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Homework Help: Is this a redox reaction?

  1. Oct 22, 2017 #1
    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!

    1. The problem statement, all variables and given/known data
    Redox or not? Ammonium chloride, dissolved in water

    2. Relevant equations

    3. 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-?
    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?
  2. jcsd
  3. Oct 22, 2017 #2


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    Check the oxidation states of each of the elements before and after the reaction. Do any of them change?
  4. Oct 22, 2017 #3
    I guess my real issue is that I'm not understanding which reaction is happening.
  5. Oct 22, 2017 #4


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    Did it now?
  6. Oct 22, 2017 #5


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    Is HCl a strong acid or a weak acid? Is NH3 a strong base or a weak base?
  7. Oct 23, 2017 #6


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    Staff: Mentor

    TeethWhitener nailed the question about which reaction really takes place.

    Whether it is a redox:

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