Question

Did increasing the starting concentration of Ca2+ in part II of this experiment increase or decrease the amount of Ca(IO3)2 that dissolved. Explain your answer using the concepts of LeChatelier’s Principle.

Answer 1

First, let us state the Le Chatelier principle which deals with changes in an equilibrium:

The statement is as follows:

If any equilibrium is disturbed, that is, change in conditions such as P,T, concentration, partial pressure, etc.., the system will counterbalance such change in order to favour the system's equilbirium.

• Change in concentration
• Change in pressure
• Change in temperature

Ca(IO3)2 <--> Ca2+ + 2IO3-

Ksp = [Ca2+][IO3-]^2

then...

if we increase Ca2+, this will NOT favour solubility, since the shift goes towards solid Ca(IO3)2

then, this will decrease amount of Ca(IO3)2 dissolved initially