[kauzs-17]

Hello,

I'm given Na₂CO₃ (aq) + AgNO₃ (aq)
Dissolved in .400L of water
I get Na⁺ + Na⁺ + CO₃^2- + Ag⁺ + NO₃^-

But I can't seem to form a precipitate with this. I feel as though I should because another problem gives the g amount of the reactants and asks which is limiting.

[Arkcon]

You will have to look up the general solubility rules.  There is most definitely a precipitate.

[kauzs-17]

Solubility Rules given to me from my teacher (Straight from Powerpoint).

Some compounds always dissociate (break up) in solution.
•   Any anion with an alkali metal (first column) or NH4+
•   Any metal with: NO3-, HCO3-, and ClO3-.
Some compounds never dissociate:
•   Halides with Ag+, Hg2+, and Pb2+
•   Sulfates with Ag+, Cd2+, Sr2+, or Pb2+
•   Metals with CO32-, PO43-, CrO42-, or S2-, unless they are akali metals.
•   Metals with OH-, unless they are alkali metals.
Na⁺ is an alkali metal so it's out.
That leaves CO₃^2-, NO₃^- and Ag⁺.
NO₃^- dissociates with all metals, plus AgNO₃ is a reactant. That's out.
And there is only one Ag⁺ so there's no other option.

Is there something I'm missing?

[AWK]

Is there something I'm missing?

I'm given Na₂CO₃ (aq) + AgNO₃ (aq)

[kauzs-17]

Is there something I'm missing?

I'm given Na₂CO₃ (aq) + AgNO₃ (aq)

Yes... I'm sorry I'm just not wrapping my head around this..

[DrCMS]

Na+ is an alkali metal so it's out.
That leaves CO₃^2-, NO₃^- and Ag⁺.
NO₃^- dissociates with all metals, plus AgNO₃ is a reactant. That's out.
And there is only one Ag⁺ so there's no other option.

Is there something I'm missing?

Look again you have 4 ions and you've only ruled out only 2 of them

[kauzs-17]

Alright, so to clarify, I get
Na⁺ + Na⁺ + CO₃^2-- + Ag⁺ + NO₃^-?
Right?

[kauzs-17]

Wait...
You can't form a precipitate with an overall - charge, can you?
Such as AgCO₃^-?

[Borek]

They don't have have to react 1:1.

Do you know what is the formula of silver carbonate? Were you perhaps taught how to write formula of such compound? You already seem to know that salt molecule should be neutral - and the silver carbonate is made of Ag⁺ and CO₃^2- - how can you combine them to produce a neutral molecule?

[kauzs-17]

Ag₂CO₃.
Since I only have a +1 charge and -2 charge, could it be Ag(CO₃)_.50? Is that even possible?

I know when I did a stoichiometry problem for the empirical formula of Methane I got C_.25H₁ which would be CH₄. Is this a similar deal?

[Borek]

Ag₂CO₃.

Correct.

Since I only have a +1 charge and -2 charge, could it be Ag(CO₃)_.50? Is that even possible?

No, it is not possible and it is not necessary. You already wrote correct formula of the salt above. As I told you earlier, sodium carbonate and silver nitrate don't react 1:1. See for yourself - try to balance this reaction equation:

Na₂CO₃ + AgNO₃ Ag₂CO₃ + NaNO₃

It is obvious that you have some misconception about how these things work, I just can't pinpoint it yet.

[Vidya]

Formulas are not decided by the amount of the ions present in the solution.The compounds combine in a fixed ratio.So here 2 moles Ag+ will combine with 1 mole of CO32-
so the precipitates are of
2Ag+ + CO32-----> Ag2CO3(s)
only IA group and NH4+ carbonates are soluble and rest all are insoluble.