1. 5.1B Acids and Bases (Part 2)

2. 1. Acids can sometimes be identified by their formula
a. Some substances will act as an acid only when dissolved in water, e.g HCl (aq)
b. Most acids begin with hydrogen, e.g. HCl, H2S, H2SO4, HF
i. The main exception are the organic acids which contain carbon, e.g. CH3COOH (aq)

3. 2. Naming acids Non-oxy acids Oxy acids HCl, HNO3 HBr H2SO4, HI H3PO4
a. There are two major groups of acids
i. Non-oxy acids which are usually binary compounds, hydrogen and one other element, e.g. HCl, HBr, HI
ii. Oxy acids which contain oxygen in the negative polyatomic ion, e.g. HNO3, H2SO4, H3PO4
Non-oxy acids
Oxy acids
HCl,
HNO3
HBr
H2SO4, HI
H3PO4

4. b. Non oxy-acids names i. begin with “hydro”
ii. change the ending of the negative ion name to “ic”
Formula
Formula in solution
Chemical Name
Acid name
HCl
HCl (aq)
HBr
HBr (aq)
H2S
H2S(aq)
H3P
H3P (aq)

5. b. Non oxy-acids names i. begin with “hydro”
ii. change the ending of the negative ion name to “ic”
Formula
Formula in solution
Chemical Name
Acid name
HCl
HCl (aq)
Hydrogen chloride
Hydrochloric acid
HBr
HBr (aq)
H2S
H2S(aq)
H3P
H3P (aq)

6. b. Non oxy-acids names i. begin with “hydro”
ii. change the ending of the negative ion name to “ic”
Formula
Formula in solution
Chemical Name
Acid name
HCl
HCl (aq)
Hydrogen chloride
Hydrochloric acid
HBr
HBr (aq)
Hydrogen bromide
Hydrobromic acid
H2S
H2S(aq)
H3P
H3P (aq)

7. b. Non oxy-acids names i. begin with “hydro”
ii. change the ending of the negative ion name to “ic”
Formula
Formula in solution
Chemical Name
Acid name
HCl
HCl (aq)
Hydrogen chloride
Hydrochloric acid
HBr
HBr (aq)
Hydrogen bromide
Hydrobromic acid
H2S
H2S(aq)
Hydrogen sulphide
Hydrosulphuric acid
H3P
H3P (aq)

8. b. Non oxy-acids names i. begin with “hydro”
ii. change the ending of the negative ion name to “ic”
Formula
Formula in solution
Chemical Name
Acid name
HCl
HCl (aq)
Hydrogen chloride
Hydrochloric acid
HBr
HBr (aq)
Hydrogen bromide
Hydrobromic acid
H2S
H2S(aq)
Hydrogen sulphide
Hydrosulphuric acid
H3P
H3P (aq)
Hydrogen phosphide
Hydrophosphoric acid

9. c. Oxy-acids names
i. If the original negative polyatomic ion ended with “ate”, change the ending to “ic”
ii. If the original negative polyatomic ion ended with “ite”, change the ending to “ous”
Formula
Formula in solution
Chemical Name
Acid name
HNO3
HNO3 (aq)
H2SO4
H2SO4 (aq)
H3PO4
H3PO4 (aq)
H2SO3
H2SO3 (aq)
HNO2
HNO2 (aq)

10. c. Oxy-acids names
i. If the original negative polyatomic ion ended with “ate”, change the ending to “ic”
ii. If the original negative polyatomic ion ended with “ite”, change the ending to “ous”
Formula
Formula in solution
Chemical Name
Acid name
HNO3
HNO3 (aq)
Hydrogen nitrate
Nitric acid
H2SO4
H2SO4 (aq)
H3PO4
H3PO4 (aq)
H2SO3
H2SO3 (aq)
HNO2
HNO2 (aq)

11. c. Oxy-acids names
i. If the original negative polyatomic ion ended with “ate”, change the ending to “ic”
ii. If the original negative polyatomic ion ended with “ite”, change the ending to “ous”
Formula
Formula in solution
Chemical Name
Acid name
HNO3
HNO3 (aq)
Hydrogen nitrate
Nitric acid
H2SO4
H2SO4 (aq)
Hydrogen sulphate
Sulphuric acid
H3PO4
H3PO4 (aq)
H2SO3
H2SO3 (aq)
HNO2
HNO2 (aq)

