perchloric, HClO 4


7. Sulfuric, H 2 SO 4

The strong acids above are all compounds that ionize completely in aqueous solution,

yielding hydrogen ions and the anions from the acid.

Strong bases include:

1. Alkali metal (Group IA) hydroxides (LiOH, NaOH, KOH, RbOH, CsOH)


2. Ca(OH) 2 , Sr(OH) 2 , and Ba(OH) 2

The strong bases listed above are all compounds that dissociate completely, yielding the

hydroxide ion (which is really the base, not the compound).

Unless told otherwise, assume that acids and bases not on the lists above are weak and

will establish an equilibrium system when placed into water.

Some salts have acid–base properties. For example, ammonium chloride, NH 4 Cl, when

dissolved in water will dissociate and the ammonium ion will act as a weak acid, donating

a proton. We will examine these acid–base properties in more detail in the next section.

Certain oxides can have acidic or basic properties. These properties often become evi-

dent when the oxides are dissolved in water. In most case, reactions of this type are not

redox reactions.

Many oxides of metals that have a +1 or +2 charge are called basic oxides (basic

anhydrides), because they will react with acids.

Many times they react with water to form a basic solution:

Many nonmetal oxides are called acidic oxides (acidic anhydrides), because they react

with water to form an acidic solution:

H 2 CO 3 (aq) is named carbonic acid and is the reason that most carbonated beverages

are slightly acidic. It is also the reason that soft drinks have fizz, because carbonic acid will

decompose to form carbon dioxide and water.

Acid–Base Reactions

In general, acids react with bases to form a salt and, usually, water. The salt will depend

upon which acid and base are used:

HCl aq NaOH aq H O l NaCl aq

HNO aq KOH aq

() () () ()

() (

+→+

+

2

3 ))() ()

() () ()

→+

+→

HOl KNO aq

HBraq NH aq NHBraq

23

34

CO g 22 ()+→H O l() H CO aq 23 ( )

Na O s H O l NaOH aq

Na O s H O l Na

22

22

2

2

() () ( )

() ()

+→

+→+(()+ 2 −()aq OH aq

Fe O s HCl aq FeCl aq H O l

Fe O s

23 3 2

23

() 623 () () ()

(

+→ +

))() () ()+→ + 623 Haq++Fe aq^3 HOl 2

Reactions and Periodicity  77

STRATEGY