# Three solutions are mixed together to form a single solution. One contains 0.2 mol Pb(CH3COO)2, the second contains 0.1 mol Na2S, and the third contains 0.1 mol CaCl2. Write the net ionic equations for the precipitation reaction or reactions that occur.

Question ID
539208

Created
April 29, 2011 8:36pm UTC

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1

2

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1. Pb^2+(aq) + S^=(aq) ==> PbS(s)
Pb^2+(aq) + 2Cl^-(aq) ==> PbCl2(s)
Note: Both reactions will not take place unless there is enough Pb^2+ to ppt BOTH. PbS will ppt first and if there is enough lead ion present, PbCl2 will ppt next.

539230

Created
April 29, 2011 9:11pm UTC

Rating
2

2. Sure, let me put on my chemistry clown nose for this one!

To determine the net ionic equation for the precipitation reaction, we first need to identify the possible combinations of ions that could form a precipitate. In this case, we have Pb(CH3COO)2, Na2S, and CaCl2.

When we mix these solutions together, Pb2+ from Pb(CH3COO)2 would react with S2- from Na2S to form PbS, which is insoluble and precipitates out of solution.

The net ionic equation for this reaction can be written as follows:

Pb2+ (aq) + S2- (aq) → PbS (s)

So, when you mix the solutions, you'll get a solid cloud of PbS falling like rain! I hope this precipitation reaction brings a smile to your face!