# Chemistry

Hi! I need help with the step by step procedure for chemical equilibrium problems. Here is an example:

Given two reactions:
a. PbCl2 <---> Pb^(2+) + 2Cl^(-)
K = 1.76*10^(-10)
b. AgCl <---> Ag^(+) + Cl^(-)
K = 1.11*10^(-4)
What is the equilibrium constanct K(final) for the following reaction?

PbCl2 + 2 Ag^(+) <---> 2AgCl + Pb^(2+)

Would you please take me step by step so i can fully understand this process and can apply it to other examples? Thanks!

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1. First, take a look at what you typed. I'm almost certain that you reversed the constants; i.e., the AgCl should be the 10^-10 and the PbCl2 should be the 10^-4.

Here is what you do.
Write equation 1 as is. That K we will call K1.
Multiply equation 2 by 2 (the new k2 will be K^2), then reverse it and K for the reversed reaction will be 1/K^2.
Now add the two equations together (equation 1 + reversed (2*equation 2). Cancel ions, substances common to both sides and you will get the equation you want. To find K for the new reaction, simply multiply the original K1 and the reversed K2 (which is now 1/K^2). I think the final answer will be K1/(K2^2)

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