Acids

1
Acids

• Acids
• Formulas
• Examples
• Properties
• sour
• dissociate in water
• feel like water but can burn.

• React with metals.
• Conduct electricity.
• Turn blue litmus red.

2
Bases

• Hydroxide
• Examples
• Uses
• Taste
• Bitter
• Feel smooth and slippery.
• Will burn if left on.

• Do not react with metals
• Conduct electricity.
• Turns red litmus blue.

3
Acids and Bases

• Neutralization reactions.
• Arrhenius Definitions
• Acids
• Bases
• Limitations
• Bronsted-Lowry Definitions
• Acids
• Bases

• Hydronium ion
• Conjugate--acid base pairs.
• Inverse relationship
• Strong acids
• ionization
• Nitric, Hydrochloric, Sulfuric
• Weak Acids

4
Acids and Bases

• Strong bases
• NaOH KOH, CaO, etc
• Weak bases
• ammonia carbonate ion phosphate ion

• Acid Dissociation Constant
• Equilibrium Constant
• Low KA weak acid
• Large Kastrong acid (1)
• Same goes for Kb
• calculating

5
Salts as Acids and Bases

• Salts of Strong acids strong bases are neutral.
• Salts of Strong acids and weak bases are slightly
  acidic.
• Salts of weak acids and strong bases are slightly
  basic.

• Salts of weak acids and weak bases can be either
  acidic, basic, or neutral

6
Naming Acids

• Monoprotic and diprotic acids
• Acidic hydrogen are usually bonded to polar
  molecules.
• Binary Acids
• Oxy acids--acidic hydrogens are attached to
  hydrogen.

• Carboxylic Acids--organic acids.Usually weak
  acids.

7
Naming Acids

• If anion ends in --ide.. Change the --ide to --ic
  and add the prefix hydro.
• ExampleHCl
• If anion ends in --ate, drop ate and add ic.
• If anion ends in --ite, drop ite and add ous.

8
Water

• Self-ionization of water.
• Amphoteric
• Kw--ion product constant.
• Kw1.0 X 10-14
• Finding H3O and OH-

• pH scale
• definition
• pH-logH3O
• pOH-logOH-
• pH pOH14
• indicators
• pH meter

9
Buffers

• Definition
• H3O C2H3O2- ---gtH20 HC2H3O2
• buffer capacity
• made of a weak acid and its conjugate base.
• Carbonic acid/bicarbonate buffer system

10
Titrations

• Controlled neutralization reaction
• Buret
• standard solution
• drop by drop
• N1V1N2V2
• Equivalence point--point at which all acid or
  base is neutralized.

• End point--point at which indicator changes
  color.

11
Choosing Indicators

• Strong acid strong baseneutral solution.
• Indicator with change at pH of 7 is needed.
• Weak Acid Strong base slightly basic
  solution.
• Indicator with pH change greater than 7 is needed.

• Weak base Strong AcidSlightly acidic solution
• Indicator with pH change below 7 is needed.