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Large K
High concentration of products
Low concentration of reactants
Forward rxn is favored
Reaction lies to the right
Small K
High concentration of reactants
Low concentration of products
Reverse rxn is favored
Reaction lies to the left
K approximately 1
Significant concentration of reactants & products
Neither reaction is favored
K for the reverse reaction
inverse of K for the forward reaction
A + B ⇌ C + D K1
C + D ⇌ A + B 1/K1
If you multiply coefficients in equation
K will be raised to that power
A + B ⇌ C + D K1
nA + nB ⇌ nC + nD K = K1n
K for a net equation
product of the K values for individual reactions
Hess’s Law
A + B ⇌ C + D K1
C + F ⇌ G + A K2
B + F ⇌ D + GK3 = (K1)(K2)
If Q = K then
those values are actually at equilibrium.
If Q > K
the right side is too large and the system will shift to the left to reach equilibrium
If Q < K
the right side is too small and the system will shift to the right to reach equilibrium
Le Chatelier’s Principle
If a system at equilibrium is disturbed the equilibrium will shift to minimize the disturbance
A system at equilibrium tries to maintain that equilibrium
If the concentration of a reactant or product is increased,
the reaction will consume what was added
Add more reactants – shift to right
Add more products – shift to left
If the concentration of a reactant or product is decreased,
the reaction will replace what was removed
Remove reactants – shift to left
Remove products – shift to right
If the volume decreases,
pressure increases, the reaction will shift to the side with fewer moles of gas particles
If the volume increases,
pressure decreases, the reaction will shift to the side with more moles of gas particles
when concentration and pressure change, K…
does NOT change
when temperature changes, K…
DOES change
In Exothermic Reactions…
N2(g) + 3H2(g) ⇌ 2NH3(g) + heat
Heat is a product
If the temperature increases, the reaction will shift to the left.
If the temperature decreases, the reaction will shift to the right
In Endothermic Reactions…
N2O4(g) + heat ⇌ 2NO2(g)
Heat is a reactant
If the temperature increases, the reaction will shift to the right
If the temperature decreases, the reaction will shift to the left
Catalysts change the _______ of the reaction but not the ________ or _______________
RATE, K or equilibrium composition
+∆H
endothermic
-∆H
exothermic
+∆S
more disorder
-∆S
less disorder
+∆G
not thermodynamically favorable
-∆G
thermodynamically favorable
∆G = ∆H – T∆S
Convert S to kJ
∆G = – RTlnK
R = 8.314 J mol-1K-1
K = e-∆G/RT
Crystallization
opposite of dissolving
Rate of dissolving =
rate of crystallization
Saturated solution
in equilibrium with undissolved solute
Maximum amount of solute is dissolved
Excess may be present on bottom
Li+1
Soluble, no exceptions
Na+1
Soluble, no exceptions
K+1
Soluble, no exceptions
NH4+1
Soluble, no exceptions
NO3-1
Soluble, no exceptions
ClO3-1
Soluble, no exceptions
ClO4-1
Soluble, no exceptions
C2H3O2-1
Soluble, no exceptions
Cl-1
Soluble
Exceptions: Ag+1, Pb+2, Hg2+2
Br-1
Soluble
Exceptions: Ag+1, Pb+2, Hg2+2
I-1
Soluble
Exceptions: Ag+1, Pb+2, Hg2+2
SO4-2
Soluble
Exceptions: Ca+2, Sr+2, Ba+2, Pb+2
OH-1
Insoluble
Exceptions: Li+1, Na+1, K+1, NH4+1, Ca+2, Sr+2, Ba+2
S-2
Insoluble
Exceptions: Li+1, Na+1, K+1, NH4+1, Ca+2, Sr+2, Ba+2
CO3-2
Insoluble
Exceptions: Li+1, Na+1, K+1, NH4+1
PO4-3
Insoluble
Exceptions: Li+1, Na+1, K+1, NH4+1
SO3-2
Insoluble
Exceptions: Li+1, Na+1, K+1, NH4+1
Ksp
represents the extent to which an ionic solid dissolves in water
Molar solubility
moles/liter
Gram solubility
g/liter or g/100mL
When salts have same number of total ions…
Higher Ksp is more soluble
If salts have different numbers of total ions…
can’t compare Ksp directly
Common Ion Effect
Solubility of a substance is reduced when a substance containing a common ion is also present in the solution
Ksp = [A+][X-]
Q = K
at equilibrium
solution is saturated
precipitation = dissolving
Ksp = [A+][X-]
Q < K
less ions are present
no precipitation
Ksp = [A+][X-]
Q > K
more ions are present
precipitation
When mixing solutions a precipitate will form from…
the salt with the lowest Ksp value first
Can only compare directly when ion ratio is the same