1. Acids and Bases

2. Properties of Acids Acidus – meaning sour or tart Feels like water
Litmus Paper – red
Conducts electricity
Reactive with metals
React with bases to form a salt and water

3. Properties of Bases Bitter taste Feels smooth and slippery (soap)
Litmus Paper – Blue
Conducts electricity
Not reactive with metals
React with acids to form a salt and water

4. Common Acids Formula Name HCl Hydrochloric acid HNO3 Nitric Acid H2SO4
Sulfuric Acid
HC2H3O2
Acetic Acid
H2CO3
Carbonic Acid
H3PO4
Phosphoric Acid

5. Common Bases Formula Name Na(OH) Sodium Hydroxide K(OH)
Potassium Hydroxide
Mg(OH)2
Magnesium Hydroxide
Ca(OH)2
Calcium Hydroxide
Sr(OH)2
Strontium Hydroxide

6. Names of Acid/Base IonsH+
H3O+
OH-

7. Arrhenius Acid
Acid: substance that produces hydrogen ions (H+) or hydronium ions (H3O+) in water
H+ = H3O+
THEY ARE THE SAME THING!!
Example:
HCl + H2O  Cl H3O+

8. Arrhenius Base
Base: substance that produces hydroxide ions (OH-) in water
Example:
Na(OH)  Na+ + (OH)-

9. Monoprotic Acids Polyprotic Acids
monoprotic acid : acid that can donate only one proton (hydrogen ion) per molecule.
Example: HCl, HNO3
polyprotic acid : acid that can donate more than one proton per molecule.
Examples: H2SO4 - diprotic
H3PO4 - triprotic
Polyprotic Acids

10. Monoprotic and Diprotic Acids

11. pH Calculations

12. To measure the concentration of these ions produced we use pH
Ionization of Water
Experiments have shown that pure water, at 25°, breaks apart (ionizes) :
H20 + H H30+ + OH-
To measure the concentration of these ions produced we use pH

13. pH Scale Acidic Basic NEUTRAL pH [ H+ ]=10-7 M=[OH- ] pH = 7
Acidic
Basic
NEUTRAL pH
[ H+ ]=10-7 M=[OH- ]
pH = 7
More acidic
More basic

14. Relationship of [H3O+] to [OH–]

15. pH - from the Danish: “power of Hydrogen”
The pH Scale
pH: scale used to indicate the [H+] of a water solution
pH - from the Danish: “power of Hydrogen”
pH = - log [H+]
or pH = - log [H3O+]

16. pH = - log [H+]
The log function converts the exponents with a base of 10 to a whole number.
The negative sign at the front of the equation cancels out with the negative sign in the exponent.
[H+]:
pH :

17. pH Practice 10-2 2 Acid 10-8 10-5 10-7 13 [H+] Concentration pH
Acid, Base, or Neutral?
10-2 2
Acid
10-8
10-5
10-7 13

18. Acids/ bases
Oven cleaner
Surface Cleaner
Detergent
Coffee
Soda

19. Acid Base Reactions

20. Neutralization Reactions
forms salt
forms water
neutralization: when an acidic solution (with hydrogen ions) and a basic solution (with hydroxide ions) react to form water
salt: an ionic compound formed from the cation of a base and an anion of an acid.

21. Neutralization Reactions

22. Buffer Solutions A solution that resists changes in pH
What are some solutions that need to maintain a certain pH level?
Blood, stomach acid (antacids), pools

23. Acid Rain
NO, NO2, CO2, SO2, and SO3 are gases from industrial processes that dissolve in atmospheric water to produce acidic solutions.
Example:
Very acidic rain is known as acid rain.

24. Why is acid rain dangerous?

25. Why is acid rain dangerous?