1. Acids, Bases, and Salts
Chapter 19

2. Chapter 19: Terms to Know
Monoprotic acid Diprotic acid Triprotic acid Conjugate acid Conjugate base Conjugate acid-base pair Amphoteric Lewis acid Lewis base
Hydronium ion Self-ionization Neutral solution Ion-product constant for water Acidic solution Basic solution Alkaline solution pH

3. Introduction
Acids and bases are commonly used inside and outside of the chemistry lab and have distinctive properties.
There are three main theories that explain acid/base properties.
Water can self-ionize to for hydrogen ions and hydroxide ions.
The pH scale is a way to measure the acidity or basicity of a solution.

4. I.) Naming Acids
Treat acids as if they were anions combined with enough hydrogen ions to make a neutral compound.
Acids will have the basic formula HnX, where “n” is the number of hydrogens and “X” is a monatomic or polyatomic ion.
Three rules for dealing with the naming of acids.

5. Naming acids Acids are ionic compounds where hydrogen is the cation.
These are the oxygen
containing acids, or oxo acids.
These are the binary acids

6. Rule #1: Compounds That End in -ide
Acid name begins with prefix hydro-
Drop –ide and add –ic
Add the word “acid” at the end
These compounds are often binary molecular compounds that do not have oxygen as a component.

7. Give the name of the following acid: HCl.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?
Answer: hydrochloric acid

8. Give the name of the following acid: H2S.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?
Answer: K2SO4

9. Rule #2: Compounds That End in –ite
Drop –ite and add –ous.
Add the word “acid” at the end.
The anions of these compounds have oxygen as a component.
All of these are polyatomic acids.
Do not use the prefix “hydro-”.

10. Give the name of the following acid: H2SO3.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?
Answer: sulfurous acid

11. Give the name of the following acid: H3PO3.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?
Answer: phosphorous acid

12. Rule #3: Compounds That End in –ate
Drop –ate and add –ic.
Add the word “acid” at the end.
Again these acids are derived from compounds that have polyatomic anions with oxygen as a component.
Do not use the prefix “hydro-”.

13. Give the name of the following acid: H3PO4.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?
Answer: phosphoric acid

14. Give the name of the following acid: H2SO4.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?
Answer: sulfuric acid

15. II.) Writing Formulas from Acid Names
Simply use the reverse process to obtain the formulas from the names of the acids.
Make sure that you include enough hydrogen ions (H+) to balance the charges of the anions.

16. Give the formula for the following compound: hydrochloric acid.
Is this a binary compound?
How do you know?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?
Answer: HCl

17. Give the formula for the following compound: nitric acid.
Is this a binary compound?
How do you know?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?
Answer: HCl

18. III.) Names and Formulas for Bases
Bases are named in the same way as other ionic compounds – the name of the cation followed by the name of the anion.
The key to identifying bases is to look for the OH- ion.

19. Give the formula for the following compound: potassium hydroxide.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?
Answer: KOH

20. Give the formula for the following compound: Iron(III) hydroxide.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?
Answer: Fe(OH)3

21. Acid-Base Theories (Section 19.1)
Properties of Acids and Bases
Arrhenius Acids and Bases
Bronsted-Lowry Acids and Bases
Lewis Acids and Bases

22. I.) Properties of Acids and Bases
Acids have properties that are more familiar to us.
The properties of bases are less familiar.
Both acids and bases are electrolytes.

23. Properties of acids. Acids have a sour taste.
Acids changes the colors of an acid-base indicator.
Acids can be strong or weak electrolytes.

24. Properties of bases. Most bases taste bitter.
Bases have a slippery feel.
Bases will also change the color of an acid-base indicator.
Bases can also be strong or weak electrolytes.

25. II.) Arrhenius Acids and Bases
Acids are hydrogen containing compounds that ionize to yield hydrogen ions in aqueous solutions.
Bases are compounds that ionize to yield hydroxide ions in aqueous solutions
Svante Arrhenius

26. Arrhenius Acids
Acids are compounds that can yield H+ ions in aqueous solutions.
Monoprotic acids: Acids with 1 ionizable H+
Diprotic acids: Acids with 2 ionizable H+
Triprotic Acids: Acids with 3 ionizable H+
Not all compounds with hydrogen atoms are acids.
Hydrogen atoms must be attached to an electronegative atom.

