1. Acids, Bases & Salts Pre-AP Chemistry LFHS

2. Acid Definitions:
Arrhenius Acid- Any substance which releases H+ (hydrogen ions or protons) in water.
Rxn: HX H2O  H3O X-
(acid) (water) (hydronium ion) (conjugate base)
Bronsted(Lowry) Acid- A proton(H+) donor.
Rxn: HX  H X-
(acid) (Proton) (conjugate base)

3. Write the dissociation reaction for each acid:
Arrhenius Bronsted HCl HCl HNO3 HNO3 HClO4 HClO4 H2CO3 H2CO3 HC2H3O2 HC2H3O2 H3PO4 H3PO4

4. Properties of Acids Acids: 1) Sour Taste 2) Turn litmus RED
3) Electrolytes-Acids release ions in water
4) Corrosive-cause chemical burns
5) Can react with metals to produce H2 gas
6) Acids Bases  Salts H2O
(Neutralization Rxn) (ionic compounds)

5. Strong Acids- 100% dissociation in H20 Weak Acids- less than 5% dissociation in H2O
Dissociation Rxn: HX  H X-
There are only 6 strong acids, all others are weak:
HCl hydrochloric acid (stomach acid AKA muriatic acid)
HBr hydrobromic acid
HI hydroiodic acid
4) HClO4 perchloric acid (strongest of all acids)
5) HNO3 nitric acid (Used to make fertilizers & explosives)
6) H2SO4 sulfuric acid (Most produced chemical Worldwide, Car Battery Acid)

6. Base Definitions
Arrhenius Base- any substance which releases OH- (hydroxide ions) in water.
Reaction: MetalOH  Metal OH-
Bronsted(Lowry) Base- a proton(H+) acceptor.
Reaction: X HOH  HX OH-
This reaction is called hydrolysis of water rxn.

7. Properties of Bases Bases: 1) Bitter Taste 2) Turn litmus BLUE
3) Electrolytes-bases release ions in water
4) Corrosive-cause chemical burns
5) Bases dissolve animal protein(slippery, soap)
6) Acids + Bases  Salts H2O

8. Strong Bases-completely (100%) ionize in water.
There are 8 strong bases(All Arrhenius Bases):
LiOH lithium hydroxide
NaOH sodium hydroxide
KOH potassium hydroxide
RbOH rubidium hydroxide
CsOH cesium hydoxide
Ca(OH)2 calcium hydroxide
Sr(OH)2 strontium hydroxide
Ba(OH)2 barium hydroxide

9. pH Scale

10. pH Calculations
Key equation: pH = -log[H+] pOH = - log[OH-] pH + pOH = 14.0 & [H+]x[OH-] = Kw(1.0 x 10-14)

11. pH calculation
Find the [H+] of a M HCl solution pH
pOH
[OH-]

12. pH calculation
Find the [H+] of a 0.082M NaOH solution pH
pOH
[OH-]

13. 0.0075 mol HNO3 are dissolved in 852 ml of solution. Find pH:

14. pH Calculations Solution pH pOH [H+] [OH-] [H3O+] Acidic/Basic
X 10-5M
X 10-12M
X 10-7M
X 10-11M
X 10-3M
X 10-5M

15. pH Calculations part II
Solution pH pOH [H+] [OH-] [H3O+] Acidic/Basic
X 10-12M
X 10-8M
X 10-1M
X 10-5M
X 10-6M
X 10-11M

16. pH Review
Find the pH if [OH-] = 3.6 x 10-11M:

17. Neutralization Reaction- the rxn between an acid + base  salt + water
Most neutralization rxns are double replacement rxns between arrhenius acid + arrhenius base
HX + MOH  MX HOH
HCl + Mg(OH)2  _____ + _____
H3PO NaOH  _____ + _____
HClO Ca(OH)2  _____ + _____
_______ + ________  Na2CO H2O
HC2H3O2 + Ba(OH)2  _______ + _____

18. Amphoteric- a substance which can act as either an acid(donate H+) or a base(accept H+).
H2O is amphoteric:
It can release a H+: HOH  H OH- (hydroxide ion)
It can accept a H+: HOH H+  H3O+(hydronium ion)
Amphoteric species can also form during the dissociation of a polyprotic acid:
Acid proton Conj. Base
H3PO4 ↔ H H2PO4-
H2PO4- ↔ H HPO42-
HPO ↔ H PO43-

19. Titration- a reaction used to find the conc. of an unknown solution.
If a titration is between an acid and a base:
NaVa = NbVb
N= normailty, N=M x #of equivalents(#H+’s or #OH-’s)
V = volume
Ex: What volume of 0.556M HCl will neutralize 50.0 mL of 0.335M Sr(OH)2?

20. 38. 5 mL of 0. 750M H2SO4 neutralizes 50. 0 mL of NaOH
38.5 mL of 0.750M H2SO4 neutralizes 50.0 mL of NaOH. What is the molarity of NaOH?
20.0 mL of 1.25M KOH neutralizes 25.0 ml H2SO3. What is the molarity of acid?

21. Name___________ pH Review, Pre-AP Chemistry
Solution pH pOH [H+] [OH-] [H3O+] Acidic/Basic
X 10-12M 4
Draw a detailed pH scale
How many ml of 0.25M HCl will neutralize 25.0ml of 0.40M NaOH?
What is the molarity of 325mL of Sr(OH)2 that neutralized 255 mL of M H3PO4