1. Acids and Bases

2. Acid Definition: aqueous solution of Hydrogen containing compounds
Name the following:
HCl H2SO4 H2SO3 H2S
Remember:
H with an element: hydro_______ic acid
H with polyatomic ion ending with –ate: _______ic acid
H with polyatomic ion ending with –ite: _______ous acid

3. Acid Definition: aqueous solution of Hydrogen containing compounds
Name the following:
HCl hydrochloric acid
H2SO4 sulfuric acid
H2SO3 sulfurous acid
H2S hydrosulfuric acid

4. Base
Definition (for now): Contains the polyatomic ion OH-1 (hydroxide) Name the following bases: NaOH Ca(OH)2 Cu(OH)2 NH4OH Follow ionic naming rules: name metal, name nonmetal, do NOT use prefixes! If the metal is a transition metal, use roman numeral for its charge

5. Base
Definition (for now): Contains the polyatomic ion OH-1 (hydroxide) Name the following bases: NaOH sodium hydroxide Ca(OH)2 calcium hydroxide Cu(OH)2 copper (II) hydroxide NH4OH ammonium hydroxide

6. Properties of Acids Ionize in water  H3O+1
Corrosive to metals and skin. (React with most metals to form hydrogen gas.)
Taste sour (like lemons)
Frequently feel "sticky"
pH less than 7.
Neutralizes bases producing salt and water.
Electrolytes.

7. Properties of Bases Ionize in water  OH- Feel "slippery".
Taste bitter (like soap)
Electrolytes
pH greater than 7.
Neutralizes acids producing a salt and water.

8. Indicators
Indicators are added to chemicals to determine the pH. They change colors in different pH’s.
You need to memorize the indicators and colors!

9. Acid Base Indicators Type Acid Neutral Base Red Litmus Red Blue
Blue Litmus
Phenolphthalein
Clear
Hot pink
Bromothymol Blue
Yellow
Green

10. Strength vs. Concentration
Concentration: amount of acid or base/amount of water or solution
Strength: how well that particular acid or base ionizes (amount of H3O+1 or OH- )
Strong acid/base: an acid/base that ionizes almost completely
Weak acid/base: an acid/base that only slightly ionizes

11. Play Strength vs. conc. Video

12. Acids and Bases

13. List of Strong and Weak acids
HCl
H2SO4 HF
HC2H3O2
HBr
HClO3
H2S
H2SO3 HI
HClO4
HNO2
H3PO4
HNO3
Organic acids: end in –COOH, weak acid
Ex: vinegar  CH3COOH

14. List of Strong and Weak Bases
Group I and II metals with hydroxides
NH3 and any non-group I or II hydroxide

15. Ionization of water Kw = 1 * 10-14 = [H3O+][OH-]
Pure water ionize slightly according to this equation:
The product of molar concentrations of the ions is equal to a constant Kw. Formula:
Kw = 1 * = [H3O+][OH-]
[ ] means concentration of (molarity)
Important Note: H+ and H3O+ are usually interchangeable (basically they are the same)

16. Relationships
In a neutral solution: In an acidic solution: In a basic solution: Basically this is saying there is more H3O+ in acidic solutions, more OH- in basic solutions. The concentrations of both are the same in neutral solutions

17. pH and pOH Neutral 0 7 14 Acid Base Neutral 0 7 14 Base Acid
pH: measure of [H3O+1] in a solution, measure of “acidity” pOH: measure of [OH-1] in a solution, measure of “basicity”
Neutral
Acid Base
Neutral
Base Acid

18. More on ph
A change in [H+] by a factor of 10 causes the pH to change by 1.
Solution with a pH of 6 has 10x the [H+] as a solution with a pH of 7.
What is the [H+] difference between pH of 1 and pH of 4?
4-1= 3  that’s how many zero’s
Answer= pH 1 has 1000x more

