Exam 1 Content Flashcards
Acid/Base
Avogadro’s Constant
6.022x10^23
Molar mass
(grams substance/moles) = molar mass
Molarity
moles of solutue/liters of solution
Buffers
resist changes in pH. Made from weak acids/bases and their salts
K(a)
represent the equilibrium constant. K<1 weak acid, K>1 strong acid.
Bronsted-Lowry Acids/Base
Acid: any substance that donates a proton (H+)
Base: any substances that accepts a proton (H+)
Henderson-Hasselbach Equation
pH = pKa + log (A-/HA) or (B/HB+)
pKa
- The pH at which both the acid (HA or HB+) and the conjugate (A- or B) base are maintained in equal amounts.
- Measure of hydrogen ion concentration required to put a H+ back on the conjugate base of the acid.
10^pH-pK
(A-/HA) or (B/HB+)
Arrhenius Acids/Bases
Acid: substance that when ADDED to WATER will increase the (H30+) concentration of the solution
Base: substance that when ADDED to WATER will increase the (OH-) concentration of the solution.
Lewis Acids/Bases
Acid: electron pair acceptor (usually metals)
Base: electron pair donor
7 Strong Acids
HCl HBr HI H2SO4 (dirpotic acid) HNO3 HClO4 (perchloric acid) HClO3 (chloric acid)
Strong Bases
Any group 1&2 Metal Hydroxides (OH). but not Mg(OH2).
Neutralization Reaction
reaction between an acid/base that yields water and a salt. (Bronsted acid/base)
Ionic equation
written with soluble substances written as ions and only those involved in the reaction. 2H(+) + 2OH(^-1) –> 2H2O
(H+) =
10^-pH
(OH-) =
10^-pOH