2. A.) Nitric acid B.) Hydronitric acid C.) Nitrous acid D.) Hydronitrous acid

3. A.) HS B.) H2S C.) H2SO3 D.) H2SO4

4. A.) Acetic acid B.) Hydroacetic acid C.) Hydrogen acetate D.) Acetous acid

5. A.) HP B.) H3P C.) H3PO3 D.) H3PO4

6.  STEP 1: Does the acid contain a polyatomic ion?  STEP 2:  If YES to polyatomic, then use NO hydro- to begin the name.  If NO to polyatomic, then YES use hydro- to begin the name.  STEP 3:  If hydro- is used, then the name ends with –ic.  If hydro is NOT used, then look closely at the polyatomic ion. ▪ If the ion is an “-ate” ion, then the name ends with –ic. ▪ If the ion is an “-ite” ion, then the name ends with –ous.

7. Does the acid contain a polyatomic ion? If YES, then you’ll use NO hydro- to begin the name. If the polyatomic ion ends with –ate, then end the acid name with –ic. If the polyatomic ion ends with –ite, then end the acid name with –ous. If NO, then (YES) you will use hydro- to begin the name. If the acid begins with hydro-, then it will always end with –ic.

8.  STEP 1: Hydrogen is ALWAYS the first element in the formula of an acid.  STEP 2:  If HYDRO begins the name of the acid, then NO polyatomic ion is present. Simply use the monatomic ion signaled by the acid name.  If HYDRO does NOT begin the name of the acid, then,YES, a polyatomic ion is present. Use the ending of the acid to help you to determine if the ion is an –ate or –ite version.  STEP 3:  Criss-cross the charges of the hydrogen ion (+1) and the monatomic or polyatomic ion.