Inorganic chemistry / module 2

chapter 7 and 8

bronstead acid

acts as a proton donor

bronstead base

proton acceptor

k_a

acid dissociation constant

products over reactants

k_b

base dissociation constant

k_w

self-ionization constant

ionic strength

a measure of the total concentration of ions in solution

the more highly its charged, more its counted

large Ka value

stronger the acid

smaller the pKa value

stronger the acid

smaller the pKb value

stronger the base

larger the Kb value

stronger the base

aquated cations as Bronstead acids

by loss of H^+ from a coordinated water molecule

charge density

charge of the ion / surface area of the ion

amphoteric behavior

if an oxide or hydroxide is able to act as either an acid or base

saturated

when equillibrium is reached

solubility

the mass of the solid is dissolved when equillibrium is reached

sparingly soluble

if the solubility of an ionic salt is extremely small

common ion effect

the suppression of the ionization of a weak acid or a weak base by the presence of a common ion from a strong electrolyte

decrease in solubility of an ionic precipitate

oxidation

refers to gaining oxygen

losing hydrogen

or losing one or more electrons

reduction

refers to losing oxygen

gaining hydrogen

gaining one or more electrons

electrolytic cell

the passage of electrical current initiates a redox reaction

galvanic cell

spontaneous redox reaction occurs and generates an electrical current

electrode

electrical conductor

anode

electrode where oxidation takes place

cathode

electrode where reduction takes place

electrical circuit

electrons flow from anode to the cathode

electrolyte

conducting ionic solution

salt bridge

completes electrical circuit by allowing migration of non-reactive ions so that electrolyte neutrality is preserved

cell potential

measure of the driving force of the reaction, ability to push electrons through the circuit

the more positive the standard reduction potential

the more readily the species on the left is reduced to the species on the right

negative standard reduction potentials

indicate that the species to the right behaves as a reducing agent

what is deltaG depends on

changes in both enthalpy and entropy

Bell’s equation

pKa is around (8-5n)

lewis acid

an electron acceptor

lewis base

an electron donor

amphoteric

when an oxide or hydroxide acts as an acid or base

saturated

when the equilibrium is reached

solubility

when a mass of solid that dissolves at a specific temp

sparingly soluble 

when the solubility of an ionic salt is extremely small