1. Naming Acids and Bases

2. Acids and Bases are both corrosive!
Important Fact:
Acids and Bases are both corrosive!
Acids and bases are a form of ionic compound. Like all other ionic compounds, acids and bases break apart into their ions when they are dissolved in water. Acids and bases are often defined by the ions that they break into.
HCl  H+ + Cl -

3. Arrhenius Definition of Acids and Bases
Svante Arrhenius was a scientist who defined acids and bases. This is the simplest definition of an acid and a base.
He defined an acid as any substance which donates a hydrogen ion (H+).
He defined a base as any substance which donates a hydroxide ion (OH-).

4. Strong acids completely break apart!
Weak Acid
When we talk about acids being strong or weak, we are referring to how well an acid dissociates into ions.
Strong acids completely break apart!
Images from The University of British Columbia

5. The equation for pH: pH = -log [H+]
The acidity of a solution is expressed as its pH and it is based on the concentration of hydrogen ions.
The equation for pH:
pH = -log [H+]

6. Determine pH of each of the solutions on your notes based on the concentration of H+ ions.
1.44
-1.000
0.82
2.04
3.10
4.17
1.12
3.68

7. As the H+ ions increase, the pH decreases!
How would you explain the relationship between pH and the hydrogen ion concentration based on this graph?
As the H+ ions increase,
the pH decreases!

8. Acids have a pH lower than 7. Bases have a pH higher than 7.

9. Pure water has a pH of exactly 7.
All NEUTRAL solutions have a pH of 7.

10. The acidity of a solution can be precisely measured using a pH meter.10

11. Acids turn litmus paper RED. Bases turn litmus paper BLUE.
It can be determined if a solution is acidic or basic by using litmus paper.
Acids turn litmus paper RED.
Bases turn litmus paper BLUE. 11

12. Naming Acids
When it comes to naming acids, there are two categories you need to be familiar with:
Binary Acids: These acids are made of H+ and one other element (often a halogen).
Ex: HCl, HF, HBr, HI
Acids of Oxyanions: These acids are made of H+ and a polyatomic ion containing oxygen.
Ex: H2SO4, HNO3, H3PO4, H2CO3

13. 1. Start with the prefix hydro- 2. Add the root of the anion
Naming Binary Acids
HCl
Hydro
+ chlor ic
acid
1. Start with the prefix hydro-
2. Add the root of the anion
3. End with the suffix -ic
4. Add the word acid
Hydrochloric acid

14. 1. Start with the prefix hydro- 2. Add the root of the anion
Naming Binary Acids
Try it one more time!
HBr
Hydro
+ brom ic
acid
1. Start with the prefix hydro-
2. Add the root of the anion
3. End with the suffix -ic
4. Add the word acid
Hydrobromic acid 14

15. This prefix will NOT appear in the names of acids made from oxyanions.
Naming Binary Acids
It is very important that you remember that binary acids (HF, HCl, HBr, HI) always begin with the prefix hydro-
This prefix will NOT appear in the names of acids made from oxyanions.

16. 1. Start with the prefix hydro- 2. Add the root of the second element
Naming Binary Acids
HI is a slight exception to the rule. We leave the “o” off of the end of hydro HI
Hydr
+ iod ic
acid
1. Start with the prefix hydro-
2. Add the root of the second element
3. End with the suffix -ic
4. Add the word acid
Hydriodic acid

17. Naming Acids of Oxyanions Add the root of the second element
First you must identify the ion. This is nitrate. Since the polyatomic ion ends with –ate, you will end the name of the acid with the suffix –ic.
HNO3
Nitrate
Nitric acid
Nitr ic acid =
Add the root of the second element
End with the suffix -ic
Add the word acid

18. HNO2 Nitrous acid Naming Acids of Oxyanions Nitrite Nitr + ous acid =
This is nitrite. Since the polyatomic ion ends with –ite, you will end the name of the acid with the suffix –ous.
HNO2
Nitrite
Nitrous acid
Nitr ous acid =
Add the root of the second element
End with the suffix -ous
Add the word acid

19. Naming Acids of Oxyanions
While you might think the acids of sulfate (SO4-2) and sulfite (SO3-2) would be sulfic acid and sulfous acid, we actually use more than just the beginning of sulfur in the names of these acids. The same is true for phosphate.
H2SO4
H2SO3
H3PO4
Sulfuric acid
Sulfurous acid
Phosphoric acid

20. Naming Acids: Important Facts
1. Binary acids ALWAYS begin with the prefix hydro-
2. Binary acids ALWAYS end with the suffix -ic
3. Acids of oxyanions NEVER begin with hydro-
4. If an oxyanion end with –ate, its acid will end with –ic.
5. If an oxyanion end with –ite, its acid will end with –ous.

21. Name the acids on your notes according to the rules and information you received in class today.
hydrobromic acid
carbonic acid
nitrous acid
chromic acid
hydrofluoric acid
phosphoric acid
hydrochloric acid
acetic acid

22. NaOH Naming Bases Sodium Hydroxide Sodium Hydroxide
Arrhenius bases are named according to the rules of ionic compounds. We learned these earlier.
NaOH
Remember that Arrhenius defined bases as hydroxide ion donors. This means that every Arrhenius base will contain the anion hydroxide.
Sodium
Hydroxide
Name the metal ion
Name the anion
Sodium Hydroxide

23. Name the bases on your notes according to the rules and information you received in class today.
potassium hydroxide
barium hydroxide
cesium hydroxide
calcium hydroxide
lithium hydroxide
ammonium hydroxide