chapter 13: part 2 for the 3rd test Flashcards
what is a polyprotic acid
acid molecules with more than 1 ionizable H
how do polyprotic acids ionize and what happens to the Ka
in steps; each H is removed sequentially the Ka decreases after each step
Ka x Kb =?
[H3O+]][OH-] = Kw
as the strength of acid increases what happens to the strength of the conjugate base
- the strength of its conjugate base must decrease
what is the relationship between the acid and conjugate base
- strong acid = weaker conjugate base
- weaker acid = stronger conjugate base
what is pK
can be used to express the strength of an acid
- pKa = -log(Ka)
- pkb= -log(Kb)
if an acid is strong, then what is the pKa
- small pKa because of the -log
what is an oxide
molecule that contains H-O-X
x is any element
in an oxide if X is a nonmental then what is the compound
SO3 + H2O –> H2SO4
the compound is a covalent oxide
- dissolved in water it becomes an acidic solution
- forms an acidic oxice
in an oxide, if X is a metal then was is the solution
CaO + H2O —> Ca(OH)2
- ionic oxide
- when dissolved in water, a basic solution forms and it is basic
what is the lewis theory
- acids: electron pair acceptors (must have an atom with an empty valence orbital0
- bases: electron pair donors (must have a lone pair electrons)
what can lewis bases interact with
things other than protons
anything that could be a bronsted lowry base is a [blank] base
- lewis base
* not all lewis bases are B-: bases
what is the arrhenius acid and base rule
- acid: substance that produces H+ in water
- base: substance that produces
what is the bronsted lowry acid and base rule
acid: a proton donor
base: a proton acceptor
