[browneyedbella]

So my professor gave out a sheet of net ionic equations to do. And needless to say I'm pretty lost. what I have typed under the number is as far as i get!!! PLEASE HELP. seriously, anything would be great.

Write balanced net ionic equations for any of the reactions that occur when aqueous solutions of the following compounds are mixed. If there is no reaction, give NR. Also - tell what type of reaction is occurring: precipitation, acid (base or oxidation-reduction)

1. chromium metal and hydroiodic acid.
I'm pretty sure this one has NR.

2. barium bromide and potassium chromate.

BaBr₂ + K₂CrO₄

3. magnesium hydroxide and nitrous acid.
Mg(OH)₂ + HNO₂

4. cobalt sulfate and lithium sulfide.
CoSO₄^2- + Li₂S

5. mercury (II) nitrate and ammonium iodide.
Hg(NO₃)₂ + NH₄I

6. silver acetate and aluminum sulfate.
AgC₂H₃O₂ + Al₂(SO₄)₃

7. nickel (II) bromide and potassium phosphate.
__________ + KH₂PO₄

8. calcium carbonate and nitric acid
CaCO3 + HNO₃

9. sodium hydroxide and copper (II) sulfate
NaOH + Cu(SO)₄

10. calcium chloride and cadmium metal
CaCl₂ + _______

11. ammonia and perbromic acid.
NH₃ + HBrO₄

12. mercury metal and lead nitrate.
Hg + Pb(NO₃)₂

13. zinc sulfite and sulfuric acid.
______ + H₂SO₄

14. magnesium metal and tin (IV) chloride.
Mg²⁺ + SnCl₄

[AWK]

Read forum rules and show your attempt.

Ammonia and metallic cadmium are neutral species not ionic.
Note - perbromic acid is extremely unstable and will decompose into water, bromine and oxygen before reaction with a weak base.

[nj_bartel]

Note - perbromic acid is extremely unstable and will decompose into water, bromine and oxygen before reaction with a weak base.

I don't think he needs to know that, does he?  Just going to complicate it.

[browneyedbella]

Hello. I don't mean to be rude here, but the above was my attempt. My professor only gave us the names of each solution. Maybe it'd be helpful if I knew what the solubility rules did? Maybe then I could post an attempt to answering them?

Again, this isn't meant to be rude. I just really don't understand this. Sorry.

[nj_bartel]

--------------------------------------------------------------------------------
 http://en.wikipedia.org/wiki/Precipitation_(chemistry)
 http://en.wikipedia.org/wiki/Single_displacement_reaction
 http://en.wikipedia.org/wiki/Metathesis_reaction_(chemistry)
 http://www.csudh.edu/oliver/chemdata/solrules.htm
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--------------------------------------------------------------------------------
 http://en.wikipedia.org/wiki/Neutralization_(chemistry)
 http://en.wikipedia.org/wiki/Acid
 http://en.wikipedia.org/wiki/Base_(chemistry)
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 http://en.wikipedia.org/wiki/Redox
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Read those pages and try to understand the gist of them.  If there's something you don't understand in one of them, ask a specific question about it.

[browneyedbella]

just to see if I'm getting the hang of things...

cobalt sulfate and lithium sulfide

Co⁸⁺+SO₄^2- + Li⁺+S^2-
CoSO₄^2- + Li₂S  Li₂S




barium bromide and potassium chromate
Ba²⁺Br + K⁺Cr⁶⁺O₄^2-
BaBr₂ + K₂CrO₄  BaK + CrO₄



magnesium hydroxide and nitrous acid
3 Mg(OH)₂ + 2 HNO₃  MgH + OH₂


??

[browneyedbella]

please see original post for my answers.

corrections would be great.

also. i included the kind of reaction at the bottom. if its wrong, please correct and/or tell me why?

thanks so much!

[browneyedbella]

So my professor gave out a sheet of net ionic equations to do. And needless to say I'm pretty lost. what I have typed under the number is as far as i get!!! PLEASE HELP. seriously, anything would be great.

Write balanced net ionic equations for any of the reactions that occur when aqueous solutions of the following compounds are mixed. If there is no reaction, give NR. Also - tell what type of reaction is occurring: precipitation, acid (base or oxidation-reduction)

1. chromium metal and hydroiodic acid.
I'm pretty sure this one has NR.

2. barium bromide and potassium chromate.
BaBr₂ + K₂CrO₄ BaK + CrO₄

3. magnesium hydroxide and nitrous acid.
Mg(OH)₂ + HNO₂  MgH + OH₂
precipitation

4. cobalt sulfate and lithium sulfide.
CoSO₄^2- + Li₂S  Li₂S

5. mercury (II) nitrate and ammonium iodide.
Hg(NO₃)₂ + NH₄I  Hg₂I

6. silver acetate and aluminum sulfate.
AgC₂H₃O₂ + Al₂(SO₄)₃  AgAl₂

7. nickel (II) bromide and potassium phosphate.
NiBr + KH₂PO₄  NiH₂ + KPO₄

8. calcium carbonate and nitric acid
CaCO₃ + HNO₃  CaCO₃ + H

9. sodium hydroxide and copper (II) sulfate
NaOH + Cu(SO)₄    NR

10. calcium chloride and cadmium metal
CaCl₂ + Cd  CaCd
precipitation

11. ammonia and perbromic acid.
NH₃ + HBrO₄  NH₄ + BrO₄
oxidation reduction

12. mercury metal and lead nitrate.
Hg + Pb(NO₃)₂  HgPb₂
precipitation

13. zinc sulfite and sulfuric acid.
ZnSO₂ + H₂SO₄  H₂O + ZnSO₄
acid base reaction

14. magnesium metal and tin (IV) chloride.
Mg²⁺ + SnCl₄  Mg₄Cl₂ + Sn



NOTE: I'm not sure if they are all balanced. And I'm not sure what state they are in (Aq, liq, gas). If you catch any mistake (which there are probably alot) please *delete me*

Again, I'm not good at this at all. Any help would be great!

[Borek]

1. chromium metal and hydroiodic acid.
I'm pretty sure this one has NR.

Metal in very strong acid.

2. barium bromide and potassium chromate.
BaBr₂ + K₂CrO₄ BaK + CrO₄

You are mixing two salts. Check solubility of barium chromate. Besides, you can't combine any ion with any ion - ionic salts have a cation and an anion, not two cations. And where is bromide on the right?

3. magnesium hydroxide and nitrous acid.
Mg(OH)₂ + HNO₂  MgH + OH₂
precipitation

Again, you are combining wrong ions. You have a base and an acid.

4. cobalt sulfate and lithium sulfide.
CoSO₄^2- + Li₂S  Li₂S

Half of your reactants disappeared. Check solubility rules.

You repeat similar mistakes now and again, so analyze these and redo the rest.

[AWK]

just to see if I'm getting the hang of things...

cobalt sulfate and lithium sulfide

Co⁸⁺+SO₄^2- + Li⁺+S^2-
CoSO₄^2- + Li₂S  Li₂S




barium bromide and potassium chromate
Ba²⁺Br + K⁺Cr⁶⁺O₄^2-
BaBr₂ + K₂CrO₄  BaK + CrO₄



magnesium hydroxide and nitrous acid
3 Mg(OH)₂ + 2 HNO₃  MgH + OH₂


??

write down like this
Co²⁺(aq) + S^2-(aq) = CoS(s)