1. Acids and Bases

2. Acids Sour tastes pH: 0 – 6.9 Reacts with carbonate
to produce CO2 gas.
Turns Litmus from
Blue to Red.
Reacts with metals to
produce hydrogen gas.

3. Acids Acids Solutions conduct electricity (In ion form) Strong (99%)
HCl (aq) + H2O (l) H+ (aq) Cl- (aq) or
H2SO4 (aq) + H2O (l) H+ (aq) + HSO4- (aq)
Weak or strong acids depends on how much the acid dissociates.

4. Bases Bitter Taste pH: 7.1 – 14 Turns Litmus from Red to Blue
Reacts with acids to
form salts.
Slippery feel

5. Bases Weak or Strong depends on how much it dissociates. Weak (4%)
Na2CO3 (aq) + H2O (l) Na+ (aq) + CO3- (aq)
Strong (99%)
NaOH (aq) + H20 (l) Na+ (aq) + OH- (aq)

6. What is an Acid and What is a Base?
Define acid and base in terms of water.
H2O or HOH
H-OH <Molecular Structure
H+ = Hydrogen (Acid)
OH- = Hydroxide (Base)
If you have more hydrogen then hydroxide, you have an acid

7. What is an Acid and What is a Base?
If you have more hydroxide then hydrogen you have a base.
H+ = Acid
OH- = Base
HOH (H2O) = Neutral
We measure acid and Base on the “pH” scale.

8. What is an Acid and What is a Base?

9. pH Scale
The pH scale goes from

10. pH Scale
Acid: pH 0 – 6.9
Base: pH 7.1 – 14
pH of 7 = Neutral pH

11. Common Acids Hydrochloric Acid = HCl Sulfuric Acid = H2SO4
Nitric Acid = HNO3

12. Common Bases Sodium Hydroxide = NaOH Ammonium Hydroxide = NH4OH
Potassium Hydroxide = KOH

13. Types of Acids
Monoprotic acids contain only one acidic hydrogen.

14. Types of Acids Diprotic contains 2 acidic hydrogens
Triprotic contains 3 acidic hydrogens
Polyprotic- more than 1 acidic hydrogen

15. Types of Acid
Most acids are oxyacids, where the acidic proton is attached to an oxygen atom.
HNO3 Nitric Acid
H2SO4 Sulfuric Acid
H3PO4 Phosphoric Acid

16. Types of Acids Amphoteric- can act as an acid or a base.
H2O H2O H3O OH-
Acid (1) Base (1) Acid (2) Base (2)
The above is an autoionization of H2O, and involves the transfer of a proton from one water molecule to another to produce a OH- and H3O+.

17. Buffers and Buffer Solutions
A buffered solution is one that “resists a change is its pH”, when either a hydroxide, OH- or hydrogen, H+, are added.
Blood is a good example of a buffer.
A buffer contains 2-components: an acid to neutralize the addition of OH-, and a base to neutralize the H+ from the addition of an acid.

18. Buffers and Buffer Solutions
When base (OH-) is added to a buffer solution, the acid in the buffer provides H+ ions, which neutralizes the base, thus, preventing a large change in pH.

19. Buffers and Buffer Solutions
The blood’s primary buffer system is made up of carbonic acid (H2CO3) and sodium bicarbonate(NaHCO3).
H HCO H2CO3
From Acid In Buffer Carbonic Acid
OH H2CO HCO H2O
From Base In Buffer Bicarbonate Ion
Buffer is weak base ammonia and its salt, used equation on page 531 to explain the buffer system.

20. Buffers and Buffer Solutions
Original Buffer pH
Added OH- ion replaced
by acid ion or
Added H+ ion replaced
by base ion
Final pH of Buffer
Close to original

21. Acids and Bases
Bases are ionic compounds containing metal cations and the hydroxide ion, OH-.
When a “Base” completely dissociates in water to produce OH-, it is referred to as Alkaline.

22. Bronsted-Lowery Acids and Bases
Bronsted–Lowery Acid is a molecule or ion that is a proton (H+) donor.
Bronsted-Lowery Base is a molecule or ion that is a proton (H+) acceptor.

23. Bronsted-Lowery
Bronsted-Lowery Acid is a molecule that is a Proton Donor.
Example
HCl NH NH Cl-
The proton is transferred from the hydrogen chloride to ammonia.

