Redox Reaction in Dissolved Ammonium Chloride

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SUMMARY

The discussion centers on the classification of the dissolution of ammonium chloride (NH4Cl) in water as a redox reaction. Participants clarify that when NH4Cl dissolves, it dissociates into NH4+ and Cl- ions, indicating no change in oxidation states, thus confirming it is not a redox reaction. The confusion arises from potential substitution reactions involving water, but ultimately, the oxidation states of all elements remain unchanged throughout the process. The consensus is that neither Cl nor NH4 undergoes oxidation or reduction during this dissolution.

PREREQUISITES
  • Understanding of ionic dissociation in aqueous solutions
  • Knowledge of oxidation states and redox reactions
  • Familiarity with acid-base chemistry, specifically strong and weak acids and bases
  • Basic chemical reaction equations involving NH4Cl and H2O
NEXT STEPS
  • Study the principles of ionic dissociation in solutions
  • Learn about oxidation states and how to identify redox reactions
  • Research the properties of strong acids and weak bases, focusing on HCl and NH3
  • Explore substitution reactions in aqueous solutions and their implications
USEFUL FOR

Chemistry students, educators, and anyone interested in understanding redox reactions and acid-base chemistry, particularly in the context of ammonium chloride and its behavior in water.

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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