1. Review of Acids, Bases, & Salts

2. Has H in the formula Produces H+ as the only positive ion in solution
Arrhenius Acid

3. Inorganic – formula starts with H Organic – formula ends with COOH
Formula of an Acid

4. Properties of Acids Sour Taste Electrolytes
React with bases to form a salt + H2O
Turn litmus RED
React with most metals to produce H2(g)
Properties of Acids

5. HCl  H+ + Cl- or
HCl + H2O  H3O+ + Cl-
Ionization of an Acid

6. Arrhenius Base Has OH in the formula
Produces OH- as the only negative ion in solution
Arrhenius Base

7. Has format MOH M is a metal
Formula of a Base

8. Properties of Bases Bitter Taste Slippery Feel Electrolytes
React with acids to form a salt + H2O
Turn litmus BLUE
Properties of Bases

9. NaOH  Na+ + OH-
Ionization of a Base

10. NH3 + H2O  NH4+ + OH-
Ionization of NH3

11. Metal + Nonmetal
Formula of a Salt

12. Write the formula of potasium sulfate
K+ & (SO4)2-
K2SO4
Write the formula of potasium sulfate

13. Electrolytes Solutions conduct – they contain ions
Acids (HX), bases (MOH), & salts (MX) are electrolytes
Electrolytes

14. Solutions of covalent compounds (all nonmetals). They do NOT conduct.
NONelectrolytes

15. Identify the electrolytes
Yes - B
Yes - B
LiOH
CH3COOH
C6H12O6
NaNO3
H2SO4
CH3OH
Ca(OH)2
HCl
C8H18
Al(OH)3
HNO3
CH3CH2COOH
K2SO4
CH3CHOHCH3
CH3OCH3
H3PO4
Mg(OH)2
CH3CH2OH
Yes - A
Yes - A
Yes - A No
Yes - S
Yes - S
Yes - A No No No
Yes - A
Yes - B
Yes - A
Yes - B No No

16. 0-14 Acidic: 0 to 7, Neutral: 7 Basic: 7-14
pH scale

17. pH = 0
Most acidic on pH scale

18. pH = 14
Most basic on pH scale

19. Hydroxide ion
OH-

20. Hydrogen ion H+

21. Hydronium ion. Interchangeable with H+.
H3O+

22. [H+]  [OH-]
Acidic Solution

23. [OH-]  [H+]
Basic Solution

24. If the pH changes from 3 to 5, how does the [H+] change?
The pH changes by 2, so the [H+] changes by 102 or 100X. Since the pH went up, it became LESS acidic.
The new solution has a [H+] 100 times less than the original solution.
If the pH changes from 3 to 5, how does the [H+] change?

25. How can pH be safely tested?
Instrumental – use pH meter
Indicators – use a series of indicators to narrow down the pH range
Test acids with metals (NOT Cu, Ag, or Au)
How can pH be safely tested?

26. Proton Donor
Bronsted-Lowry Acid

27. Proton Acceptor
Bronsted-Lowry Base

28. Bronsted-Lowry Acids & Bases
HCl + H2O  H3O+ + Cl-
Bronsted-Lowry Acids & Bases

29. Complete or almost complete ionization.
Strong Acids & Bases

30. Ionization occurs only to a slight extent.
Weak Acids & Bases

31. Reactions of Acids with Metals
Metal + Acid  H2(g) + salt
Reactions of Acids with Metals

32. Zn(s) + 2HCl  H2(g) + ZnCl2
Zn(s) + HCl  ?

33. 2Al(s) + 6HCl  3H2(g) + 2AlCl3
Al(s) + HCl  ?

34. Neutralization Reactions
Acid + Base  Salt + H2O
Neutralization Reactions

35. Net Ionic Equation for Neutralization Reactions
H+ + OH-  H2O
Net Ionic Equation for Neutralization Reactions

36. Moles H+ = Moles OH-
At neutralization

37. Molarity = Moles solute
Liters of soln
Molarity (M)

38. MaVa = MbVb
Titration Equation

39. -log[H+] or –log[H3O+] pH

40. -log[OH-]
pOH

41. 14
pOH + pH =

42. The pH = The pOH = The [OH-] =3 11
1 X 10-11
If the [H+] = 1 X 10-3

43. Substance that changes color over a narrow pH range.
Indicator

44. Molarity H2SO4 Vs. Molarity H+
H2SO4  2H+ + SO42-
[H+] = 2[H2SO4]
2M H2SO4  4M H+
Molarity H2SO4 Vs. Molarity H+

45. MaVa = MbVb X(20.0 mls) = .250M(50.0mls)
What is the concentration of a hydrochloric acid solution if 50.0 mL of a M KOH solution are needed to neutralize 20.0 mL of the HCl solution of unknown concentration?

46. (1.50 M)(10.62 mls) = X(20.20 mls) Acid 1.50 M Base ? M Final Volume
16.07
24.25
Initial Volume
5.45
4.05
Amount Used
10.62
20.20
(1.50 M)(10.62 mls) = X(20.20 mls)