27. Sample problem #1
Identify each acid as monoprotic, diprotic, or triprotic.
H2CO3
H3PO4
HCl
H2SO4

28. Arrhenius bases.
Bases are compounds that can yield an OH- ion in aqueous solution.
Bases of the Group 1A metals are very strong bases and dissociates completely in aqueous solution.
Bases of other metals do not dissociate completely.

29. Examples of Arrhenius acids and bases.
HCl
KOH
HNO3
NaOH
H2SO4
Ca(OH)2
H3PO4
Mg(OH)2

30. III.) Bronsted-Lowry Acids and Bases
This theory is broader than the Arrhenius theory.
Acids are H+ ion donors
Bases are H+ ion acceptors.
Johannes Bronsted
(1879 – 1947)

31. Conjugate acids and bases
Conjugate acid: A particle formed when a base gains a H+ ion.
Conjugate base: The particle that remains after an acid has donated its H+ ion.
NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq)
Base
Acid
Conjugate
Acid
Conjugate
Base

32. Conjugate Acid-Base Pairs
HCl
Cl-
H2SO4
HSO4-
H3O+
H2O
SO42-
CH3COOH
CH3COO-
OH-
Water is an amphoteric compound because
it can be both an acid and a base.

33. IV.) Lewis Acids and Bases
This theory is the broadest.
Acid = electron pair acceptor
Base = electron pair donor
Gilbert Lewis
(1875 – 1946)

34. Examples of Lewis acid and bases.H+
OH-
H2O
BF3
NH3
AlCl3
Cl-

35. Comparing all three acid/base theories.
Theory
Acid
Base
Arrhenius
H+ producer
OH- producer
Bronsted-Lowry
H+ donor
H+ acceptor
Lewis
Electron-pair acceptor
Electron-pair donor

36. Hydrogen Ions and Acidity (Section 19.2)
Hydrogen Ions from Water
Ion Product Constant for Water
The pH Concept
Measuring pH

37. I.) Hydrogen Ions from Water
Water molecules are highly polar.
Collisions of two water molecules results in the transfer of a H+
This process occurs to a small extent.
The Hydronium Ion

38. II.) Ion Product Constant for Water
Kw = [H+] x [OH-] = 1.0 x 10-14
The H+ and OH- concentration of pure water is 1x10-7 M. This is a neutral solution.
The product of the two concentrations is 1x10-14 M for dilute aqueous solutions.
Adding acids or bases to a neutral solution will change the ion product constant for water.

39. Using ion-product constant to solve for H+ and OH- concentrations.
If [H+] is less than 1.0 x 10-7 M, the solution is basic.
If [H+] is greater than 1.0 x 10-7 M, the solution is acidic.
If we know the ion concentration of either H+ or OH- for a solution we can solve for the other using the ion-product constant.

40. Sample problem
Colas are slightly acidic. If the [H+] in a solution is 1.0 x 10-5 M, is the solution acidic, basic or neutral? What is the [OH-] of this solution?

41. III.) The pH Concept
The pH scale is a less cumbersome way of expressing the [H+].
The scale ranges from 0 – 14.
pH 7 = neutral, pH 0 = very acidic, pH 14 = very basic.

42. pH = -log[H+] Calculating pH.
Calculating the pH of a solution is a very simple process.
The pH of a solution is the negative logarithm of the [H+].
Calculate pH by using the log key on your calculator and using the above formula.

43. Sample problem
What is the pH of a solution with a [H+] of 4.2x10-10M?

44. pOH = -log[OH-] pH + pOH = 14 Calculating pOH.
There is one of two ways that you can solve for the pOH:
pOH = -log[OH-]
pH + pOH = 14

45. IV.) Measuring pH
There are many reasons why we need to know the pH of a solution in the real world and the lab.
There are chemical indicators and instruments to do this.

46. Acids, Bases, And Salts
Chapter 19
The End