Chapter 10 Flashcards
Arrhenius Acids
Dissociate to form excess H+ in solution
Arrhenius Bases
Dissociate to form excess OH- in solution
Brønsted-Lowry Acid
H+ donor
Brønsted-Lowry Base
H+ acceptor
Lewis Acid
Electron pair acceptor
Lewis Base
Electron pair donor
Amphiprotic
Can either accept/donate an H
Amphoteric Species
Can behave as an acid or base
Ka
High Ka: strong acid that will completely dissociate in solution
Ka greater than water slightly: acid is weak acid with minimal dissociation
Kb
High Kb: strong base that will completely dissociate in solution
Kb greater than water slightly: base is weak base with minimal dissociation
pH and pOH
pH + pOH = 14
Kw
= Ka * Kb
Acid
- Loses a proton
- Use moles of H+ (H3O+)
Conjugate Acid: Base that gains a proton
Ending in -ic: derivatives of anions ending in -ate
Ending in -ous: derivatives of anions ending in -ite
Base
- Gains a proton
- Use moles of OH-
Conjugate Base: Acid that loses a proton
Normality
Amount of mols of OH- or H+ yielded from a certain M of compound
M * mols = N
Henderson-Hasselbach Equation
Titration Curve
Buffering Region: [HA] ~ [A-]
Flattest portion of titration curve (resistant to changes in pH)
Half-equivalence Point: [HA] = [A-]
Center of Buffering Region
Equivalence Point:
Steepest point of titration curve, equivalents of acid present = equivalents of base added
Endpoint: pH where an indicator turns its final color
Buffer Solution
Designed to resist changes in pH with optimal buffering capacity within 1pH from pKa