24. Bronsted-Lowery
Bronsted-Lowery Base is a molecule that is a proton acceptor.
Example
HCl NH NH Cl-
Proton Proton
Donor Acceptor
Acid Base

25. Dissociates / Ionizes
A strong acid is one that ionizes completely in an aqueous solution.
A strong acid is a strong electrolyte.
Electrolyte – Any compound that conducts electricity when melted or dissolved in water.

26. Dissociates / Ionizes
Acids that are weak electrolytes are known as weak acids.
They do not dissociate or ionize very much.
Dissociation- The separation of ions that occurs when an ionic compound dissolves.
Ionization-The process where ions form from a covalent compound.

27. Dissociates / Ionizes

28. Arrhenius Acids and Bases
An Arrhenius Acid is a chemical compound that increases the concentration of hydrogen ions, H+, in an aqueous solution.
Arrhenius Base is a substance that increases the concentration of hydroxide ions, OH-, in an aqueous solution.

29. Conjugated Acid and Bases
When an acid gives up a proton, it can re-accept the proton and acts as a base.
HF H2O F H3O+
Acid Base Conjugated Conjugated
Base Acid
In the above reaction the water molecule is a Bronsted-Lowery Base. The hydronium ion is now able to donate a hydrogen proton, so it is called a conjugated acid.

30. Lewis Acids and Bases A Lewis acid is an electron-pair acceptor.
A Lewis base is an electron-pair donor.
H [ O – H ] H O H
Lewis Acid Lewis Base

31. Graphic organizer time!

32. Neutralization Reaction
The reaction of an acid and base is called a neutralization reaction because the properties of both the acid and base are diminished of neutralized when they react.

33. Concentration of Solution
The concentration of a solution is a measure of the amount of the solute (solid) in a given amount of solvent (Liquid).
Molarity- The number of moles of a solute in one liter of solution.
Molarity, M= Moles/Liter

34. Concentration of Solution
If 3 moles of LiCl are added to 100 L of water, what is the molarity of the solution?
3 mol/100 L = 0.03 M of LiCl

35. Concentration of Solution
If you put 20.0 g of NaOH in 1-liter of water, what is the molarity (M).
20.0g NaOH mole = 0.5 mole
40.0 g NaOH
0.5 mol/1.0 L = 0.5 M of NaOH

36. Concentration of Solution
If you put 50.0 g of HCl in 2.0 liters of water, what is the molarity (M)?
50.0g HCl mole = 1.37 mole
36.46 g HCl
1.37 mol/2.0 L = 0.69 M of HCl

37. Concentration of Solution
When making-up a solution:
M1V1=M2V2
M1 = Initial or Beginning Molarity
V1 = Initial or Beginning Volume
M2 = Final or Ending Molarity
V2 = Final or Ending Volume

38. Concentration of Solution
If you have 300mL of a 0.5 M solution of HNO3. What volume of water needs to be added to get 0.8 M solution of HNO3?
M1 = 0.5 M
V1 = 300 mL
M2 = 0.8 M
V2 = ?
M1V1=M2V2

39. If you have 56 mL of a 3 M solution of H2SO4
If you have 56 mL of a 3 M solution of H2SO4. What volume of water needs to be added to get 0.1 M solution of H2SO4?
M1 = 3 M
V1 = 56 mL
M2 = 0.1 M
V2 = ?

40. If you have 56 mL of a 3 M solution of H2SO4
If you have 56 mL of a 3 M solution of H2SO4. What will the concentration of H2SO4 be if we add 1000mL (1L) of water?
M1 = 3 M
V1 = 56 mL
M2 = ? M
V2 = 1000 mL

41. If you have 5 mL of a 12 M solution of HCl
If you have 5 mL of a 12 M solution of HCl. What will the concentration of HCl be if we add 500mL (1L) of water?
M1 = 12 M
V1 = 5 mL
M2 = ? M
V2 = 500 mL

42. Acid-Base Titration
The general process of determining the molarity of an acid or a base through the use of an acid-base reaction is called an acid-base titration.

43. Acid-Base Titration
The known reactant molarity is used to find the unknown molarity of the other solution.
Solutions of known molarity that are used in this fashion are called standard solutions.
In a titration, the molarity of one of the reactants, acid or base, is known, but the other is unknown.