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!

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)

Of course! I'll guide you through the steps to solve this chemical equilibrium problem.

Step 1: Write the balanced equations
Start by writing the balanced equations for the given reactions:
a. PbCl2 ⇌ Pb2+ + 2Cl-
b. AgCl ⇌ Ag+ + Cl-

Step 2: Write the expression for the equilibrium constant
For each reaction, write the expression for the equilibrium constant (K) using the concentrations of the products and reactants. Remember, solids (like PbCl2, AgCl) are not included in the expression because their concentrations remain constant:
a. K1 = [Pb2+][Cl-]^2 / [PbCl2]
b. K2 = [Ag+][Cl-] / [AgCl]

Step 3: Determine the desired equilibrium constant
To find the equilibrium constant (Kfinal) for the overall reaction, we need to multiply the equilibrium constants of the individual reactions. The balanced equation for the desired reaction is:
PbCl2 + 2Ag+ ⇌ 2AgCl + Pb2+

So, K(final) = K1 × K2.

Step 4: Substitute the given values
Now, substitute the given values of K1 and K2 into the equation for K(final):
K(final) = (1.76 x 10^(-10)) × (1.11 x 10^(-4))

Step 5: Calculate the final equilibrium constant, K(final)
Multiply the values inside the parentheses and calculate the product:
K(final) = 1.9536 x 10^(-14)

Therefore, the equilibrium constant for the reaction PbCl2 + 2Ag+ ⇌ 2AgCl + Pb2+ is approximately 1.9536 x 10^(-14).

Remember, in each step, it is essential to consider the units used for the equilibrium constants and concentrations. Additionally, always double-check the accuracy of the values used in the equations to ensure correct calculations.

I hope this step-by-step guide helps you understand how to solve chemical equilibrium problems! Let me know if you have any further questions.