Redox Reaction in Dissolved Ammonium Chloride

[alphaj]

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?

 

[TeethWhitener]

Check the oxidation states of each of the elements before and after the reaction. Do any of them change?

 

[alphaj]

I guess my real issue is that I'm not understanding which reaction is happening.

 

[Bystander]

in one, H2O lost a proton

Did it now?

 

[TeethWhitener]

Is HCl a strong acid or a weak acid? Is NH₃ a strong base or a weak base?

 

[Borek]

TeethWhitener nailed the question about which reaction really takes place.

Whether it is a redox:

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?