Chemistry Flashcards
(26 cards)
Precipitation
The process of forming a solid product from aqueous reactants
Dissolution
The process of forming aqueous products from solid reactants
Solubility Product, Ksp
The equilibrium constant for solubility equilibria
Qsp > Ksp
The reaction proceeds in the reverse direction and precipitation will occur
Qsp < Ksp
The reaction proceeds in the forward direction and the solution is not saturated
Selective Precipitation
A technique used to separate ions in an aqueous solution by using a reactant that precipitates one or more of the ions while leaving other ions in the solution
Common Ion Effect
An effect that suppresses the ionization of a weak base by adding more of an ion that is a product of the equilibrium. Uses Le Chatelier’s Principle
An increase in one’s ion concentration…
…must be balanced by a proportional decrease in the other.
Coordinate Covalent (Dative) Bond
occurs when one of the atoms in a covalent bond provides both bonding electrons.
Lewis acid-base chemistry
Reactions involving the formation of coordinate covalent bonds
Lewis Acid
The species accepting the electron pair (usually positive)
Lewis Base
The species donating the electron pair forming the covalent bond (usually negative)
Lewis Acid-Base Adduct
Product(s) of a lewis acid and base
Formation constant, Kf
Equilibrium constant for the reaction of a metal ion with one or more ligands to form a coordination complex in the forward direction (products/ reactants)
Dissociation Constant, Kd
equilibrium constant for the reverse reaction/ decomposition of the complex ion
Molar Solubility
Number of moles of a substance to make 1 L of saturated solution
Galvanic Cell
a combination of a reductive and an oxidation half reaction and the components necessary to exchange electrons and counterions
anode
where oxidation occurs (lose e-) Ex. Cu(s) -> Cu2+(aq) + 2e-
cathode
Where reduction occurs (gain e-) Ex. Ag+(aq) + e- -> Ag(s)
Salt bridge
allows for flow of counterions to maintain charge balance, has electrolytes
Wire
connects electrodes to allow for exchange of e-, measures current
Eº(cell)
Determines spontaneity of a redox process and the amount of free energy available to do electrical work and is recorded at STP
For a redox reaction to be spontaneous, the reductive half raction must have a _______ than the oxidative half reaction
higher Eº
Electrochemical reactions that are ____________ are galvanic cells
spontaneous
