Solutions of potassium carbonate, copper(II) chloride, and lead(II) nitrate are each added to a beaker. Will any compound(s) precipitate from solution? Write a balanced net ionic equation for any precipitation reaction that occurs.

Question

I have gotten this so far:
K2CO3(aq) + CuCl2(aq) + Pb(NO3)2(aq) -> ?
But I am not sure how to complete the equation with 3 reactants.

Answer 1

Remember that reactions occur for one of a few reasons.
1. a ppt is formed
2. a gas is formed
3. a slightly ionized substance is formed.
This problem requires that you know the solubility of compounds. Here is a site that gives a simplified set of solubility rules.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html

Therefore you see that PbCO3 is insoluble which means we can write
K2CO3 + Pb(NO3)2 ==> 2KNO3 + PbCO3(s)
Now you need to turn that into a net ionic equation to answer that part of the question.
This is not the only reaction. Can you find the other one?

Answer 2

So when solving this equation, we only use two of the reactants and not all three?

And since there is more than one reaction, do we use the net ionic equations of both as the answer for this question or just one equation?

So would the other reaction be this:
CuCl2(aq) + Pb(NO3)2(aq) --> Cu(NO3)2(aq) + PbCl2(s)

Answer 3

Yes that is another reaction. There is a third one with the formation of CuCO3(s),
And yes you write three net ionic equations.
Pb^2+(aq) + 2Cl^-(aq) ==> PbCl2(s) is one of them.
Pb^2+(aq) + CO3^2-(aq) ==> PbCO3(s) is another one.
Then Cu^2+(aq) + CO3^2-(aq) ==> CuCO3(s) is the third one.

Answer 4

Thank you so much!

Answer 5

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