1. Acids and Bases

2. Outline Acidic and Basic Solutions Neutral Solution Arrhenius Model
Bronsted-Lowry Model
Amphoteric and Polyprotic
Strength of Acids and Bases
Neutralization Reaction
Titration

3. Acidic and Basic Solutions
Acidic Solution – Contains more hydrogen ions than hydroxide ions
Turn blue litmus red, tastes sour, has a pH of less than 7, and reacts with active metals, carbonates, and bases. The closer to 1, the more acidic.

4. Acidic and Basic Solutions
Basic Solution – Contains more hydroxide ions than hydrogen ions
Turns red litmus blue, tastes bitter, feels soapy or slippery, has a pH of greater than 7, and reacts with acids. The closer to 14 the more basic.

5. Neutral Solutions
Neutral Solution – Contains equal number of hydroxide ions and hydrogen ions.
Has a pH of 7.
Water is a good example

6. Arrhenius Model
Acids contain hydrogen and ionize to produce hydrogen ions in aqueous solutions
Bases contain hydroxide groups and dissociate to produce hydroxide ions in aqueous solutions

7. Bronsted-Lowry Model
Acid is a hydrogen ion donor. Creates a conjugate base.
Base is a hydrogen ion acceptor. Creates a conjugate acid.
Works in any solvent

8. Bronsted-Lowry Model Cont.
Conjugate Acid – substance produced when a base accepts a hydrogen ion.
Conjugate Base – substance produced when an acid donates a hydrogen ion.

9. Amphoteric and Polyprotic Acid
Amphoteric – Substance that can act as both an acid and a base such as water.
Polyprotic Acid – An acid that can donate more than one hydrogen ion.
Two is diprotic
Three is triprotic

10. Strength of Acids and Bases
Strong Acids/Bases – ones that completely ionize
Includes HCl, HNO3
Weak Acids/Bases – Only partially ionizes in dilute aqueous solutions.
Includes HF, Acetic, H2S
Every change in pH is a factor of ten in hydrogen ion concentration. The smaller the number, the higher the concentration.
pH of 1 has 1000 times more hydrogen ions than a pH of 4.
pH of 12 has 100 times less hydrogen ions than a pH of 10.

11. Neutralization Reaction
When an acid and a base react in an aqueous solution (water) to produce a salt and water
Salt – ionic compound with the cation from the base, and the anion from the acid
HCl + NaOH -> NaCl, a salt, + H2O

12. Titration
Reacting a known concentration of solution with an unknown concentration of solution
Equivalence Point – when moles of H+ equal moles of OH-
End Point – Indicator in titration changes color indicating equivalence point
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