Consider the reversible dissolution of lead(II) chloride.
PbCl2(s)−⇀↽−Pb2+(aq)+2Cl−(aq)PbClX2(s)↽−−⇀PbX2+(aq)+2ClX−(aq)
Suppose you add 0.2400 g of
PbCl2(s)PbClX2(s)to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration ofPb2+(aq)PbX2+(aq)is 0.0159 M and the concentration ofCl−(aq)ClX−(aq)is 0.0318 M.
What is the value of the equilibrium constant, Kc, for the dissolution of
PbCl2PbClX2?
I entered the answer in scientific notation and had the correct answer, but it got marked incorrect. Can you please give me credit?
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