Problem: Some idiot dumped 200 g of toxic PbCl2(s) into a swimming pool containing 104 liters of water. Part I: Calculate how much PbCl2(s) remains undissolved at equilibrium. Part II: A chemistry student suggested to add 106 g of NaCl into the pool, to cause more PbCl2 to precipitate. How much PbCl2(s) would be present in the bottom of the pool (ready to be vacuumed up and removed) after this treatment? The molecular masses of PbCl2 and NaCl are 278.1 g/mol and 58.4 g/mol, respectively. Potential answers to Parts I and II (in grams) are... A. 59, greater than 199B. 23; greater than 199C. 7; 46D. 2; 46E. 0; 184

FREE Expert Solution

We’re being asked to calculate for the mass of undissolved PbCl2(s) and how much PbCl2(s) would be present in the bottom of the pool after 106 g NaCl is added.

For this problem, we're going to do the following steps:

Step 1: Construct an ICE chart for the equilibrium reaction of PbCl2.
Step 2: Calculate the solubility of PbCl2.
Step 3: Calculate the mass of undissolved PbCl2.
Step 4: Calculate the concentration of Cl- ions in the solution after the addition of NaCl.
Step 5: Construct an ICE chart and calculate the solubility of PbCl2 after the addition of NaCl.
Step 6: Calculate the amount of precipitated PbCl2.



Step 1: Construct an ICE chart for the equilibrium reaction of PbCl2.

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Problem Details

Some idiot dumped 200 g of toxic PbCl2(s) into a swimming pool containing 104 liters of water. 

Part I: Calculate how much PbCl2(s) remains undissolved at equilibrium. 

Part II: A chemistry student suggested to add 106 g of NaCl into the pool, to cause more PbCl2 to precipitate. How much PbCl2(s) would be present in the bottom of the pool (ready to be vacuumed up and removed) after this treatment? The molecular masses of PbCl2 and NaCl are 278.1 g/mol and 58.4 g/mol, respectively. Potential answers to Parts I and II (in grams) are... 

A. 59, greater than 199

B. 23; greater than 199

C. 7; 46

D. 2; 46

E. 0; 184

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