π¨π»βπ¨ Flashcards
Solubility rules 1
(Li+) (Na+)(K+)(Rb+)(Cs+)(NH4)
soluble no exceptions!!!
Solubility rule 2
(No3-)(C2H3O2-)(CH3COO-) are all soluble
No exceptions!!!!
Solubility rule 3
Cl- Br- I-
Are soluble
Except when bound to
Ag+ Hg2 2+ or Pb 2+
Solubility rule 4
SO4 2- is soluble except when bound to Ca 2+ Sr 2+ Ba 2+ Hg2 2+ Pb 2+
Solubility rule 5
All other compounds are practically insoluble
Soluble trends
Heat and pressure for solids
As heat increase solublilty also increases
Pressure has no particular change
Solubility trends for gases
As temp increases solubility decreases!!!!!!
As pressure increases solubility also increases!!!!
Think CO2 in soda pop
Molarity
Moles / L of solution
Mass percent
g of solute / g of solution x 100%
Dilution or concentration formula
M1V1=M2V2
Equilibrium constant expression
Keq = [c]^c x [D]^d / [A]^a x [B]^b
Only for aqueous or gases
aA + bB <=> cC + dD
The brackets indicate concentrations molarity
If a given equation is at equilibrium at the same temperature the keq will always be the same
What is a precipitation reaction
When two aqueous compounds forma solid
It will occurs if one of the products is a solid or insoluble
Complete ionic equation
All ions and soluble things are broken apart into ions
Insoluble things are not!!!!
Spectator ions
Ions that donβt change
Net ionic equation
Does not contain the spectator ions
Energy
The ability to do work
Jules to calories ratio
Calorie to kilocalories
4.184 Jules for 1 calorie (lower case)
1 Calorie or kilocalorie = 1000 calories
System
V
Surrounding
The part of the universe being studied (generally the reaction being studied)
V
Everything else
Law of the conservation of energy
Energy can neither be created or destroyed
Heat
Is the transfer of energy from one βbodyβ to another due to a difference of temperature
^H or the change of enthalpy
Is equal to heat at a constant pressure
Endothermic
V exothermic
Endo = +^ = products have more energy then reactants
Exo = -^ = products have less energy then reactants
ColisiΓ³n theory
Desired product only forms if effective collision forms
The collisions gives the particles the energy they need to break up and form bonds
Increase concentration
More collisions
Increase rate of reactions
Temp and collisions
As temp increases it will increase number of collisions and increase the energy of the reactions
Right shift of the curve
Activation energy
E(a)
The minimum kinetic energy required by a collision of reactants to create the desired products
Energy of reactants to the top of the hump
Catalyst
Reduces the height of the hump ( Ea) which speeds up the reaction
(Shifts dotted line to the right)
Is not consumed instead it facilitates the reaction
(HAS NO EFFECT On LE Chatliers )
Equilibrium
Many (not all) chemical equations are reversible - they can both forward or backwards
The reaction does not stop !!!!!
But when rate forward and backward are equal it has reached equilibrium
Does not have to have the same amount on both sides
οΏΌ
Le chatliers principal
Equilibrium can be shifted by changing conditions of the system
If the equilibrium is stressed it will temporarily not be at equilibrium but will the shift to remove the stress so it can regain equilibrium
Stresses include
Change in concentrations of reactants or products (does not change keq)
Change in pressure
Change in temp ( exothermic written with products, endo written with reactants)
Not no bad (catalyst) π΅
How pressure causes a shift
Only gas !!!
If increased will shift from high to low to balance
If decreased will shift from low to high to balance
Not soluble solubility rules 1 π
Co3 2- is not soluble except when
Bound to NA li k rb cs nh4
Saturated
Unsaturated
Supersaturate
Saturated is max amount of solute dissolved in solvent
Unsat < max
Super > max
Solute vs solvent
Solvent major
Solute minor
Types of mixtures
Solid liquid or gas / liquid
Solid / solid
Liquid / liquid
Polar dissolves in polar
Non polar in non polar
Dissociation
When an ionic compound splits apart into ions in an aqueous solution
Hydrated
When an ion is completely surrounded by water
Electrolyte
Any substance that can divide into ions when placed in water
Not soluble rule 2
Oh is not soluble except when bound to li NA k Rb Cs NH4 Sr Ba
