Understanding Net Ionic Equations for MgCl2 + Cu(NO3)2

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The discussion centers on the lack of a reaction between MgCl2 and Cu(NO3)2, with participants clarifying that both nitrate and chloride ions are soluble, leading to no precipitate formation. It is emphasized that solubility pertains to salts rather than individual ions, correcting the misconception about stating ions as soluble. The net ionic equation is not applicable here because no reaction occurs. Participants suggest that searching for examples online may not yield results due to the absence of a reaction. Overall, the key takeaway is that no net ionic equation exists for this combination.
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MgCl2 + Cu(NO3)2

I need the full and net ionic equations for this.

I know NO3 is soluble and Cl is soluble too since there's no Ag, Pb, or Hg. Not sure how to write them out though.
 
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MG5 said:
MgCl2 + Cu(NO3)2
You can often find a worked example if you paste that without formatting into google.
 
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NascentOxygen said:
You can often find a worked example if you paste that without formatting into google.

Tried but couldn't find it
 
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Not without a reason - there will be no reaction.

Note: your statement

I know NO3 is soluble and Cl is soluble too since there's no Ag, Pb, or Hg.

doesn't make much sense. Solubility is a property of a SALT, not of a single ion. So you can state "Cl- will not precipitate out of the solution, as there is no cation that will create insoluble salt with it", but you can't state "Cl- is soluble" as it doesn't mean anything - you can't have flask with isolated Cl-.
 
Borek said:
Not without a reason - there will be no reaction.

Note: your statement



doesn't make much sense. Solubility is a property of a SALT, not of a single ion. So you can state "Cl- will not precipitate out of the solution, as there is no cation that will create insoluble salt with it", but you can't state "Cl- is soluble" as it doesn't mean anything - you can't have flask with isolated Cl-.

Oh. I was just looking at solubility rules in my book.
 

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