Because calcium carbonate is a sink for CO₃ ^2– in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCO₃. The reaction is:

The equilibrium constant for this reaction is 2.1 × 10⁸. If the initial calcium ion concentration is 0.02 M and the carbonate concentration is 0.03 M, what are the equilibrium concentrations of the ions?

Data from exercise 12.39

A student is simulating the carbonic acid–hydrogen carbonate equilibrium in a lake:

She starts with 0.1000 M carbonic acid. What are the concentrations of all species at equilibrium?

Transcribed Image Text:

Ca²+ (aq) + CO3²- (aq) = CaCO3(s)