1. Acids and Bases

2. Properties of Acids (in aq solution)
Sour taste
Low pH
Turn litmus paper red
Conduct electrical current

3. Properties of Bases (in aq solution)
Bitter taste
Slippery
High pH
Turn litmus paper blue
Conduct electrical current

4. Acid = substance that releases H+ ions in aq solution HCl  H+ + Cl-
Arrhenius Definition
Acid = substance that releases H+ ions in aq solution
HCl  H+ + Cl-
Base = substance that releases OH- ions in aq solution
NaOH  Na+ + OH-

5. Acid-Base Reactions
Known as a neutralization reaction. Acids and bases will react with each other to form salt and water.
HCl + NaOH  NaCl + H2O

6. Bronsted-Lowry Definition
As more and more substances were determined to have acidic or basic properties, even some without obvious H+ or OH-, a new definition was needed.
Acid = proton donor
Base = proton acceptor

7. Bronsted-Lowry Definition
Acid = proton donor
H2O + HCl  H3O+ + Cl-

8. Bronsted-Lowry Definition
Base = proton acceptor
NH3 + H2O  NH4+ + OH–

9. Lewis Acid – something that accepts an electron pair to form a covalent bond
Lewis Base – something that donates an electron pair to form a covalent bond
A + :B → A—B

10. Acids & Bases Review Acid Base
substance that releases H+ ions in aq solution
Proton donor
Electron pair acceptor
Base
substance that releases OH- ions in aq solution
Proton acceptor
Electron pair donator

11. Conjugate Acid-Base Pairs
In an acid-base reaction, and acid plus a base reacts to form a conjugate base plus a conjugate acid
Acid + Base  Conjugate Base + Conjugate Acid
The conjugate acid of a base is formed when the base gains a proton. A conjugate base is formed when an acid loses a proton.

12. NH3 + H20  NH4+ + OH-
Additional Proton means it is now a Proton Donor = Conjugate Acid
Loss of proton means it is now a Proton Acceptor = Conjugate Base
Proton Acceptor = Base
Proton Donor = Acid
Note:
The conjugate name only refers to acids and bases in the PRODUCTS
Conjugate pairs differ only by a proton
NH3 and NH4+ are a conjugate acid-base pair
H20 and OH- are a conjugate acid-base pair
A strong acid becomes a weak conj. base (and vice versa)

13. Acid & Base Naming Bases are named exactly the same
Ex. Ca(OH)2 is Calcium hydroxide

14. Acid Naming Overview Binary Start with hydro- Element
End with –ic acid
Tertiary (Oxyacids)
“I ate something, and now I am sick”
If anion ends in –ate then the acid ends in –ic
If the anion ends in –ite then the acid ends in -ous

15. Naming WS

16. Acid Strength
A stronger acid will transfer MORE protons (H+) than a weak acid. It will create more hydronium ions (H3O+) in water.
Hydrochloric acid
HCl + H2O  H3O+ + Cl-
Acetic Acid
CH3COOH + H2O  H3O+ + CH3COO-
More dissociation!
Less dissociation!

17. How do we compare the strength of an acid or a base?
We measure the amount of hydronium ions they create (acids) or the amount of hydroxide ions they create (bases)….using concentration.

18. When water gains a proton it is called HYDRONIUM!!
H3O+

19. When water loses a proton it is called HYDROXIDE!!
OH-

20. What is concentration?
Using molarity, it is a measure of moles of solute in liters of solution.
Concentration is measured in WATER!

21. H2O is both an acid and a base
Water is simultaneously donating and accepting protons!

22. What are the ion concentrations in water?
The concentrations of H3O+ and OH- in pure water are each 1.0×10-7 mol/L at 25ºC.
Putting a symbol in brackets is used to signify the concentration.
[H30+] = 1.0×10-7 M
[OH-] = 1.0×10-7 M

23. Ionization Constant of water, KW
KW = [H30+] [OH-]
KW = (1.0×10-7)(1.0×10-7) = 1.0×10-14

24. Bases increase the [OH-]
Acids increase the [H30+] Whenever [H30+] is greater than [OH-], the solution is acidic.
Bases increase the [OH-]
Whenever [OH-] is greater than [H30+], the solution is basic.
With an increase in [H30+], some of the H30+ ions will react with the OH- ions, reducing [OH-] . [H30+][OH-] will still = 1.0x10-14

25. Concentration values tend to be small…so we use a more convenient scale. pH!

27. pH + pOH = 14
pH – A measure of the acidity of a solution.
It is the negative logarithm of the hydronium ion [H30+] concentration.
pH = -log [H30+]

28. pH + pOH = 14
pOH – A measure of how basic a solution is.
It is the negative logarithm of the hydroxide [OH-] concentration.
pOH = -log [OH-]

29. The logarithm scale is created to make numbers over a large range more manageable.

30. The logarithm base 10 of a number x is the power to which 10 must be raised in order to equal x.
Log 10 x = ? Log 100 = ?
10? = x 10 ? = 100

31. Remember, our concentrations are SMALL
Remember, our concentrations are SMALL. So we are going to be dealing with decimals…
Log 10 x = ? Log .001 = ?
10? = x 10 ? = .001

32. [H+] = 1×10-3 = 0.001
pH = -log [H+]
pH = -log (1×10-3)
pH = 3
To determine pH from a concentration where 1 is the only digit, write the concentration in scientific notation. The absolute power of the exponent will be the pH.

33. For a base, you do the same thing except remember that you are solving for pOH first…

34. Ionization Constant of water, KW
KW = [H30+] [OH-]
KW = (1.0×10-7)(1.0×10-7) = 1.0×10-14

35. 11 3.0 2.0 12 8 6 10.8 3.22 13 .70 2.22 11.8 Solutions [H+] pH [OH-]
pOH
1.0×10-3M HClO4
0.010 M HCl
M KOH
6.00×10-4 HBr
0.20 M NaOH
H2SO4 11
3.0
1.0×10-3M
1.0×10-11M
2.0 12
1.0×10-2M
1.0×10-12M 8 6
1×10-8M
1×10-6M
10.8
3.22
6.00×10-4M
1.67×10-11M 13
.70
5.0×10-14M
2.0×10-1M
2.22
11.8
6.00×10-3M
1.67×10-12M

36. [H30+] [OH-] = 1.0×10-14 M pH + pOH = 14 pH = -log [H30+]
Equations to Know!!
[H30+] [OH-] = 1.0×10-14 M
pH + pOH = 14
pH = -log [H30+]
pOH = -log [OH-]
[H30+] = 10-pH
[OH-] = 10-pOH

38. Green Workbook
Pg. 262 #2
Pg. 264 #1
Pg. 267 #3
Pg. 269 #1 & #2
Pg. 270 #7