1. ACIDS & BASES

2. Acid Nomenclature Flowchart
Oxyacids or Ternary
-ite
-ate
Binary
-ide

3. NAMES AND FORMULAS A Review
HX means Acid
If anion ends in “–ide”
Acid name begins with “hydro-”
Ends with “–ic” , followed by “Acid”
HCl – Hydrochloric Acid (Chloride)
HBr – Hydrobromic Acid (Bromide)
HCN – Hydrocyanic Acid (Cyanide)

4. NAMES AND FORMULAS If anion ends in “–ite”
Acid ends with “–ous”, followed by “Acid”
H2SO3 – Sulfurous Acid
HNO2 – Nitrous Acid
H3PO3 – Phosphorous Acid

5. NAMES AND FORMULAS If anion ends in “–ate”
Acid ends with “–ic” ,followed by “Acid”
H2SO4 – Sulfuric Acid
HNO3 – Nitric Acid
H3PO4 – Phosphoric Acid

6. NAMES AND FORMULAS Bases named same as ionic compound
NaOH –Sodium Hydroxide (Lye)
Ca(OH)2 – Calcium Hydroxide (Lime)
Pb(OH)2 – Lead Hydroxide
KOH – Potassium Hydroxide

7. WATER IONIZATION Water molecules in continuous random motion
Collisions between two molecules
Result in transfer of hydrogen ion
H2O + H2O H3O+ + OH-
H3O+ = hydronium ion
OH- = hydroxide ion

8. 3 Theories Acid-Base Theories

9. 3 Theories Acid/Base Theory #1: Arrhenius (traditional)
a) Acids – produce H+ ions (or hydronium ions H3O+) in aqueous solution
i: Monoprotic Acid  gives up 1 H+ (HCL)
ii: Diprotic Acid  gives up 2 H+ (H2SO4)
iii: Triprotic Acid  gives up 3 H+ (H3PO4)
b) Bases – produces OH- ions in aqueous solutions

10. Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water

11. Brønsted – Lowry Theory #2: Brønsted – Lowry
a) Acids – proton (H+) donor
(H+ is given away)
b) Bases – proton (H+) acceptor
(H+ gained)
A “proton” is really just a hydrogen atom that has lost it’s electron!

12. A Brønsted-Lowry acid is a proton donor
A Brønsted-Lowry base is a proton acceptor
conjugate acid
conjugate base
base
acid

13. Lewis a) Lewis acid – electron pair acceptor
Theory #3 – Lewis
a) Lewis acid – electron pair acceptor
b) Lewis base – electron pair donor

14. WATER DISSOCIATION, SIMPLIFIED
Dissociation of water:
H2O  H+ + OH-
One H+ and one OH- produced, so
[H+] = [OH-]
[ X ] = concentration (Molarity)

15. PROPERTIES OF ACIDS Sour or tart taste in foods
Strong Acid = Strong Electrolyte
Release H+ ions in water
Turn blue litmus paper Red

16. Hydrogen Ion in Water Water + a proton  Hydronium Ion
H2O H  H3O +1
The H+ ion has no electrons so it attached itself to a water molecule to share its electrons

17. ARRHENEIUS ACIDS
Theory developed by Arrhenius ( )
Defined acids and bases as compounds that ionize to produce H+ and OH-

18. ARRHENIUS ACIDS
Theory: substance that contains hydrogen, and releases the H+ in water
HCl H2O  (1) H3O+ (aq) + Cl - (aq) monoprotic
H2SO4 + H2O  (2) H3O+ (aq) + SO4-2 (aq)
diprotic
H3PO4 + H2O - (3) H3O+ (aq) + PO4-3 (aq)
triprotic

19. Types of Arrhenius Acids
Monoprotic acids contain 1 ionizable proton HCl, HBr, HF, HI
Diprotic acids contain 2 ionizable protons H2SO4
Triprotic acids contain 3 ionizable protons H3PO4

