Determine the value of the equilibrium constant (report your answer to three sig

Question

Determine the value of the equilibrium constant (report your answer to three significant figures) for the following reaction if an equilibrium mixture contains 0.010 mol of solid PbF2, and is 0.0100 M in Pb2+ ions and 0.00190 M in F1- ions. Use the notation 4.31e-5 to indicate a number such as 4.31 x 10-5.

I used K = (0.01 * 0.0019^2) / 0.01 = 3.61e-6, but it tells me I'm wrong, and I can't figure out why.

PbF2(s) Pb2+(aq) + 2F1-(aq) K = Determine the value of the equilibrium constant (report your answer to three significant figures) for the following reaction if an equilibrium mixture contains 0.010 mol of solid PbF2, and is 0.0100 M in Pb2+ ions and 0.00190 M in F1- ions. Use the notation 4.31e-5 to indicate a number such as 4.31 times 10-5.

Explanation / Answer

PbF2(s) <=> Pb2+(aq) + 2 F-(aq)

K = [Pb2+][F-]^2

= 0.0100 x 0.00190^2

= 3.61 x 10^(-8) (or 3.61e-8)


(Note that you do not include any terms for solid PbF2 in the K expression)

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