Chemistry Notes for Thursday, 4/15

In class we discussed how Dr. B checked and graded the R constant labs. I however, do not have those notes, and leave it to you guys to fill that part in.
CLASS NOTES:
- Arrhenius Acids are molecular compounds with ionizable hydrogen atoms
-Their water solutions are known as aqueous acids
-All aqueous acids are elctrolytes
- A strong acid ionizes completely in aqueous solutions.
-Strong acids are strong electrolytes
Ex: HClO4 HCl, HNO3

-A weak acid relaes few ions in aqueous solutions
- Hydronium ions, anions, and dissolved acid molecules in aqueous solutions
Ex: HCN
-organic acids (____COOH molecules), such as acetic acid are weak acids

-Most bases are inoic compounds containing metal cations and the OH- anion
-Ammonia, NH3, is molecular
-Ammonia produces OH- ions when it reacs with water molecules
-The strength of a base depends on the extent in which it dissociates in a solution
-Strong bases --> Strong electrolytes
Amount of H3O+'s to OH-'s in types of solutions
Acidic
H3O+ > 10^-7 Moles >OH-
Nuetral
H3O+ = 10^-7 Moles = OH-
Basic
H3O+ < 10^-7 Moles< OH-

Bronsted Lowry Acids and Bases
- A Bronsted Lowry-Acid is a molecule or ion that is a proton donor
-HCl acts as a Bronsted-Lowry acid when it reacts with ammonia
-Water can act as a Bronsted-Lowry Acid
-A Bronsted-Lowry Base is a molecule or ion that Acts as a proton acceptor
-Ammonia accepts a proton from HCl, and is therefore and Bronsted-Lowry Base
- the OH- ion produced in solutions by acids is a Bronsted-Lowry Base

- In a Bronsted-Lowry Acid-Base reaction, protons are transferred from one reactant(the acid) to another (the base)