Question

Ionic Equations.
Na2CO3+AgNO3 --> NaNO3 + Ag2Co3
B: Separate Aqueous solutions, remove spectator ions.
C: Net Ionic Equation.

Answer 1

For B, I got
2Na + CO3(2-) +AG(+) + NO3(-) -->Na(+) + NO3(-) + Ag2CO3
C was
CO3(2-) +Ag(+) --> Ag2CO3.
Do you know if these are right?

Answer 2

Silver carbonate is your insoluble precipitate.\[2Na _{}^{+} + CO _{3}^{2-} + 2Ag _{}^{+} + 2NO _{3}^{-} \rightarrow 2Na _{}^{+} + 2NO _{3}^{-} + Ag _{2}^{}CO _{3}^{} (s)\]
Cancel out the spectator ions \[CO _{3}^{2-} + 2Ag _{}^{+} \rightarrow Ag _{2}^{}CO _{3}^{} (s)\]

Answer 3

Why does the Ag on the left have a two in front of it? I noticed this in class, but I could never figure out why.

Answer 4

So the equation could be balanced, in your equation the # of Ag's on the reactant side does not equal the product side.

Answer 5

I get it. In my class, we do the balancing at the end, during the NET phase.
Our teacher saw no reason to balance ahead of time, if some may just be canceled out as spectator ions.

Answer 6

Thanks for the help. Up for some more? I've got seven left. Seven very painful, very chemical, very annoying problems.

Answer 7

Sure, but I won't be solving them, I'll tell you what to do if you get stuck :P

Answer 8

CURSES. My ultimate plan, foiled. You and your stupid dog.
The next one I have is Pb(NO3)2 +Na2CO3.

Answer 9

Its pretty much like the last one, but your insoluble precipitate is Phosphorous Carbonate this time.

Answer 10

Oops, lead carbonate

Answer 11

Roger. Give me some time.
Like.... an hour. Chemistry is my hardest subject.

Answer 12

ಠ_ಠ

Answer 13

Are you take college chemistry or AP chem in high school?

Answer 14

Chem in high school.
It's a cool class and the teacher is awesome, but its so hard. DX
Our teacher likes setting things on fire. :)

Answer 15

Sounds fun, last year for ap chem, we had the boring teacher :(

Answer 16

Ouch. I'd hate that. Our teacher makes it enjoyable. Mostly because she acquaints everything with a Metaphor. One of the most memorable ones was selling and buying babies, as electrons.

Answer 17

Wait a minute. How did you get Phosphorous Carbonate?
My results were
PbCO3 + NaNO3
Did you mean Lead Carbonate?

Answer 18

Or lead something?

Answer 19

*DERP*
Just read below it.

Answer 20

K. Results were
Pb(NO3)2 + Na2CO3 --> PbCO3 + Na(NO3)

Answer 21

The precipitate is confusing me most. I don't know if I got it right. o.o

Answer 22

Yeah, that seems right, then just separate them into the ions and cancel. The precipitate is the compound that remains a solid dissolved in the aqueous solution; it does not ionize.

Answer 23

Got it. Step A is the hardest to me. Separating & finding NET are much easier. :)

Answer 24

By the way - What's the charge on lead? It's between the negatives and the positives.
Confused.

Answer 25

2+ in this situation.

Answer 26

Thank you. I knew it was either 2+ or 4+.

Answer 27

I've got it all set out, what would it be as Balanced? Mine reads:
2 (NO3)2 + Na2 --> 2 Na(NO3)
I'm just wondering if my balancing at the end is interfering with anything.

Answer 28

:O Na(NO3) ? thats a spectator.

Answer 29

Pb(NO3)2 + Na2CO3 --> PbCO3 + Na(NO3)
Pb2+ + CO3 2- --> PbCO3

Answer 30

I SEE IT. I MESSED UP.
I switched the Na(NO3) and the Lead Carbonate.
:D At least it was minor.

Answer 31

Mkay. The adjustments made me right. Thanks for that. ಠ_ಠ

Answer 32

The next one is
Pb(NO3)2 + Na3PO4 --> PbPO4 + Na(NO3)2.
Is that right for the first step?

Answer 33

Your products don't have the right formulas. Lead phosphate is Pb3PO4. Sodium nitrate is NaNO3.

Answer 34

Why does the 2 after Sodium Nitrate go away?
I see how I messed up the other one.

Answer 35

NEVERMIND. I see it. Thanks again. :)

Answer 36

:o Is the charge on lead still 2+, or 4+ this time? ;o

Answer 37

ಠ_ಠ Stupid question. Nevermind.

Answer 38

Look at the reactant, Pb(NO3)2. When criss crossed charge is +2.

Answer 39

:) I noticed. Thank you~ :D
I need to look more before asking questions. :<

Answer 40

Which one was the precip? :O Lead Phosphate?

Answer 41

Mhm. Use page 2 on this PDF to determine which one is the precipitate. The insoluble compounds are the precipitates.
http://www.p12.nysed.gov/apda/reftable/chemistry-rt/chemrt-2011.pdf

Answer 42

:O Thank you. I feel comfortable with these enough to try them on my own.
You've been a great help. :D Thanks~!

Answer 43

Alright, no problem, good luck :)