Chem Equilibrium

K < 1

favors reactants - lies to the left

K > 1

favors products - lies to the right

Large K value

favors products

small K value

favors reactants

K > Q

not at eq yet, reaction moves right towards products

K < Q

Past Eq, reaction moves left towards reactants

K = Q

reaction is at equilibrium

why does temp affect K

temperature changes affect the rates of the forward and reverse reactions

Le Chatelier's principle

If you stress a reaction at eq, the system will shift in a direction to relieve that stress

4 types of stress:

concentration, pressure, temperature, and addition/removal of reactants/products

where does heat go in an exothermic reaction and what is its effect on eq when temp is raised

in the products - shifts left (reactants)

where does heat go in an endothermic reaction and what is its effect on eq when temp is raised

in the reactants - shifts right (products)

Qsp<𝐾𝑠𝑝

The solution is unsaturated. More ionic solid can dissolve into the solution, and no precipitate will form. 

Qsp=Ksp

The solution is saturated and at equilibrium. The rate of dissolution equals the rate of precipitation. 

Qsp>Ksp

The solution is saturated and at equilibrium. The rate of dissolution equals the rate of precipitation. 

ammonium

NH4+

carbonate

CO3 2-

hydroxide

OH-

Iodate

IO3-

Nitrate

NH3-

sulfate

SO4 2-