Net Ionic Equations: NaCl + AgNO3 Reaction

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The discussion centers on determining the net ionic equation for the reaction between aqueous sodium chloride (NaCl) and aqueous silver nitrate (AgNO3). Participants clarify that NaCl dissociates into Na+ and Cl- ions, while AgNO3 dissociates into Ag+ and NO3- ions. The key reaction involves the formation of solid silver chloride (AgCl) as a precipitate, while sodium nitrate (NaNO3) remains in solution as spectator ions. The correct net ionic equation is Ag+(aq) + Cl-(aq) → AgCl(s). Understanding the solubility rules is crucial for identifying the precipitate and writing the net ionic equation accurately.
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Homework Statement


So the question is:

Enter the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate.


Homework Equations


So i know that the first part of the equation is:
Na(ClO2)aq+Ag(NO3)aq --> i have no clue what should go here.
Please help

The Attempt at a Solution


and i don't ebern know how to attempt this problem... i tried:
Ag(aq) --> (ClO2)s
because this is what would change but it is saying it is not right.
 
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NaClO2 is not sodium chloride.

Start writing both compounds in ionic form, the way they dissociate in the solution. Don't ignore charges.

--
 
Borek said:
NaClO2 is not sodium chloride.

Start writing both compounds in ionic form, the way they dissociate in the solution. Don't ignore charges.

--
www.titrations.info, www.chemistry-quizzes.info, www.ph-meter.info

OH WAIT! Sodium Chloride is just NaCl.

So it would be:

Na++Cl++Ag+NO3-
 
Close, just add correct charge to Ag.

Do you have any idea what can happen when you mix these salts? Hint: answer lies in the solubility rules.
 
Borek said:
Close, just add correct charge to Ag.

Do you have any idea what can happen when you mix these salts? Hint: answer lies in the solubility rules.

The Charge on Ag is a + right but my professor said something about in the Net ionic equation how all the reactents are not in it. so i was wondering how i would write the end equation... would it be:

Ag+(aq) --> Cl-(s) or something like that..
 
Try to answer my question: what will happen in the solution?

--
 
Borek said:
Try to answer my question: what will happen in the solution?

--
www.titrations.info, www.chemistry-quizzes.info, www.ph-meter.info

the soluble ployatomic ion NO3 would attach to the Na and the Ag would attach to the Cl and the AgCl would become a solid while the Na(NO3) would still be aq... right?
 
Yes and no. You are right about AgCl precipitating from the solution and becoming solid, you are wrong about NO3- attaching to Na+ - they will just float in the solution, they aren't called spectators without a reason.

Now you should be able to write full ionic equation and cancel out spectators.
 

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