1. Acids & Bases

2. Acids Naming Acids Properties of Acids: Sour Taste Electrolytes
Change indicator colors
React with metals to form hydrogen
React with carbonates to form carbon dioxide
React with bases to form salt & water
Produces H+ in water
Naming Acids
Look at ending
-ate polyatomic ions -ic acids
example:
-ite polyatomic ions  -ous acids
-ide monatomic ions hydro –ic acid

3. Bases Naming Bases Bitter Feel Slippery Electrolytes
Properties of bases:
Bitter
Feel Slippery
Electrolytes
Change indicator colors
React with acids to produce salt & water
Produce OH- in water
Naming Bases
name the metal and hydroxide

4. Water Self ionization of water: H2O + H2O  H3O+ + OH-
Hydronium ion H3O+
Hydroxide ion OH-
Only 1X 10 –14 M of water molecules do this so [H3O+][OH-] = 1X 10 –14 M
If [H3O+]=[OH-] neutral solution
If [H3O+]>[OH-] acidic solution
If [H3O+]<[OH-] basic or alkaline solution
If the hydroxide concentration is 1 X 10–4M, what is the hydronium ion concentration?

5. Formulas [H3O+][OH-] = 1 X 10 –14 M
Use to find one [] given the other []
Find the hydroxide ion concentration if the hydronium ion concentration is 1 X 10-5M. Is this acidic basic or neutral?
pH=-log [H3O+]
Use to find pH given [H+]
Find the pH if the hydronium ion concentration is 2.1 X 10-5M.
pOH= -log [OH-]
Use to find pOH given [OH-]
Find the pOH if the hydroxide ion concentration is 4.1 X 10-5M.

6. pH pH 1-6 7 8-14 Acid neutral base pOH 14-8 7 6-1 pH +pOH=14
Use to find one given the other.
Example: Find the pOH if the pH is 8.2.
[H+]= 10-pH
Use to find [H3O+] given to pH
Example: Find the [H+] given a pH of 11.5.
[OH-]= 10-pOH
Use to find [OH-] given to pOH
Example: Find the [OH-] given a pOH of 7.5.

7. pH paper- have indicators on them pH meter
Measuring pH
To measure pH:
Use acid/base indicators: change color based on [hydrogen ion ], many types pg 590
pH paper- have indicators on them
pH meter

8. 3 Types of Acids & Bases Arrhenius acids & bases
Bronsted-Lowery acids & bases
Lewis acids & bases

9. 3 Types of Acids & Bases Arrhenius acid: Produce H+ ion
Arrhenius base: Produce OH- ion
Bronsted-Lowery Acid: H+ donor
Bronsted Lowery Base: H+ acceptor
Lewis acid- can accept pair of e- to form a covalent bond (H+)
Lewis base- can donate pair of e- to form a covalent bond (OH-)

10. 3 Types of Acids & Bases Type Arrhenius Bronsted-Lowry Lewis Acids
Produce H+ ion
H+ donor
can accept pair of e- to form a covalent bond (H+)
Bases
Produce OH- ion
H+ acceptor
can donate pair of e- to form a covalent bond (OH-)

11. Conjugate Pairs Be able to identify conjugate acid base pair:
Conjugate base – what is left of acid after hydrogen ion is donated
Conjugate acid – base plus the hydrogen ion that was donated/accepted
Amphoteric- can be acid or base
Identify the conjugate acid-base pairs in the following reactions.
    H2SO4 + H2O  HSO4- + H3O+
    HI(aq) + H2O(l)  H3O+(aq) + I-(aq)

12. ionization Ionization- Strong acid- completely ionizes becomes weak CB
Weak acid- incompletely ionizes becomes strong CB
Can write ionization equation:
Can write acid dissociation constant (Ka)
Ka= [Products]/[Reactants]
Don’t include water
Smaller #=weaker acid
Polyprotic acids- take 1 H at a time
Also applies to bases called Kb

13. Example Questions Write the steps in the complete ionization of H2S.
Write the ionization equation and acid ionization constant expression for the following acids.
a.       HCl
b.      HNO2
c H3PO4
Write ionization equations and base ionization constant expressions for the following bases.
a.   propylamine (C3H7NH2)
Given: 0.1M solution of ethanoic acid is partially ionized. The [H+] is 1.34 X 10-3M. What is the Ka of ethanoic acid?

14. Neutralization Neutralization- Double displacement reaction NaCl
Acid + Base  salt + water
Nitric acid & calcium hydroxide
Sulfuric acid & aluminum hydroxide
Can find acid & base that form salt
NaCl
NaHCO3

15. Titration Measure volume of acid soln. Of [unknown] in flask
Titration- Use known to find unknown
Need mol ratio for H+:OH-
Steps in titration:
Measure volume of acid soln. Of [unknown] in flask
Add indicator
Measured volume of base [known] ‘standard’ are added until slight color change (endpoint)
Use MV=MV
A 25 mL soln of hydrochloric acid neutralized by 18mL of 1M NaOH. What is the [hydrochloric acid]?

16. Salts Salts Strong acid + strong base neutral salt solution.
Made from an acid & base
Strong acid + strong base neutral salt solution.
Weak acid + strong base  basic salt solution.
Strong acid + weak base  Acidic salt soution.
Be able to predict the acid & base that make the salt
Buffers- solution where the pH remains constant when an acid/base are added
Can absorb or release H+