20. PROPERTIES OF BASES Feels slippery Bitter taste
Strong Base = Strong Electrolyte
Produce hydroxide ions in water
Red litmus turns Blue in a Base (RBB)
EX: LYE USED IN SOAPMAKING
AMMONIA USED IN CLEANING

21. ARRHENIUS BASES
Substance that contains OH and releases the OH- in water.
NaOH + H2O  Na+1 (aq) + OH- (aq)
Mg(OH)2 + H2O  Mg +2 (aq) + 2 OH- (aq)

22. Some Definitions Arrhenius acids and bases
Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions (protons, H+).
Base: Substance that, when dissolved in water, increases the concentration of hydroxide ions.

23. Complete book practice problems
Pg 609
#34,43,44,45,46
Or check your Power packet ( Acids + Bases) pg 9

24. Three definitions of acid
Who
Theory:
Acid=
When
Arrhenius
increases H+
1880’s
Brønsted & Lowry
proton donor
1923
Lewis
Electron-pair acceptor

25. ALTERNATE THEORIES
Not all materials with acidic/basic properties in aqueous solution contain H or OH.
Don’t fit Arrhenius definition of acids & base
Johannes Brønsted ( ) and
Thomas Lowry ( ) independently proposed a new definition.

26. Some Definitions Brønsted–Lowry: must have both
1. an Acid: Proton donor
and
2. a Base: Proton acceptor

27. Brønsted – Lowry Acids and Bases
B/L Acid is a hydrogen ion donor
B/L base is a hydrogen ion acceptor
Arrhenius acids and bases fit into the Brønsted – Lowry Theory

28. Brønsted-Lowry acids and bases are always paired.
The Brønsted-Lowry acid donates a proton,
while the Brønsted-Lowry base accepts it.
Which is the acid and which is the base in each of these rxns?

29. Brønsted – Lowry Acids and Bases
NH3 + H2O g NH OH-
Ammonia is a base
accepts hydrogen ion
Water is an acid
donates hydrogen ion

30. What Happens When an Acid Dissolves in Water?
Water acts as a Brønsted–Lowry base and abstracts a proton (H+) from the acid.
As a result, the conjugate base of the acid and a hydronium ion are formed.
Movies…

31. A Brønsted–Lowry acid…
…must have a removable (acidic) proton.
HCl, H2O, H2SO4
A Brønsted–Lowry base…
…must have a pair of nonbonding electrons.
NH3, H2O

32. Conjugate Acids and Bases:
From the Latin word conjugare, meaning “to join together.”
Reactions between acids and bases always yield their conjugate bases and acids.

33. Brønsted – Lowry Acids and Bases
Conjugate Acid
Formed when a base gains a hydrogen ion.
NH4+ is the Conjugate Acid
Conjugate Base
What remains when an acid has donated the hydrogen ion.
OH- is the Conjugate Base

34. Brønsted – Lowry Acids and Bases
Conjugate Acid
Conjugate Base
Base
Acid

35. Brønsted – Lowry Acids and Bases
Conjugate acid / base pair
Two substances that are related by the loss or gain of a hydrogen ion.
HCl + H2O g H3O Cl-
Water is Amphoteric - Acts as both Acid and Base

36. Brønsted – Lowry Acids and Bases
In General:
Conjugate Base of a Strong Acid is weak
HCl (acid) has a weak conjugate base in Cl-
Conjugate Acid of a Strong Base is weak
NaOH (base) has a weak conjugate acid in Na+

37. Remember the Lewis Dot Structure?
ALTERNATE THEORIES
Gilbert Lewis ( ) focused
on the donation or acceptance of electrons.
Lewis acid accepts electrons to form a covalent bond
Lewis base donates electrons to form a covalent bond
Remember the Lewis Dot Structure?
This is the same guy…

38. Acid-Base Definitions
Type
Acid
Base
Arrhenius
H+ producer
OH- producer
Brønsted-Lowry
H+ donor
H+ acceptor
Lewis
Electron-pair acceptor
Electron-pair donor