1. 5/8 Bell Work
Boiling water is poured into a thick-walled drinking glass and a very thin-walled tea cup.
Which is more likely to crack? Why?
(Hint: Heat = expansion)
Drinking glass, thick walls do not transmit heat easily so inside and outside are at different temps.

2. 5/8 Schedule Finish “Gas Laws” test?
Notes Ch 19.1 “Acid-Base Theories” in Acids and Bases unit
SR 19.1

3. Unit: Acids and Bases
Ch 19
Antacid + Acid = Fun!!

4. 19.1
Acid-Base Theories
Bracken Cave, near San Antonio, Texas, is home to million bats. Visitors to the cave must protect themselves from the dangerous levels of ammonia. It is a byproduct of the bats’ urine.
You will learn why ammonia is considered a base.

5. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Acids
Acids taste sour, will change the color of an acid-base indicator, and can be strong or weak electrolytes in aqueous solution.
Citrus fruits contain citric acid. Tea contains tannic acid.

6. Properties of Acids and Bases
19.1
Properties of Acids and Bases
Bases
Bases taste bitter, feel slippery, will change the color of an acid-base indicator, and can be strong or weak electrolytes in aqueous solution.
Antacids use bases to neutralize excess stomach acid. The base calcium hydroxide is a component of mortar.

7. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
Arrhenius Acids and Bases
Acids are hydrogen-containing compounds that ionize to yield hydrogen ions (H+) in aqueous solution.
Bases are compounds that ionize to yield hydroxide ions (OH–) in aqueous solution.

8. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
Hydrochloric Acid
Hydrochloric acid is actually an aqueous solution of hydrogen chloride. Hydrogen chloride forms hydronium ions, making this compound an acid.

9. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
Arrhenius Acids
Acids with one ionizable hydrogen, like nitric acid (HNO3), are monoprotic acids.
Acids with two ionizable hydrogens, such as sulfuric acid (H2SO4), are diprotic acids.
Acids with three ionizable hydrogens, such as phosphoric acid (H3PO4) are called triprotic acids.

10. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases

11. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
Arrhenius Bases
Hydroxide ions are one of the products of the dissolution of an alkali metal in water.

12. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases

13. Arrhenius Acids and Bases
19.1
Arrhenius Acids and Bases
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. Brønsted-Lowry Acids and Bases
19.1
Brønsted-Lowry Acids and Bases
Brønsted-Lowry Acids and Bases
Defines an acid as a hydrogen-ion donor, and a base as a hydrogen-ion acceptor.

15. Brønsted-Lowry Acids and Bases
19.1
Brønsted-Lowry Acids and Bases
Why Ammonia is a Base
Ammonia dissolves in water to form ammonium ions and hydroxide ions. In this reaction, the water molecule donates a hydrogen ion to the ammonia molecule. Explaining
Why is ammonia not classified as an Arrhenius base?

16. CaCO3 + CH3COOH → Ca(CH3COO)2 + CO2 + H2O
Antacid Rockets
These “rockets” are powered by mixing an acid and a base.
Balance the equation below.
CaCO3 + CH3COOH → Ca(CH3COO)2 + CO2 + H2O
Goal is to get cap to pop off as quickly and as high as possible.
Change temperature, concentration, or surface area one at a time.
Use a water bath to warm/cool vinegar NOT directly.
Wipe up mess and rinse materials down sink.

17. Brønsted-Lowry Acids and Bases
19.1
Brønsted-Lowry Acids and Bases
Conjugate Acids and Bases
A conjugate acid is the particle formed when a base gains a hydrogen ion.
A conjugate base is the particle that remains when an acid has donated a hydrogen ion.

18. Brønsted-Lowry Acids and Bases
19.1
Brønsted-Lowry Acids and Bases
A conjugate acid-base pair consists of two substances related by the loss or gain of a single hydrogen ion.
A substance that can act as both an acid and a base is said to be amphoteric.

19. Brønsted-Lowry Acids and Bases
19.1
Brønsted-Lowry Acids and Bases
Reactive acids: test tubes with 5-10 mL of 1 M HCl and pieces of Zn and Mg.

20. Brønsted-Lowry Acids and Bases
19.1
Brønsted-Lowry Acids and Bases
A water molecule that gains a hydrogen ion becomes a positively charged hydronium ion (H3O+).
When sulfuric acid dissolves in water, it forms hydronium ions and hydrogen sulfate ions. Identify which ion is the conjugate acid and which he the conjugate base?

