Problem: 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 > KB. A precipitate will form, because Q < KC. A precipitate will not form, because Q > KD. A precipitate will not form, because Q < KPart 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 belowPart 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.

FREE Expert Solution

Part 2.

Recall the formula for Q is:

Q = productsreactants

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


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Problem Details

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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Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.