[brocasbrain00]

A student added 1 liter of 1M Na2SO4 solution to 1 liter 1M silver acetate solution. A silver sulfate precipitate formed and nearly all of the silver ions disappeared from the solution. Which of the following lists the ions remaining in solution in order of decreasing concentration:

A)     SO4 > C2H3O2 > Na
B)     C2H3O2 > Na > SO4
C)     C2H3O2 > SO4 > Na
D)     Na > SO4> C2H3O2
E)     Na> C2H3O2 > SO4


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That's all thats given in the problem.

The balanced equation I wrote (I think its correct) is

Na2SO4 + 2Ag(C2H3O2) ----->  Ag2SO4 + 2Na(C2H3O2)

Can anyone tell me how to solve this?? I keep getting that there are the same amount of sodium and acetate ions in the solution...      Please

[SirPants]

You should try to balance the equation first to check out the ratio between sodium ions and acetate ions

[Padfoot]

brocasbrain00 - You are forgetting the limiting reagent.

[AWK]

Reaction is balanced correctly. Calculate moles of reagents in solution as a first step

[Borek]

How many Na⁺ per 1 molecule of Na₂SO₄?

[Padfoot]

The acetate ion concentration will be greater than that of the soduim ion.

[Borek]

The acetate ion concentration will be greater than that of the soduim ion.

No. How much of both ions do you put in the solution? Are they used in the reaction, or are they only spectators?

Please note that you are hijacking brocasbrain00 thread.