We are being asked to determine whether a precipitate will form when you add 69.4 mL of a 0.447 AgNO3 solution to solution to 119.5 mL of a 0.128 M NaCl solution
We will do the following steps:
Step1: Write the net ionic equation
Step 2: Calculate initial concentrations
Step 3: Calculate Q
Step 4: Compare Q and K
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
You add 69.4 mL of a 0.447 AgNO3 solution to 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 precipitation will form, because Q < K
C) A precipitation will not form, because Q > K
D) A precipitation will not form, because Q < K
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the The Reaction Quotient concept. You can view video lessons to learn The Reaction Quotient. Or if you need more The Reaction Quotient practice, you can also practice The Reaction Quotient practice problems.