Redox Reaction in Dissolved Ammonium Chloride

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Discussion Overview

The discussion revolves around whether the dissolution of ammonium chloride (NH4Cl) in water constitutes a redox reaction. Participants explore the chemical processes involved, including the dissociation of the salt into its ions and potential reactions with water.

Discussion Character

  • Homework-related
  • Debate/contested
  • Conceptual clarification

Main Points Raised

  • One participant suggests that upon dissolving, ammonium chloride dissociates into NH4+ and Cl-, indicating no redox reaction occurs.
  • Another participant questions whether a substitution reaction involving water's ions should be considered, proposing different potential reactions.
  • There is a suggestion to check the oxidation states of elements before and after the reaction to determine if any changes occur.
  • A participant expresses uncertainty about which specific reaction is taking place during the dissolution.
  • Questions arise regarding the strength of HCl as an acid and NH3 as a base, which may relate to the overall understanding of the reaction dynamics.
  • One participant references a previous contribution that addressed the nature of the reaction, reiterating the need to examine oxidation numbers of the elements involved.

Areas of Agreement / Disagreement

Participants do not reach a consensus on whether the dissolution of ammonium chloride involves a redox reaction, with multiple competing views and uncertainties remaining regarding the specific reactions and oxidation states.

Contextual Notes

Participants express limitations in understanding the reactions and the role of oxidation states, indicating that assumptions about the nature of the reactions and definitions of redox processes may not be fully resolved.

alphaj
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Quick note:
Sorry for dominating the homework help board, guys! But, I wanted to say thank you to everyone who replies to my excessive questions. This forum's input has become integral to me as I am in a position now where I can't go to my teacher for help because of the logistics of commuting :(. SO, THANKS!

Homework Statement


Redox or not? Ammonium chloride, dissolved in water

Homework Equations


n/a

The Attempt at a Solution


I think...when we dissolve, the salt dissociates into its ions.
NH4+Cl---water--> NH4+ + Cl- (If this is the case, no redox.)

But, are we considering some sort of substitution reaction with water's ions?
NH4Cl+H2O = NH4+ + Cl- + H2O = NH4+ + HCl + OH-?
OR
NH4Cl + H2O = NH4 + Cl- + H2O = NH3 + HCl + H2O

I'm not quite sure how this would proceed...But, in both, Cl is not oxidized or reduced. In one, NH4 stays the same (+1 charge). And in one, H2O lost a proton, so it was...reduced?
 
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Check the oxidation states of each of the elements before and after the reaction. Do any of them change?
 
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I guess my real issue is that I'm not understanding which reaction is happening.
 
alphaj said:
in one, H2O lost a proton
Did it now?
 
Is HCl a strong acid or a weak acid? Is NH3 a strong base or a weak base?
 
TeethWhitener nailed the question about which reaction really takes place.

Whether it is a redox:

alphaj said:
NH4Cl+H2O = NH4+ + Cl- + H2O = NH4+ + HCl + OH-?
OR
NH4Cl + H2O = NH4 + Cl- + H2O = NH3 + HCl + H2O

Does the oxidation number of any of the ELEMENTS involved change?
 

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