Naming Acids
chapter 6
lesson 2
Objective
You will be able to;
· name acids using the classical naming
system.
· name acids according to the IUPAC
system
· cite examples of common acids
IUPAC Naming
The international union of pure and applied
chemists are responsible for the world wide
chemistry standards.
To name acids according to IUPAC rules you
simply name the molecular compound and
preface it with aqueous. Why would we do this?
Classical Naming System
This is still the most common system used in
industry.
The molecular name is changed as follows:
hydrogen -----ide becomes hydro---ic acid
Ex: hydrogen sulfide →
hydrogen -----ate becomes -----ic acid
Ex: hydrogen phosphate →
hydrogen -----ite becomes ----ous acid
Ex: hydrogen phosphite →
Common Acids
stomach acid = hydrochloric acid: HCl
(aq)
muriatic acid= HCl(aq) weak form of the acid
vinegar= ethanoic acid or acetic acid: CH3COOH (aq)
carbonic acid: H2CO3 (aq)= fizz in pop
sulfuric acid : H2SO4 (aq)= acid rain or battery acid
nitric acid: HNO3 (aq) = acid rain
benzoic acid: C6H5COOH (aq)=food preservative
Note: when the hydrogen is bonding with an ion that ends in
--COO then the H is placed after it.
Other common names for polyatomic ions.
There many ions not listed in your table that
commonly exist. The rules for these have to do with
numbers of oxygens.
The ---ate ending is the most common of that ion.
Example: chlorate ClO3The ---ite ending has one less oxygen than the 'ate'
Example: chlorite ClO2The hypo---ite means two less oxygen than the 'ate'
Example: hypochlorite ClO
The per---ate means one more oxygen.
Example: perchlorate ClO4-
Assignment
Do p. 209 #1,2, worksheet