1. Acids and Bases

2. BELL WORK
*Obtain ipad from cart corresponding to seat number answer survey question! PollEv.com/michellemart898

3. How many foods can you think of that are sour?
sour milk – lactic acid
vinegar – acetic acid
carbonated beverages – phosphoric acid
lemons – citric acid
apples – malic acid
Chances are almost all the foods you thought of owe their sour taste to an acid!

4. Question? Who has heard of someone using an antacid for an upset stomach?
What does this indicate about the contents of our stomach?
Answer! Our stomachs contain acid. Medical antacid preparations typically contain weak bases to counteract high levels of acids.

5. H. pylori
Barry Marshall Nobel Prize 2005

6. Objectives List general properties of aqueous acids and bases.
Name common binary acids and oxyacids.
Explain the difference between strong and weak acids and bases.

7. Acids Characteristics:
sour taste
change color of acid-base indicators
react with bases to produce salts and waters
Acids were 1st recognized as a distinct class of compounds bc of their common properties of their aqueous solutions

8. Acids Conduct Electric Current
Acids Characteristics:
Acids Conduct Electric Current
Acids dissolve in water break into ions
Ions in solution conduct an electric current
Example: Sulfuric acid in car battery conducts electricity to start car’s engine

9. Acids Characteristics:
some acids react with active metals and release hydrogen gas

10. Acid Nomenclature
*binary acid- contains only 2 different elements= H + EN element
*oxyacid- compound of H,O, and a 3rd element, usually a nonmetal

11. Name the following acids:
1. HBr
Hydrobromic acid
2. HNO3
nitric acid
3. H2SO3
sulfurous acid

13. Base Characteristics:
bitter taste in aqueous solutions
corrosive/contact skin can result in severe burns
conduct electric current
change color of acid-base indicators
dilute solutions feel slippery
react with acids to produce salts and water

14. Common Bases Found in cleaning products
Ammonia is in cleaners and fertilizer
Sodium hydroxide is used to make soap (lye)
Milk of magnesia and antacids

16. Svante Arrenhius Swedish chemist 1859-1927
Understood that aqueous solutions of acids and bases conducted an electric current
Theorized that acids and bases must produce certain ions in solution…

17. Arrhenius Acids
def. a chemical compound that will increase the concentration of H+ ions in aqueous solutions
HCl  H+ + Cl-

18. Acids in Water
H+ that separates from the acid and forms with a water molecule H2O to form hydronium ions H3O+

19. Arrhenius Base
substance that will increase the concentration of hydroxide ions (OH-) in water ex: NaOH
NaOH(s) + H20(l) Na+(aq) + OH-(aq) + H2O(l)

20. Ammonia, NH3 Base that does not contain an –OH
In water, ammonia attracts an H+ which leaves an OH-.
household cleaner that should not be mixed with other cleaners that contain chlorine (bleach etc) bc produces toxic gases that can damage to lungs or even death

21. Strong Acids and Bases Strong completely ionizes in aqueous solutions
Weak partially ionizes

22. Relationship of [H3O+] to [OH–]
Section 1 Properties of Acids and Bases
Chapter 14
Relationship of [H3O+] to [OH–]

23. HOMEWORK
Section Review pg 476 #1-5

24. Bell Work
Read the Cross-Disciplinary Connection entitled “Acid Water-A Hidden Menace” on page 477.
Answer the three questions at the end of the article.

25. List 3 terms that describe this person…

28. Section 2 Acid-Base Theories
Chapter 14
Objectives
Define and recognize Brønsted-Lowry acids and bases.
Define a Lewis acid and a Lewis base.
Name compounds that are acids under the Lewis definition but are not acids under the Brønsted-Lowry definition.

29. Brønsted-Lowry Acids and Bases
Section 2 Acid-Base Theories
Chapter 14
Brønsted-Lowry Acids and Bases
A Brønsted-Lowry acid is a molecule or ion that is a proton donor.
Hydrogen chloride acts as a Brønsted-Lowry acid when it reacts with ammonia.
Water can act as a Brønsted-Lowry acid.

