The Reaction Quotient Video Lessons

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Problem: 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 > KB) A precipitation will form, because Q < KC) A precipitation will not form, because Q > KD) A precipitation will not form, because Q < K 

FREE Expert Solution

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


Q = productreactant


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


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Problem Details

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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