1. Acids & Bases

2. Acid/Base Theory
Acids and bases are solutions which can be described differently by multiple theories.
So far, we have treated everything that utilizes
“H” as a cation = ___________________
H3PO4
“OH” as an anion = _________________
NaOH

3. Arrhenius Theory
The theory that anything capable of producing ________ ions are acids and those producing ________ anions are bases is Arrhenius’ Theory of acids/bases.
Based on the notion that these substances _______________ in solution into their ions.
H2SO4
H20

4. Acid or Base?
HNO3 KOH
Ca(OH)2 HBr
HC2H3O2 Al(OH)3

5. Bronstad Lowry Acids/Bases
More general description of acids and bases, incorporates all Arrhenius acid/bases
Acids = ___________________________________
Bases = ___________________________________
Example:
NH3 (aq) + H2O (l)
Would solutions of NH3 be acidic or basic?

6. Conjugate Acids/Bases
NH3 (aq) + H2O (l) NH4+ (aq) + OH-(aq)
____________________: The compound remaining after H+ acceptance by a base.
NH NH4+
Base Conjugate Acid
____________________: The compound remaining after H+ donation by an acid.
H2O OH-
Acid Conjugate Base

7. Lewis Acid/Bases Describes Acid/Bases based upon electron donation.
Lewis Acid: A substance that can _____________ a pair of electrons to form a covalent bond.
Lewis Base: A substance that can _____________ a pair of electrons to form a covalent bond.
H + + OH - H2O

8. Strength of Acids/Bases
For this class, we will mostly discuss Arrhenius acid/bases (H+ cation/OH- anion)
The strength of these solutions is determined by the ___________________ of H+ or OH- ions in the solution.
Dependent upon… 1) 2)

9. Concentration of solute
Just like calculating the molarity of non acid/base solutions.
M =
Example: What is the concentration of a H2SO4
solution if 13.2 g of solute are dissolved in 100mL of
di-water?

10. Calculating [H+ ] & [OH-]
However, we cannot assume the molarity (concentration) of H+ /OH- ions is the same as the molarity of the solution for 2 reasons:
Not all

11. Dissociation
Complete dissociation: all solute dissociates into ions, meaning the concentration of ions can be calculated with the __________ _____________.
HCl H+ + Cl-
1 mol HCl produces 1 mol H+
So a 0.2M HCl solution would have a H+ concentration of ______________

12. Complete Dissociation
Few acids/bases completely dissociate
If they do, they are termed “____________ _______________” because they produce high concentrations of their ions upon dissociation.
Strong Acids (7):
Strong Bases (8):

13. Calculating ion donation
Not all acids/bases donate 1 H+ or OH- into solution when they dissociate!
How many ions would the following acids/bases donate if they completely dissociate?
HBr
Ca(OH)2
H2SO4

14. [H+] Example
Using the previous H2SO4 example (13.2 g of solute are dissolved in 100mL of di-water), calculate the [H3O+] of the solution.

15. Partial Dissociation
Weak acids/bases do not completely dissociate in water. They are called weak, because a ____________ concentration of H+ or OH- ions results.
Example: Only about 1% of Phosphoric Acid (H3PO4) dissociates into H+ + H2PO4.

16. Dissociation of Strong & Weak Acids/bases
In other words, you would need to know what _____________________ of an acidic/basic compound is likely to donate its ions into solution in order to calculate the [H+ ] & [OH-].
For this class, we will be working with strong acids/bases. So complete _______________________ (ion donation) can be assumed.

17. Potential of Hydrogen pH = _______________________________
pH is an expression of the concentration of _____________ in solution. Since H+ readily reacts with water to form H3O+, we calculate…
pH = −log [H3O+]
[H3O+] = 10-pH

18. pH & POH
Just as pH is an expression of the concentration of H+ ions in solution, pOH expresses the concentration of OH- ions in solution…
pOH = −log [OH-]
[OH-] = 10-pOH
pH & pOH always add up to 14 and thus are related through the equation:
pH + pOH = 14

19. pH Scale pH < 7 pH = 7 pH > 7 High [H3O+] Low [H3O+]
[H3O+] = ~1x10-7

20. Acid/Base Reactions
Also known as ____________________ reactions, because the pH of the final solution becomes neutralized towards pH=7
Either [H3O+] or [OH-] is __________________by forming more neutral products.
Acid + Base Salt + Water

21. 2) Acid + Carbonate Salt + H2O + CO2
Acid/base reactions
2 Types you will need to know…
1) Acid + Base Salt + H2O
2) Acid + Carbonate Salt + H2O + CO2

22. Acid/base reaction #1
Example: Hydrochloric acid reacts with sodium hydroxide.

23. Acid/Base Reaction #2
Example: Potassium carbonate reacts with sulfuric acid.