Chapter 8 Flashcards
Relationship between hydronium ion concentration and pH
Hydronium ion concentration is ten raised to the power of the negative pH
pH = -log [H3O+]
What is the relationship between pOH and [OH-]?
pOH = -log[OH-]
acids vs. bases
which are the strong bases on the periodic table
start at Li, go down 5 and up 3
strong acids
HCl, HBr, HI, HNO3, H2SO4, HClO4
What’s the clue for a weak acid?
If we are given a Ka value
Ka
Kb
Conjugate acid-base pairs
more positive = acid
acid names from anion names: -ide
hydro___ic
acid names from anion names: -ate
-ic
if you ate it, it’s icky
acid names from anion names: -ite
-ous
review oxyanions: +O atom
per___ate (acid changes to -ic)
review oxyanions: -O atom
-ite (acid changes to -ous)
review oxyanions: -2 O atoms
hypo___ite (acid changes to -ous)
What is the relationship between pKa and Ka?
How do we get Ka if given pKa?
pKa = -logKa
OR
Ka=10^ -pKa
relationship between Ka, Kb, and Kw
Ka x Kb = Kw
relationship between pKa and pKb
pKa + pKb = 14
What is [H30+] x [OH-]
[H30+] x [OH-] = 1.0 x 10^-14
What is a pH indicator?
(not part of chemical reaction, just tells us when to stop titrating)
What are the criteria for a buffer system?
smaller pKa means ___ acid and ___ ka
smaller pKa means stronger acid and larger ka
Henderson-Hasselbalch equation
pH=pKa + log [A-] / [HA]
Rearrange Hasselbalch to solve for [A-] or [c.base]
