Reaction Quotient (Q vs. K), Common Ion Effect
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K>1
products area favored at equilibrium
K<1
reactants are favored at equilibrium
What is Q? (Qc or Qp)
Q is what you get when you measure the amounts of products and reactants in an equilibrium reaction and then insert those numbers into your Kc equation (these numbers may or may not be at equilibrium yet). This is how you check if your solution is at equilibrium
Q = K
at equilibrium
Q is less than K
shift right (products) (too much reactant. need more products)
Q is more than K
shift left (reactants) (too much product. need more reactants)
When solving for Ksp calculation on the DAT, you’ll be asked one of 4 things:
1) calculate molor solubility 2) calculate Ksp 3) calculate solubility for a common ion effect questions 4) determine if precipitation will occur
When solving K rate equations, remember NOT to include
reactants or products that are a liquid or a solid
What is the common ion effect?
You have an equilibrium reaction. And add a strong electrolyte that produces one of the ions on the Right side of the equilibrium reaction, then the reaction will be driven LEFT
Will you get precipitation is Q > Ksp ?
Q > Ksp = have precipitation Q < Ksp = NO precipitation