1. Acids and Bases

2. Arrhenius Theory Acids produce H+ ions. Bases produce OH- ions.
HCl g H+ + Cl-
NaOH g Na+ + OH-
Applies only to water solutions

3. Strong acids HCl (stomach acid) H2SO4 (battery acid)
HNO3 (nitric acid)
Weak acids
H2CO3 (carbonic acid)
HC2H3O2 (acetic acid)
Formic acid- wasp stings

4. Strong bases
KOH
NaOH
Weak bases
NH4OH
Mg(OH)2 (milk of magnesia)

5. Bronsted-Lowry Theory
Acids donate protons
Bases accepts protons
NH3(g) + H2O(l) g NH4+(aq) + OH-(aq)
conjugate acid
conjugate base
base
acid

6. Conjugate acids and bases
A conjugate acid is formed when a base gains an H+ ion.
A conjugate base is formed when an acid loses an H+ ion.
HCl(g) + H2O(l) g H3O+(aq) + Cl-(aq)
acid base
H3O+(aq) + Cl-(aq) g HCl(g) + H2O(l)
acid base
Acid + base g conjugate base + conjugate acid
conjugate acid
conjugate base
H+ is a proton.
Conjugate acid of a base is formed when the base acquires a proton.
Conjugate base of an acid forms when a proton is released from an acid.
conjugate acid
conjugate base

7. Acid conjugate base
HCl Cl-
H2SO4 HSO4-
H3O+ H2O
Base conjugate acid
NH3 NH4+
H2O H3O+

8. Monoprotic- has 1 H; HCl
Diprotic- has two H; H2SO4
Triprotic- has three H; H3PO4

9. Characteristics of acids
Taste sour
pH from
Has H+ at the beginning of the formula
Produce H2h when reacting with most metals
Neutralize bases
Conducts electricity (electrolytes)
Turns litmus paper red

10. Characteristics of bases
Taste bitter
pH between
Have OH- ion
Feels slippery
Neutralize acids
Turns litmus paper blue

11. Naming acids anion acid name example
-ide Hydro- ic HCl hydrochloric acid
-ite ous HNO2 nitrous acid
-ate -ic HNO3 nitric acid

12. Try these H2SO4 HF H3PO4 H2SO3 sulfuric acid hydrofluoric acid
phosphoric acid
sulfurous acid

14. 1 l l l l l 7 l l l l l l14 acid neutral base
pH scale
1 l l l l l 7 l l l l l l14
acid neutral base

15. Ionization of water
H2O(l) H+(aq) + OH-(aq)

16. [H+] means hydrogen ion concentration in moles per liter (molarity).
Water at 25◦C : [H+] = 10-7moles/L
[OH-] = 10-7moles/L
Since [H+] = [OH-], water is neutral

17. [H+] ∙ [OH-] = mole2/L2
Example: Find the [OH-] in a solution in which [H+] = 10-5.
[H+] ∙ [OH-] = mole2/L2
[OH-] = 10-9
If the concentration of either ion is known, the concentration of the other can be determined.

19. [H+] = 10-pH [OH-] = 10-pOH
pH + pOH = 14.0
Sample problem:
A 0.01 M sample of NaOH completely ionizes. What is its pH, pOH, [H+], and [OH-] ?
[OH-] = 0.01 mole/L = pOH = 2
pH = 14 – pOH = [H+] = 10-12

20. Sample Problem 2:
A solution has a pH of 3. What is its pOH, [H+], and [OH-]?
pOH = 14 – 3 = 11
[OH-] = 10-11
[H+] = = 10-3
10-11

21. pH values of common liquids
Human gastric juices 1-3
Lemon juice
Vinegar
Soda 2-4
O.J. 3-4
Coffee, black 4
Milk 6.5
Blood
Sea water
Ammonia
1M NaOH 14.0

22. Neutralization reactions
Always form a salt and water
Salt- a crystalline compound formed from an acid’s anion and a base’s cation.

23. Titration
An unknown concentration of acid or base can be determined by measuring the amount of a known acid or base that will neutralize the other.
An indicator changes color when the “endpoint”, or neutralization occurs.

24. Titration Standard solution- one whose concentration is known
Endpoint- the point at which equivalent amounts of reactants are present.
M∙V = moles
MaVa=MbVb
The standard solution is dropped from a buret into a measured amount of unknown solution.

25. If 15. 0ml of 0. 500M NaOH is used to neutralize 25
If 15.0ml of 0.500M NaOH is used to neutralize 25.0ml HCl, what is the concentration of the acid?
NaOH + HCl g H2O + NaCl
15mL x 0.500M = 25.0 ml x Ma
= 0.300M HCl

26. Buffers Can absorb acids and bases without changing its pH
A weak acid (HA) with its salt (NaA)
A weak base (MOH) with its salt (MA)
They contain ions that will react with H+ (a base) and OH- ions (an acid).

27. HF(aq) D H+(aq) + F-(aq)
Buffered solution is mostly HF and F-.
If H+ is added: H+ + F- g HF
If OH- is added: OH- + HF g F- + H2O