| Chapter 14 |
| Strong Acids: HCl HBr HI HNO3 H2SO4 HClO4 |
| Strong Bases: *anything in groups 1&2 on the periodic table with OH-* ex. NaOH Ca(OH)2 Mg(OH)2 |
| %ionization or dissaociation = Amount Disassociated / initial concentration X 100 pH = -log [H+] Kw= 1x10^-14 [H+] [OH-] = 1x10^-14 Acid > 1x10^-7 Base < 1x10^-7 Kb- OH Ka- H pOH = -log [M] pH = -log [M] |
| Highest to Lowest pH: RbOH H2S CaCl2 NaCN HI NH3= 1.8x10^-15 Kb |
| Example: A 0.1 M solution of HC3H5O2 has a pH of 1.35. What is the Ka? HC3H5O2 ---> C3H5O2- + H+ I .1 0 0 C -x x x E .1-x x x |
| [H+] = 10^-1.35 = 4.47x10^-2 M (4.47x10^-2)^2 ---------------------- = .1- (4.47x10^-2) Ka= .0361 |