12. c. Oxy-acids names
i. If the original negative polyatomic ion ended with “ate”, change the ending to “ic”
ii. If the original negative polyatomic ion ended with “ite”, change the ending to “ous”
Formula
Formula in solution
Chemical Name
Acid name
HNO3
HNO3 (aq)
Hydrogen nitrate
Nitric acid
H2SO4
H2SO4 (aq)
Hydrogen sulphate
Sulphuric acid
H3PO4
H3PO4 (aq)
Hydrogen phosphate
Phosphoric acid
H2SO3
H2SO3 (aq)
HNO2
HNO2 (aq)

13. c. Oxy-acids names
i. If the original negative polyatomic ion ended with “ate”, change the ending to “ic”
ii. If the original negative polyatomic ion ended with “ite”, change the ending to “ous”
Formula
Formula in solution
Chemical Name
Acid name
HNO3
HNO3 (aq)
Hydrogen nitrate
Nitric acid
H2SO4
H2SO4 (aq)
Hydrogen sulphate
Sulphuric acid
H3PO4
H3PO4 (aq)
Hydrogen phosphate
Phosphoric acid
H2SO3
H2SO3 (aq)
Hydrogen sulphite
Sulphurous acid
HNO2
HNO2 (aq)

14. c. Oxy-acids names
i. If the original negative polyatomic ion ended with “ate”, change the ending to “ic”
ii. If the original negative polyatomic ion ended with “ite”, change the ending to “ous”
Formula
Formula in solution
Chemical Name
Acid name
HNO3
HNO3 (aq)
Hydrogen nitrate
Nitric acid
H2SO4
H2SO4 (aq)
Hydrogen sulphate
Sulphuric acid
H3PO4
H3PO4 (aq)
Hydrogen phosphate
Phosphoric acid
H2SO3
H2SO3 (aq)
Hydrogen sulphite
Sulphurous acid
HNO2
HNO2 (aq)
Hydrogen nitrite
Nitrous acid

15. 3. The formulas of bases can usually be identified by the hydroxide group (OH)
a. E.g. Ca(OH)2, NaOH, KOH
b. Bases may also have more common names
c. Solutions of highly reactive bases are called caustic solutions
i. Caustic solutions can burn human skin and tissue
ii. Solutions of highly reactive acids are called corrosive solutions

16. Formula
Chemical name
Common name
NaOH
Mg(OH)2
Ca(OH) 2

17. Formula
Chemical name
Common name
NaOH
Sodium hydroxide
Caustic soda, lye
Mg(OH)2
Ca(OH) 2

18. Formula
Chemical name
Common name
NaOH
Sodium hydroxide
Caustic soda, lye
Mg(OH)2
Magnesium hydroxide
Milk of magnesia
Ca(OH) 2

19. Formula
Chemical name
Common name
NaOH
Sodium hydroxide
Caustic soda, lye
Mg(OH)2
Magnesium hydroxide
Milk of magnesia
Ca(OH) 2
Calcium hydroxide
Hydrated lime

20. 4. Another way of defining acids and bases is by the types of ions that they produce
a. an acid is a compound that produces hydrogen (H+) ions in solution
i. HCl(aq)  H+(aq) + Cl-(aq)
ii. H2SO4(aq)  2H+ (aq) + SO42- (aq)
b. A base is a compound that produces hydroxide (OH-) ions in solution
i. NaOH(aq)  Na+(aq) + OH- (aq)
ii. Mg(OH)2(aq)  Mg2+(aq) + 2OH- (aq)

21. 5. pH can be seen as a measure of the concentration of hydrogen ions in a solution
a. concentration refers to the number of hydrogen ions in a specific volume (usually litres) of solution
b. a highly acidic solution will have a
i. low pH
ii. a high concentration of hydrogen (H+) ions
c. highly basic/alkaline solution will have a
i. high pH
ii. a high concentration of hydroxide (OH-) ions

22. c. It is impossible for a solution to have both high hydrogen and hydroxide ion concentrations
i. The two ions react together to form water
ii. H+ + OH-  H2O
d. If an acid and a base are mixed together, the two solution can neutralize each other
i. Acid + base  salt + water
ii. HCl + NaOH  NaCl + H2O