19. Important formulas 1 4 2 5 3 6

20. Play pH/pOH calc. Video

21. Find the pH of the following:
[H3O+] = 1.00 x 10-3M
[H3O+] = 6.59 x 10-10M
[H3O+] = 7.01 x 10-6M

22. Find the [H3O+1]
pH = 3
pH = 6.61
pH = 2.52

23. Find the pH for the following:
pOH = 2
pOH = 1.26
pOH = 4.98

24. Find the pH for the following:
[OH-] = 1.00 x 10-11M
[OH-] = 2.64 x 10-13M
[OH-] = 3.45 x 10-8M

25. [OH-] = 1.00 x 10-6M [OH-] = 4.97 x 10-10M [OH-] = 2.93 x 10-2M
Find the [H3O+1]
[OH-] = 1.00 x 10-6M
[OH-] = 4.97 x 10-10M
[OH-] = 2.93 x 10-2M

26. Find the ph
0.054M HCl
0.178M NaOH

27. Types of Acids and Bases
Theory
Acid Definition
Base Definition
Arrhenius
Releases H+1 into solution
Releases OH-1 into solution
Bronsted-Lowery
Proton (H+1) donor
Proton (H+1) acceptor

28. What happens when you mix an Arrhenius acid with an Arrhenius base?
Neutralization, producing a salt and water Generic Equation: Salt: Ionic compound formed from the cation of a base and the anion of an acid

29. Name the salt produced and write the balanced reaction:
Sodium hydroxide and hydrochloric acid
Calcium hydroxide and sulfuric acid
Potassium hydroxide and nitric acid
Remember: these are double replacement reactions! You will switch the anions of the reactants.
Don’t forget to balance charges when making the products! The subscripts might change! That’s okay! 

30. Name the salt produced and write the balanced reaction:
Sodium hydroxide and hydrochloric acid NaOH + HCl  NaCl + H2O
Calcium hydroxide and sulfuric acid Ca(OH)2 + H2SO4  CaSO4 + 2H2O
Potassium hydroxide and nitric acid
KOH + HNO3  KNO3 + H2O

31. Review Acids and Bases
Watch this video by clicking the title

32. Quiz Topics Acid/Base Properties Acid/Base Definitions
Strong vs. Weak Acids and Bases (memorize them!)
Neutralization Reactions
pH/pOH Calculations

33. Definitions
Monoprotic acid: only has one ionizable hydrogen ex: HCl, HBr, HC2H3O2, HNO3
Polyprotic acid: more than one ionizable hydrogen ex: H2SO4, H3PO4
Amphoteric: substance that can act as an acid or as a base ex: H2O, NH3

34. Titrations
An acid-base titration is a neutralization reaction that is performed in the lab in order to determine an unknown concentration of acid or base.
Remember this: MAVA= MBVB
M  molarity (M)
V  volume (V)

35. Titrations
Endpoint: When the chosen indicator changes color and you stop the titration.
Equivalence point: When the solution is completely neutralized. The reaction is complete. [H+] = [OH-]

36. Titration terms
Indicator: weak acid or base and its conjugate ion; whose color changes in different pH’s
Standard solution: solution of known concentration used as the titrant
Carolina Biological Video

37. Play Titration Calculations Video

38. Titrations
1) If it takes 54mL of 0.1M NaOH to neutralize 125mL of an HCl solution, what is the concentration of the HCl?
2) If it takes 25mL of 0.05M HCl to neutralize 345mL of NaOH solution, what is the concentration of NaOH solution?

39. Play Titration Curve Video

40. Titration Curves
On the following slide you you will see 3 different curves.
The relationships are:
Strong Acid titrated with Strong Base
Weak Acid titrated with Strong Base
Strong Acid titrated with Weak Base
Using those graphs compare the pH values of each substance as well as the equivalence points

41. More Titration Curves Strong acid and weak base curve
Strong base and weak acid curve
Strong acid and strong base curve