21. Lewis Acids and Bases Lewis Acids and Bases
19.1
Lewis Acids and Bases
Lewis Acids and Bases
Acid accepts a pair of electrons during a reaction, while a base donates a pair of electrons.
Lewis acid accepts a pair of electrons to form a covalent bond.
A Lewis base donates a pair of electrons to form a covalent bond.

22. 19.1
Lewis Acids and Bases

25. for Conceptual Problem 19.1

26. 19.1 Section Quiz.
1. Which of the following is NOT a characteristic of acids?
taste sour
are electrolytes
feel slippery
affect the color of indicators C

27. 19.1 Section Quiz.
2. Which compound is most likely to act as an Arrhenius acid?
H2O
NH3.
NaOH.
H2SO4. D

28. 19.1 Section Quiz. 3. A Lewis acid is any substance that can accept
a hydronium ion.
a proton.
hydrogen.
a pair of electrons. D

29. Stop Notes Here!

30. 5/9 Bell Work
How high would you have to count to use the letter “A” in the proper English spelling of a whole number?
1,000

31. 5/13 Bell Work
What is the difference between a lacto-ovo vegetarian and a vegan?

32. Hydrogen Ions and Acidity
19.2
Hydrogen Ions and Acidity
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.

33. Hydrogen Ions from Water
19.2
Hydrogen Ions from Water
Hydrogen Ions from Water
The reaction in which water molecules produce ions is called the self-ionization of water.

34. Hydrogen Ions from Water
19.2
Hydrogen Ions from Water
In the self-ionization of water, a proton (hydrogen ion) transfers from one water molecule to another water molecule.
The self-ionization of water. A proton (hydrogen ion) transfers from one water molecule to another water molecule. The result is one hydronium ion (H3O+) and one hydroxide ion (OH-).

35. Ion Product Constant for Water
19.2
Ion Product Constant for Water
For aqueous solutions, hydrogen-ion concentration times the hydroxide-ion concentration equals 1.0 
Any aqueous solution in which [H+] and [OH-] are equal is described as a neutral solution.

36. 19.2
Measuring pH
Acid-Base Indicators

37. Measuring pH 19.2 Universal Indicators
You can find acidic and basic substances in your home. a) Universal indicator solution has been added to solutions of known pH in the range from 1 to 12 to produce a set of reference colors. b) Universal indicator has been added to samples of vinegar, soda water, and ammonia solution. Interpreting Photographs Use the reference colors to assign pH values to vinegar, soda water, and ammonia solution.

38. 19.2
Measuring pH
pH Meters
A pH meter provides a quick and accurate way to measure the pH of a solution. a) Water is neutral, having a pH of 7. b) The pH of vinegar, a dilute aqueous solution of ethanoic (acetic) acid, is about 3. c) The pH of milk of magnesia, an aqueous suspension of magnesium hydroxide, is Applying Concepts What are some advantages of using a pH meter rather than an indicator?

39. Measuring pH
Use the yellow pH paper to determine the pH of the products.
Determine if they are acids or bases.
Test the products again using the red and blue litmus paper
What do acids and bases do to the red litmus?
What do acids and bases do to the blue litmus?

40. 5/14 Bell Work
As a rule, how long will an “Eight Day Clock” run without winding?

41. Ion Product Constant for Water
19.2
Ion Product Constant for Water
The product of the concentrations of the hydrogen ions and hydroxide ions in water is called the ion-product constant for water (Kw).

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

43. 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?

44. 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.

45. 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?

46. 19.1

47. 19.1

48. for Sample Problem 19.1

49. 19.2
The pH Concept
The pH of a solution is the negative logarithm of the hydrogen-ion concentration.

50. 19.2
The pH Concept
Calculating pH

51. 19.2
The pH Concept
A solution in which [H+] is greater than 1  10–7 M has a pH less than 7.0 and is acidic. The pH of pure water or a neutral aqueous solution is 7.0. A solution with a pH greater than 7 is basic and has a [H+] of less than 1  10–7 M.

52. 19.2
The pH Concept
The hydrogen-ion concentrate of a solution is used to classify the solution as acidic, neutral, or basic. INTERPRETING GRAPHS a. Identify What is [H3O+] in a neutral solution? b. Describe How does [H3O+] compare with [OH-] in an acidic solution? c. Compare and Contrast In terms of ion concentrations, how are basic solutions different from acidic solutions?

53. 19.2
The pH Concept

54. 19.2
The pH Concept
Calculating pOH

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

56. 19.2

57. 19.2

58. for Sample Problem 19.2

59. 19.3

60. 19.3

61. 19.3

62. 19.3