30. Brønsted-Lowry Acids and Bases, continued
Section 2 Acid-Base Theories
Chapter 14
Brønsted-Lowry Acids and Bases, continued
A Brønsted-Lowry base is a molecule or ion that is a proton acceptor.
Ammonia accepts a proton from the hydrochloric acid. It acts as a Brønsted-Lowry base.
The OH− ion produced in solution by Arrhenius hydroxide bases (NaOH) is the Brønsted-Lowry base.
The OH− ion can accept a proton

31. Brønsted-Lowry Acids and Bases, continued
Section 2 Acid-Base Theories
Chapter 14
Brønsted-Lowry Acids and Bases, continued
In a Brønsted-Lowry acid-base reaction, protons are transferred from one reactant (the acid) to another (the base).
acid base

32. Monoprotic and Polyprotic Acids
Section 2 Acid-Base Theories
Monoprotic and Polyprotic Acids
A monoprotic acid is an acid that can donate only one proton (hydrogen ion) per molecule.
HClO4, HCl, HNO3 only one ionization step

33. Monoprotic and Polyprotic Acids, continued
Section 2 Acid-Base Theories
Chapter 14
Monoprotic and Polyprotic Acids, continued
A polyprotic acid is an acid that can donate more than one proton per molecule.
H2SO4, H3PO4
Multiple ionization steps
(1)
(2)
Sulfuric acid solutions contain H3O+,
ions

34. Monoprotic and Polyprotic Acids, continued
Section 2 Acid-Base Theories
Chapter 14
Monoprotic and Polyprotic Acids, continued
A diprotic acid is the type of polyprotic acid that can donate two protons per molecule
H2SO4
A triprotic acid is the type of polyprotic acid that can donate three protons per molecule.
H3PO4

35. Chapter 14 Lewis Acids and Bases
Section 2 Acid-Base Theories
Chapter 14
Lewis Acids and Bases
A Lewis acid is an atom, ion, or molecule that accepts an electron pair to form a covalent bond.
The Lewis definition is the broadest of the three acid definitions.
A bare proton (hydrogen ion) is a Lewis acid

36. Lewis Acids and Bases, continued
Section 2 Acid-Base Theories
Chapter 14
Lewis Acids and Bases, continued
The formula for a Lewis acid need not include hydrogen.
The silver ion can be a Lewis acid
Any compound in which the central atom has three valence electrons and forms three covalent bonds can react as a Lewis acid.

38. HOMEWORK pg 482 #1-3 answer on same page as section 1
HOMEWORK pg 482 #1-3 answer on same page as section 1

39. Section 3 Acid-Base Reactions
Chapter 14
Objectives
Describe a conjugate acid, a conjugate base, and an amphoteric compound.
Explain the process of neutralization.
Define acid rain, give examples of compounds that can cause acid rain, and describe effects of acid rain.

40. Conjugate Acids and Bases
Section 3 Acid-Base Reactions
Chapter 14
Conjugate Acids and Bases
The species that remains after a Brønsted-Lowry acid has given up a proton is the conjugate base of that acid.
acid conjugate
base

41. Conjugate Acids and Bases, continued
Section 3 Acid-Base Reactions
Chapter 14
Conjugate Acids and Bases, continued
Brønsted-Lowry acid-base reactions involve two acid-base pairs, known a conjugate acid-base pairs.
acid1 base base acid2

42. Conjugate Acids and Bases, continued
Section 3 Acid-Base Reactions
Chapter 14
Conjugate Acids and Bases, continued
Strength of Conjugate Acids and Bases
The stronger an acid is, the weaker its conjugate base
The stronger a base is, the weaker its conjugate acid
strong acid base acid weak base

43. Conjugate Acids and Bases, continued
Section 3 Acid-Base Reactions
Chapter 14
Conjugate Acids and Bases, continued
Strength of Conjugate Acids and Bases, continued
Proton transfer reactions favor the production of the weaker acid and the weaker base.
stronger acid stronger base weaker acid weaker base
The reaction to the right is more favorable
weaker acid weaker base stronger acid stronger base
The reaction to the left is more favorable

44. Relative Strengths of Acids and Bases
Section 3 Acid-Base Reactions
Chapter 14
Relative Strengths of Acids and Bases
Relative Strengths of Acids and Bases

45. Chapter 14 Amphoteric Compounds
Section 3 Acid-Base Reactions
Chapter 14
Amphoteric Compounds
Any species that can react as either an acid or a base is described as amphoteric.
example: water
water can act as a base
acid1 base2 acid base1
water can act as an acid
base acid acid base2

46. Amphoteric Compounds, continued
Section 3 Acid-Base Reactions
Chapter 14
Amphoteric Compounds, continued
–OH in a Molecule
The covalently bonded OH group in an acid is referred to as a hydroxyl group.
Molecular compounds containing —OH groups can be acidic or amphoteric.
The behavior of a compound is affected by the number of oxygen atoms bonded to the atom connected to the —OH group.

