1. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Properties of Acids and Bases
What are the properties of acids and bases?

2. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Acids
Acids taste sour
Change the color of an acid-base indicator
Litmus paper demonstration
Universal Indicator Demonstration
Strong or weak electrolytes in aqueous solution
Strong acids/bases = strong electrolytes
Weak acids/bases = weak electrolytes
Light bulb demonstration

3. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Citrus fruits contain citric acid. Tea contains tannic acid.
Many items contain acids or bases, or produce acids and bases when dissolved in water. a) Citrus fruits contain citric acid. b) Tea contains tannic acid. c) Antacids use bases to neutralize excess stomach acid. d) The base calcium hydroxide is a component of mortar.

4. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Bases
Taste bitter
Feel slippery
Change the color of an acid-base indicator
Strong or weak electrolytes in aqueous solution.

5. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Antacids use bases to neutralize excess stomach acid. The base calcium hydroxide is a component of mortar.
Many items contain acids or bases, or produce acids and bases when dissolved in water. a) Citrus fruit contain citric acid. b) Tea contains tannic acid. c) Antacids use bases to neutralize excess stomach acid. d) The base calcium hydroxide is a component of mortar.

6. A quick Video Review of Acids and Base Characteristics
Another Quick Video

7. Naming Acids – A Quick Overview
Binary Acids
Hydro then –ic
Just Remember
I –ate it and it was –ic
I caught an –ite -ous

8. If the ion ends in –ate change the acid name to –ic
For example
Carbonate ion CO32-
Carbonic acid H2CO3
Sulfate ion SO42-
Sulfuric Acid H2SO4

9. If the ion ends in –ite change the acid name to –ous
For example
Nitrite ion NO2-
nitrous acid HNO2
Sulfite ion SO32-
Sulfurous Acid H2SO3

10. Naming Binary Acids
HCl
H2S
Hydrobromic acid
Hydroiodic acid

12. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
Be sure to add the correct number
of hydroxide groups to the metal ion
If metal ion is +1 charge add 1 OH- group
If metal ion is +3 charge add 3 OH- groups

13. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
A common Base
Milk of magnesia is a base used as an antacid.
Milk of magnesia is a base used as an antacid. Bases are usually hazardous when taken internally, but the low solubility of milk of magnesia makes it safe to use.

14. Hydrogen Ions and Acidity
19.2
To test a diagnosis of diabetic coma, a doctor orders several tests, including the acidity of the patient’s blood. Results from this test will be expressed in units of pH. You will learn how the pH scale is used to indicate the acidity of a solution and why the pH scale is used.

15. Ion Product Constant for Water
19.2
Ion Product Constant for Water
An acidic solution is one in which [H+] is greater than [OH-].

16. Ion Product Constant for Water
19.2
Ion Product Constant for Water
Unrefined hydrochloric acid, commonly called muriatic acid, is used to clean stone buildings and swimming pools.
Acids and bases have many uses in the home and in industry. a) Unrefined hydrochloric acid, commonly called muriatic acid, is used to clean stone buildings and swimming pools. b) Sodium hydroxide, or lye, is commonly used as a drain cleaner. Predicting How will each chemical affect the hydrogen-ion and hydroxide-ion concentration of an aqueous solution?

17. Ion Product Constant for Water
19.2
Ion Product Constant for Water
A basic solution is one in which [H+] is less than [OH]. Basic solutions are also known as alkaline solutions.

18. Ion Product Constant for Water
19.2
Ion Product Constant for Water
Sodium hydroxide, or lye, is commonly used as a drain cleaner.
Acids and bases have many uses in the home and in industry. a) Unrefined hydrochloric acid, commonly called muriatic acid, is used to clean stone buildings and swimming pools. b) Sodium hydroxide, or lye, is commonly used as a drain cleaner. Predicting How will each chemical affect the hydrogen-ion and hydroxide-ion concentration of an aqueous solution?

19. 19.2
The pH Concept
The pH Concept
How is the hydrogen-ion concentration used to classify a solution as neutral, acidic, or basic?

20. 19.2
The pH Concept
The pH of a solution is the negative logarithm of the hydrogen-ion concentration.

21. Is the solution acidic or basic?
19.2
The pH Concept
Calculating pH
What is the pH of solution if the [H3O+] is 2.3 x 10-13?
Is the solution acidic or basic?

22. Is the solution acidic or basic?
19.2
The pH Concept
Calculating pH
What is the pH of solution if the [H3O+] is 4.7 x 10-5?
Is the solution acidic or basic?

23. Is the solution acidic or basic?
19.2
The pH Concept
Calculating pH
What is the pH of solution if the [H3O+] is 1.0 x 10-7?
Is the solution acidic or basic?

24. 19.2
The pH Concept
Calculating pOH
What is the pOH of a solution where [OH-] =3.4 x 10-12?

25. What is the pOH of a solution where [OH-] =5.3 x 10-5?

26. Given [OH-]…how can you find pH?

27. If [OH-] = 5.6 x 10-9, what is the pH?

28. If [OH-] = 2.3 x 10-7, what is the pH?

29. If [OH-] = 1.0 x 10-7, what is the pH?

30. A game to see what you know about pH and pOH

31. 19.2
pH scale
The pH scale shows the relationship between pH and the hydrogen-ion concentration. Interpreting Diagrams What happens to [H+] as pH increases?

32. 19.2

33. 19.4

34. Neutralization Reactions
19.4
Excess hydrochloric acid in the stomach can cause heartburn and a feeling of nausea. Antacids neutralize the stomach acid and relieve the pain of acid indigestion. You will learn what a neutralization reaction is.

35. 19.4
Acid-Base Reactions
Acid-Base Reactions
What are the products of the reaction of an acid with a base?
A Molecular Model Simulation

36. Neutralization Reactions Acid + Base → Salt + Water
19.4
Acid-Base Reactions
Neutralization Reactions
Acid + Base → Salt Water

37. 19.4
Acid-Base Reactions

38. Predict the Products of the Following Reactions
HBr LiOH →
HNO Mg(OH)2 →
H2SO KOH →