1. Acids and Bases

2. Definitions of Acids
Arrhenius Acid-any substance that produces hydrogen ions (H+) when dissolved in water.
Bronsted Lowry acid-any substance that donates protons to form hydronium ions (H3O+)
Examples of acids: HCl, HNO3, H2SO4, HC2H3O2

3. Properties of Acids Taste sour React with metals Conduct electricity
pH<7
Turn litmus red
Turn phenolphthalein colorless

4. Definitions of Bases
Arrhenius Base-any substance that produces hydroxide ions (OH-) when dissolved in water.
Bronsted Lowry Base- any substance that accepts protons.
Examples of bases: NaOH, Ca(OH)2, Mg(OH)2, NH3

5. Properties of Bases Taste bitter Feel slippery Conduct electricity
pH>7
Turn litmus blue
Turn phenolphthalein pink

6. General formula for Acid in water:
HA (aq) + H2O (l) H3O+ (aq) + A- (aq)

7. NaOH is an example of a(n)10
Acid
Base
Neither 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

8. A substance that is a proton acceptor is a(n)10
Acid
Base
neither 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

9. HCl is an example of a(n)
Acid
Base
Neither 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

10. Lemon juice is an example of a(n)
Acid
Base
Neither 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

11. A substance that is a proton donor is an example of a(n)
Acid
Base
Neither 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

12. Drain cleaner is an example of a(n)
Acid
Base
Neither 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

13. Vinegar is an example of a(n)
Acid
Base
Neither 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

14. Water is an example of a(n)
Acid
Base
Neither 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

15. A substance that turns litmus red is a(n)
Acid
Base
Neither
Both 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

16. A substance that conducts electricity is a(n)
Acid
Base
Neither
Both 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

17. Naming Acids Binary acids- consist of hydrogen and one other element.
Use the prefix –hydro and change the ending of the element to –ic.
Example: HCl hydrochloric acid
HBr hydrobromic acid
H2S hydrosulfuric acid

18. Naming acids
Oxyacids-consist of hydrogen, oxygen, and one additional element.
If the polyatomic ion ends in –ate, change the ending to –ic.
If the polyatomic ion ends in –ite, change the ending to –ous.
Example: H2SO4 sulfuric acid (diprotic)
H2SO3 sulfurous acid (diprotic)
HNO nitric acid (monoprotic)
HNO2 nitrous acid (monoprotic)
H3PO phosphoric acid (triprotic)

19. Naming bases
All bases consist of the hydroxide ion and one additional element.
Name the element followed by hydroxide.
Example: NaOH sodium hydroxide
Ca(OH)2 calcium hydroxide
Al(OH)3 aluminum hydroxide
Fe(OH)3 iron (III) hydroxide

20. Which of the following is the correct name of HBr?10
Hydrobromic acid
Bromic acid
Bromous acid
Bromine hydroxide 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

21. Which of the following is the correct name of H2CO3?10
Hydrocarbonic acid
Carbonic acid
Carbonous acid
Hydrogen coarbon oxide 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

22. Which of the following is the correct name of Ba(OH)2?10
Hydrobaric acid
Baric acid
Barous acid
Barium hydroxide 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

23. pH Scale

24. Calculating pH
The pH scale is a logarithmic scale used to quantitatively represent the strength (concentration) of an acid.
The greater the concentration of the hydrogen ion (H+), the stronger the acid and the lower the pH.

25. Sample Problems What is the pH of a solution in which [H+] = 1 x 10-2?
Which is more concentrated?
pH=2

26. pH and pOH
The pOH scale is a logarithmic scale used to quantitatively represent the strength (concentration) of a base.
The greater the concentration of the hydroxide ion (OH-), the stronger the base and the lower the pOH.
pOH + pH = 14

27. Practice Problems
Calculate the pH and pOH of solutions with the following concentrations and classify as acidic, basic, or neutral.
[OH-] = 1 x 10-9
[H+] = 1 x 10-7
[H+] = 1 x 10-4
[OH-] = 1 x 10-2

28. Indicators and pH
Indicators are substances that change color depending on the concentration of hydrogen ions (H+) in a solution.
Litmus and phenolphthalein are examples of indicators.
Indicators can be used to determine the pH of a solution.

29. A solution with a pH of 3 is10
Acidic
Basic
Neutral 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

30. Which of the following is an expected pH for a sample of lemon juice?10 3 6 7 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

31. A substance with a pH of 12.7 is a(n)
Acid
Base
Neither
Both 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

32. A solution with a [H+] =1x 10-5 has a pH of9 14 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

33. A solution with a pH of 8 has a pOH of10 2 6 8 14 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

34. A solution with a [OH-]=1x10-3 has a [H+] =11
1 x 1011
1 x 10-11 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

35. Neutralization Reactions
Neutralization reactions occur when acids react with bases and produce a salt and water.
A salt is an ionic compound consisting of the positive ion of the base and the negative ion of the acid.
Example: HCl + NaOH  NaCl + H2O
acid base salt water
If the [H+] = [OH-], the resulting solution will be neutral (pH=7).
Neutralization reactions are a specific type of double displacement reaction.

36. What salt is formed? HCl + KOH  H3PO4 + NaOH  Ca(OH)2 + H2SO4 
Mg(OH)2 + HF 
HNO3 + NaOH 

37. Titration
A titration is a method for determining the concentration of a solution by reacting a known volume of that solution with a solution of known concentration.
The reaction that takes place is a neutralization reaction.

39. Pre-lab: Which is the most effective antacid?
What makes an antacid effective?
How does the antacid affect the acid?
How will you determine which antacid is most effective at neutralizing the stomach acid?