Recall the formula for Q is:
Depending on if Q is greater than or less than K, our reaction will shift to attain equilibrium by reaching the equilibrium constant K:
If Q = K → the reaction is at equilibrium
If Q < K → the reaction shifts in the forward direction to reach equilibrium
If Q > K → the reaction shifts in the reverse direction to reach equilibrium
We will do the following steps
Step 1: Write the reaction
Step 2: Calculate initial concentration
Step 3: Calculate Q
Step 4: Compare Q and K
Part 2: You add 69.3 mL of a 0.447 M AgNO3 solution to 119.5 mL of a 0.128 M NaCl solution. Determine the concentration of Ag+ and Cl- ions in solution as if all remain dissolved. After, use your Ksp expression to determine if a precipitate will form. Which of the following represents what will occur and why?
A. A precipitate will form, because Q > K
B. A precipitate will form, because Q < K
C. A precipitate will not form, because Q > K
D. A precipitate will not form, because Q < K
Part 3. Create an ICE table for the formation of AgCl. React the two ions completely, and then determine which ions is the limiting reagent. Finally, determine the concentration (in molarity) of the ion remaining, and enter the value below
Part 4. Finally, create another ICE table for the dissolution of AgCl. Use the concentration from part 3 for the initial concentration of ion remaining in part 4 and 0.000 M for the initial concentration of the other ion. Finally, calculate the equilibrium concentration for both ions. Enter the concentration of the ion that was the limiting reagent in part 4 below.
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