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Soluble Ionic Compounds
All common compounds of Group 1A (Na, K) All common nitrates, acetates and most perchlorates All common chlorides, bromides and iodides (except Ag, Pb, Cu and Hg2) and all common fluorides (except Pb and Group 2A) All common sulfates (except Ca, Sr, Ba, Ag, and Pb
Insoluble Ionic Compounds
All common metal hydroxides (except group 1A) All common carbonates and phosphates (except group 1A and NH4) All common sulfides are insoluble (except group 1A, Group 2A and NH4)
Solubility and Equilibrium
A saturated solution contains max amount of dissolved solute in the presence of undissolved solute An unsaturated solution contains less than the equilibrium concentration of dissolved solute. If more solute is added, it will dissolve
Effect of pH on Solubility
The addition of H3O will increase the solubility of a salt that contains the anion of a weak acid
Predicting the Formation of a Precipitate
If Q > K, a precipitate will form
Selective Precipitation
A precipitation ion is added to the solution until the Q of the more soluble compound is almost equal to K The less soluble compound will precipitate, leaving behind the ion of the more soluble compound
Complex ion formation
Complex ions form when a central metal cation becomes covalently bonded to two or more anions and/or molecules
Spontaneous change
One that occurs without a continuous input of energy
Freedom of Particle Motion
All spontaneous endothermic processes result in an increase in the freedom of motion of the particles in the system
Molecular interpretation of entropy
S = k lnW S: entropy W: microstates K: Boltzmann constant
Entropy
A system with fewer microstates has lower entropy A system with more microstates has higher entropy All spontaneous endothermic processes exhibit an increase in entropy
Concept of delta S
deltaS = qrev/T
Second Law of Thermodynamics 
All real processes occur spontaneously in the direction that increases the entropy of the universe For a process to be spontaneous, a decrease in the entropy of the system must be offset by a larger increase in the entropy of the surroundings
Standard Molar Entropies
S0 is the standard molar entropy of a substance, measured for a substance in its standard state in J/molK 1 atm for gas, 1M for solutions, substance in its most stable form for solids and liquids
Factors affecting entropy
Temperature (temp increases, S0 increases) Physical state (disorder increases, S0 increases) Formation of a solution Atomic size and molecular complexity (atom size increases, S0 increases)
Entropy change and dissolution of a salt
The entropy of a salt solution is usually greater than that of the solid and of water
Entropy of gas dissolved in liquid
Entropy of a gas is already so high that it decreases when the gas dissolves
Standard entropy of reaction
ΔSºrxn is the entropy change that occurs when all reactants and products are in their standard states
Predicting the Sign of ΔSºrxn
ΔSºrxn is positive if the amount of gas increases ΔSºrxn is negative if the amount of gas decreases ΔSºrxn is likely to be positive if a new structure forms that has more freedom of motion
Entropy changes in the surroundings
A decrease in the entropy of the system is outweighed by an increase in the entropy of the surroundings In an exothermic process, the surroundings absorbs the heat released by the system and Ssurr increases In an endothermic process, Ssurr decreases
Temperature at which heat is transferred
The heat transferred is specific for the reaction and is the same regardless of temperature The impact on the surroundings is larger when they are at lower temperature because there is a greater relative change in Ssurr
ΔSºuniv for spontaneous reactions
Exothermic reactions will always be spontaneous For endothermic reactions where ΔSºsys < 0, ΔSºsurr must be larger thanΔSºsys for the reaction to be spontaneous For endothermic reactions where ΔSºsys > 0, ΔSºsurr must be smaller than ΔSºsys for the reaction to be spontaneous
Gibbs Free Energy
ΔG is a measure of the spontaneity of a process and of the useful energy available from it ΔG < 0 for spontaneous ΔG > 0 for nonspontaneous ΔG = 0 for equilibrium 
Calculating ΔG
ΔGsys = ΔHsys - TΔSsys ΔGºrxn = ΣmΔGproducts - ΣnΔGreactants
ΔG and Useful Work
ΔG is the max useful work done by a system during a spontaneous process ΔG is the minimum work that must be done to a system to make a nonspontaneous process occur

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