Balancing acid equation-net ionic equation

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Discussion Overview

The discussion revolves around the process of writing net ionic equations for reactions involving sodium chloride (NaCl), nitric acid (HNO3), silver nitrate (AgNO3), and ammonia (NH3). Participants explore the formation of products, the role of spectator ions, and the complexities of balancing the equations.

Discussion Character

  • Homework-related
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant expresses confusion about how to derive the net ionic equation from the given reactants and mentions an example equation that includes NO2 as a product.
  • Another participant asserts that Ag+ binds with Cl- and states that there is no gaseous product in the reaction.
  • A participant questions how nitric acid contributes to the formation of H2O and NO2, suggesting that these products are obligatory due to the acid.
  • Discussion includes the identification of spectator ions, with participants noting that Na+ and NO3- do not change during the reaction.
  • There is a challenge regarding the conversion of two NO3- ions into one NO2-, with one participant stating that this does not happen and that the information about NO2 being a product is incorrect.
  • Participants discuss the need to balance the net ionic equation and whether to include spectator ions in the final representation.
  • One participant successfully writes the net ionic equation for the first reaction as Ag+(aq) + Cl-(aq) → AgCl(s) and expresses gratitude for the assistance received.
  • Further complexity is introduced with the addition of NH3, leading to questions about the reactions that occur when ammonia is added to the mixture.

Areas of Agreement / Disagreement

Participants generally agree on the role of certain ions as spectators and the formation of AgCl. However, there is disagreement regarding the products of the reactions, particularly the presence of NO2, and the complexities introduced by the addition of NH3 remain unresolved.

Contextual Notes

Some participants express uncertainty about the conditions under which certain products form and the implications of the nitric acid in the reactions. The discussion reflects varying levels of understanding and interpretation of the chemical processes involved.

Who May Find This Useful

This discussion may be useful for students learning about net ionic equations, chemical reactions involving acids and bases, and the concept of spectator ions in chemistry.

yosef
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Thread moved from the technical forums, so no HH Template is shown.
I was asked to take NaCl then add HNO3, then add AgNO3, and to write a net ionic equation... then add NH3 to the same mixture and write another net ionic equation. I have been trying between work and everything else to try to do this one. it wasn't well understood in class and now I haven't found any resources to figure it out. I need whatever tips possible to guide me in the correct direction. At least for now I don't know what to do. Someone showed me an answer of Ag(aq)+ + 2H+ + Cl- + NO3----->> AgCl(s) + NO2(g) + H2O. I have tried 3 or four times, but I just have ZERO IDEA how that answer arrives... I know Ag+ binds with Cl- and as far as I know, because of the nitric acid H2O and a salt will be in the product. I am Having a hard time seeing how the NO2 gets in the picture. Thank You in advance for any help.
 
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yosef said:
I know Ag+ binds with Cl-

And that's all you need for the first step.

There is no gaseous product.

Ammonia is known to complex metals.
 
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OK. Thank You. How does the Nitric Acid on the reagent side fit into the 'mix' (no pun intended). I really am trying here. Where am I missing the formation of H2O and NO2? In the attached picture, on the second line
20160322_185929 (1).jpg
, to the right, is where I am getting stuck. (Is it correct to say that 'because of the acid (Nitric in this case), a salt and H2O are OBLIGATORY products'?)
 
Last edited:
Net ionic reaction means - whatever was not changed during reaction is removed from the equation. These removed molecules/ions are called "spectators".

Did the Na+ change? Did the NO3- change during the reaction?
 
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Thank you again. Na+ for sure doesn't change. It is removed. How do the 2 NO3's become 1 NO2-? (Also, how do you input the elevated + and - signs in the text? [this question isn't as important to me as the first])
 
yosef said:
How do the 2 NO3's become 1 NO2-?

It doesn't, there is no reduction taking place. Whoever told you about NO2 being a product was wrong, that's what I told you in my very first post in the thread.

There are buttons for formatting the post, above the edit window (at least if you are using a normal browser).
 
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OK . I am following you. Right now, in the picture, it looks like almost all of them, the Na+, both NO3's, and the H+ as well, do not change in the product side. I just do not think that is correct.
 

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That's perfectly correct, most of the ions present are spectators. Can you write the net ionic equation for the first reaction now?
 
Na+ + Cl¯ + Ag+ + NO3¯ - - - >> AgCl?
 
  • #10
As written, it is not balanced, as Na+ and NO3- are present only on the left side of the equation.

However, do they change during the reaction, or are they spectators? And if they are spectators, do you need to include them at all?
 
  • #11
Ag+(aq) + Cl- (aq) ----->>>> AgCl(s) ?? (Since, as you mentioned, NO2 is not part of the product, this is all i can think of right now). I very much appreciate your patience with me. I see you are in Poland and you seem to have a very good understanding of English too.
 
  • #12
yosef said:
Ag+(aq) + Cl- (aq) ----->>>> AgCl(s)

Yes, that's perfectly correct.

The second one will be a bit more tough, as actually there are two reactions taking place. Each needs a separate equation.
 
  • #13
So it will become AgCl(s) + NH3(aq)+ - - - - > ? :wideeyed:
 
  • #14
No such thing as NH3+(aq).

One reaction will be more or less what you wrote - dissolving precipitate in ammonia.

The other - sample was initially acidified with nitric acid, wasn't it? What do you know about ammonia and acids?
 
  • #15
Thank You again for helping me. I have since gotten that answer. I am learning enthalpy now, and it is going well. I just wanted to convey good wishes to you for your time.
 
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  • #16
I scored a %98! Thank you again for your time and help! I have new questions but first I wanted to share the good news :smile:
 
  • #17
Here is the test.
test.jpg
 

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