Because calcium carbonate is a sink for CO 3 2 in a lake, the student in Exercise

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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:

Ca+ (aq) + CO3- (aq) = CaCO3(s)


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:

HCO3(aq) H*(aq) + HCO3(aq) K = 4.4 x 10-7


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

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Chemistry For Engineering Students

ISBN: 9780357026991

4th Edition

Authors: Lawrence S. Brown, Tom Holme

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