1. Naming Bases Bases are ionic compounds composed of
a) metallic or positively charged ions
& b) negatively charged hydroxide ion (OH-)
Rule for naming: add the word “hydroxide” to the name of the positive ion
Ex) NaOH KOH Ca(OH)2

2. SALTS
Salts are usually described as ionic solids, made up of a positive metallic ion & a negative non-metallic ion joined together by an ionic bond. Salts may be prepared through the neutralization reaction between an acid & a base. acid + base  salt + water Ex) HCl + NaOH  NaCl + H2O

3. Naming Salts:
The negative ion of a salt is named by using a stem, the name of the acid with a different ending.
The pattern is as follows:
ending of name of acid ending of negative ion
“ic” becomes ate
“ous” becomes ite
Ex) 1. HBrO4 + NaOH  NaBrO4 + H2O
perbromic acid sodium perbromate

4. bromous acid sodium bromite 4. HBrO + NaOH  NaBrO + H2O
bromic acid sodium bromate
3. HBrO2 + NaOH  NaBrO2 + H2O
bromous acid sodium bromite
4. HBrO + NaOH  NaBrO + H2O
hypobromous acid sodium hypobromite
Name the parent acid & base of each salt:
Negative ion – from acid Positive ion – from base
SALT
PARENT ACID
PARENT BASE
KNO3
Na2SO4
LiClO
NaFO4

5. Salts of Diprotic Acids (H2SO4 & H2CO3)
Salt with 1 hydrogen are sometimes indicated by the use of the prefix “bi”.
Ex) NaHSO4  sodium bisulfate or sodium hydrogen sulfate
Salts of Polyprotic Acids (H3PO4)
Prefixes may be used to indicate the number of acid hydrogens remaining.
Ex) H3PO4 - acid parent  phosphoric acid
NaH2PO4  sodium dihydrogen phosphate
Na2HPO4  sodium monohydrogen phosphate
Na3HPO4  sodium phosphate

6. NOTE: the charge of the negative ion is determined by the number of protons (H+) lost.
CO32-  lost 2H+ = H2CO3
PO43-  lost 3H+ = H3PO4
NO2-  lost 1H+ = HNO2
Sample Problems: Name the following salts.
NaFO calcium hyponitrite
KClO2
LiBrO iron (III) percarbonate
NaClO3
HNO