47. Section 3 Acid-Base Reactions
Chapter 14
Oxyacids of Chlorine

48. Neutralization Reactions
Chapter 14
Neutralization Reactions
Strong Acid-Strong Base Neutralization
In aqueous solutions, neutralization is the reaction of hydronium ions and hydroxide ions to form water molecules.
A salt is an ionic compound composed of a cation from a base and an anion from an acid.

50. Neutralization Reactions
Section 3 Acid-Base Reactions
Chapter 14
Neutralization Reactions

51. Chapter 14
Acid Rain
NO, NO2, CO2, SO2, and SO3 gases from industrial processes can dissolve in atmospheric water to produce acidic solutions.
example:
Very acidic rain is known as acid rain.
Acid rain can erode statues and affect ecosystems.

52. Modern Chemistry Chapter 15 Acid-Base pH

53. Draw the chemical formula of a hydroxide ion and a hydronium ion:

54. Self-ionization of water occurs when two water molecules produce a hydronium (H3O+) and a hydroxide (OH-) ion

55. Concentration (moles per liter) = [ ]
In water at 25°C:
[H3O+] = 1.0 x 10-7 M
[OH-] = 1.0 x 10-7 M
The mathematical product of [H3O+] and [OH-] remains constant in water and dilute aqueous solution at constant temperature.
The ionization constant (Kw) of water is: Kw = [H3O+] [OH-] = 1.0 x M

56. Acidic, Basic, & Neutral IF [H3O+] > [OH-] then solution is acidic.
IF [H3O+] < [OH-] then solution is basic.
IF [H3O+] = [OH-] then solution is neutral.

57. Calculating [H3O+] & [OH-]
Since the product of the hydronium and hydroxide ion concentrations is a constant, we can use the following formula to determine these concentrations.
[H3O+] [OH-] = 1.0 x M

58. Practice Problems
Determine the hydronium and hydroxide ion concentration in a solution that is x10-4 M HCl.

59. Determine the hydronium and hydroxide ion concentration in a solution that is 1.0 x10-3 M HNO3.

60. Determine the hydronium and hydroxide ion concentration in a solution that is 3.0 x10-2 M NaOH.

61. The pH Scale pH- hydrogen power
The pH of a solution is defined as the negative of the common logarithm of the hydronium ion concentration, [H3O+].
pH = -log [H3O+] pH = -log [1 x 10-7] = 7.0

62. The pOH of a solution is defined as the negative of the common logarithm of the hydroxide ion concentration, [OH-].
pOH = -log [OH-] pOH = -log [1x10-7] = 7.0

63. pH & pOH
pH + pOH = 14
14 – pH = pOH
14 – pOH = pH

64. Determine the pH of the following solutions:
a. 1 x 10-3 M HCl
b. 1.0 x 10-5 M HNO3
c. 1 x 10-4 M NaOH
d. 1.0 x 10-2 M KOH

65. Calculating pH
What is the pH of a solution if the [H30+] is 6.7 x 10-4 M? What is the pH of a solution if the [H30+] is 2.5 x 10-2 M? What is the pH of a 2.5 x 10-6 M HNO3 solution? What is the pH of a 2.0 x 10-2 M Sr(OH)2 solution?

66. Calculate Concentration from pH
The pH of a solution is determined to be 5.0. What is the hydronium ion concentration of this solution?
The pH of a solution is determined to be What is the hydronium ion concentration of this solution?

67. Indicator An organic compound that changes color in acid or base
Examples:
litmus - red/blue
phenolphthalein - colorless/pink
red cabbage juice - pink/green
Acid  blue indicator litmus paper turns red in the presence of acid
Base red indicator litmus paper turns blue in the presence of base