Chem 1A Unit 3

a state reached by reversible reactions when forward rate = reverse rate

[products]/[reactants]

stressing the equilibrium

an equilibrium system under stress will shift in the direction required to relieve said stress

acid-base, solubility, separation (ass)

molecules separate from each other

donate H+

accept H+ ion

high

low

water

moles of H+ are equal to moles of OH-

gradually adding known acidase to a sample to gain info on the sample

known volume and concentration

known volume and unknown concentration

changes rapidly

point in titration curve where amount of titrant added is equal to analyte amount

act 1: stress equilibrium to use up limiting reactant, act 2: use ICE table to calculate the pH after the new equilibrium is met

a balanced chemical equation

1/2 equivalence point

tabular method to organize initial concentrations of reactants, the changes that occur and the equilibrium concentration reached

acid, base

strong base

H2O

OH- or H3O

solutions containing large amounts of both weak acid and conjugate base that can resist large pH changes if adding strong acid or base

weak acidase and conjugate base/acid, or weak acidase and strong base/acid

stabilize pH against stress

strong acid

neutralized

the area on the titration curve where K is stressed and the pH is stable

conjugate base

conjugate acid

product of a base in a reaction, can donate H+ in reverse reaction

product of acid in a reaction, can accept H+ in reverse reaction

used to approximate equilibrium concentration when x is very small relative to concentration of the reactants

maximum amount of a solute that can dissolve completely in a given solvent

forward reaction rate = backward reaction rate

molarity in terms of mol/L

k= proportionality constant/K=equilibrium constant

stoichiometric coefficient, represents molarity^n

forward reaction/product favored

backward reactioneactant favored

excess products

excess reactants

stress

Temperature, delta H can verify

speeds up

slows down

speeds up

slows down

more soluble

molecular covalent liquids and solids

gases

ionic solids/solubility product

maximum, cannot

reactants may have run out

hard

easier

14

polyatomic ion OH-

H3O+

negative log of [H+]

negative log of [OH-}

negative log of (whatever)

relative low pH

relatively high pH

low pH

higher than 7 pH

donors

acceptors

control how much H+ ends in solution and how acidic it is

being an acid

being an acid

weak acid

spread/stabilize charge making it less/more likely to donate protons

being a base

being a base

steal protons from water to make OH-

Nitrogen with lone pair (always a weak base)

water

do not participate in reaction but neutralize charge

neutral water, unequal moles leave excess acid or base

small K, mostly solid
large K, mostly dissolved

small K, higher pH
large K, lower pH

different

equiblibrium associated with separating something

uses sepration funnel to separate layers with a spigot

uses charged beads instead of separate liquid layer to separate ionic substances from neutral ones, typically separating acids from acids

be used to separate components of a mixture

predicted by comparing pH/pOH to pKa/pKb

-RTlnK

negative delta G= favorable (forward rxn), 0=equilibrium, positive=unfavorable (reverse rxn)

inverse relationship, if p value increases, the other will decrease

1*10^-14

1 reactant is strong acidase

reactants are all weak acidase