smaerd
International Hazard
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Registered: 23-1-2010
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Mood: hmm...
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Net Ionic Equation - little help please
I have some basic questions. My text book is no help. I understand the concept, at least I think I do, could someone check this one problem for me and
make sure I've got the right idea.
Say the problem is this:
Write the ionic and net ionic equation for the following reaction:
Mg(NO3)2(aq) + 2NaOH(aq) ->
Here's what I have:
For the standard balanced equation.
Mg(NO3)2(aq) + 2NaOH(aq) -> Mg(OH)2(aq) + 2Na(NO3)(s)
Now for ionic equation. Here's where I am getting a little hung up. So the subscripts of the polyatomic ions such as Nitrates, say I have 2 Nitrates
on the Magnesium Nitrate. Do I move the subscript to become a coefficient or leave it as a subscript? Did I do this right?
Mg(+2) + 2(NO3)(-1) + 2Na(+1) + 2(OH)(-1) -> 2Na(+1) + 2(NO3)(-1) + Mg(OH)2(s)
Then here is what I have for the net ionic equation. So for the net ionic equation I remove all of the spectator ions pertaining to the reaction(Ions
not being used directly for the reaction). In this case a metathesis precipitate reaction.
So even though the Nitrate, is bouncing from the magnesium and being replaced by a Hydroxide it is considered a spectator ion right?
Mg(+2) + 2(OH)(-1) -> Mg(OH)2
Thanks for any help. I hope I didn't type to much I was just trying to be clear as to where I am stuck.
[Edited on 29-9-2010 by smaerd]
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crazyboy
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You need to add a coefficient of 2 to the nitrate anion because as it is now the ionic equation is not balanced.
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smaerd
International Hazard
Posts: 1262
Registered: 23-1-2010
Member Is Offline
Mood: hmm...
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Oh right I just forgot to type that I have it down on paper, thank you . I fixed
that now. Does it look okay otherwise?
[Edited on 29-9-2010 by smaerd]
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