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Valesia S.

asked • 08/11/19

Calculate the concentrations of each ion remaining in solution after the precipitation is complete.

The precipitation reaction involves 75.0 mL of .0750 M solution of potassium phosphate and 75.0 mL of .0750 M iron (II) acetate.


I'm very confused as to how to find the concentration of the remaining solutions, particularly because I am not sure if I am supposed to regard the coefficients that are in the balanced equation (for example, when i balanced the equation, i got 6 KC2H3O2 on the side of the products, and those are technically the only ions remaining in solution but i don't know whether i should say that there are 6 K+ ions or what....i am extremely confused.) I would appreciate a clear, helpful answer!

2 Answers By Expert Tutors

By:

Valesia S.

Thank you, this was very helpful!
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08/13/19

Valesia S.

I'm still a little confused... when the question asks for the concentration of "each ion", I was thinking that meant K+ ions and acetate ions. Is the question not asking for specific ions?
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08/12/19

Jim L.

tutor
Since the K ions and the acetate ions are the came valence they each have the same number of ions, sothe concentration of each is the same
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08/12/19

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