Naming Bases

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 acidending of negative ion “ic” becomes ate “ous” becomes ite Ex)1. HBrO4 + NaOH NaBrO4+ H2O perbromicacid sodium perbromate

4. 2. HBrO3 + NaOH NaBrO3 + 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

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. • NaFO4 6. calcium hyponitrite • KClO2 • LiBrO 7. iron (III) percarbonate • NaClO3 • HNO