Redox, redux table, exercise 2 (Redox-29)

Use the redox table to assess whether the following reactions are possible.

1. Ag in copper sulphate
2. Silver nitrate in copper
3. You react (elementary) bromine with iron. Bromine is in excess.
4. [translation unavailable] in 1 M HCl
5. How can silver be extracted from nitrate in solid form? Only acids or bases are permitted as auxiliaries.
6. Gold is to be dissolved in a solution. Please specify a suitable variant.

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• October 16, 2026 at 4:42 am #9506
    Exercise: Redox-29    

  ⓘ    🔄 Reload     🖨️ print           ◀  –   ▶     ?! Question/Answer ?!

  Use the redox table to assess whether the following reactions are possible.

  1. Ag in copper sulphate
  2. Silver nitrate in copper
  3. You react (elementary) bromine with iron. Bromine is in excess.
  4. [translation unavailable] in 1 M HCl
  5. How can silver be extracted from nitrate in solid form? Only acids or bases are permitted as auxiliaries.
  6. Gold is to be dissolved in a solution. Please specify a suitable variant.

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    Exercise: Redox-29    

  ⓘ    🔄 Reload     🖨️ print           ◀  –   ▶     ?! Question/Answer ?!

  Use the redox table to assess whether the following reactions are possible.

  1. Ag in copper sulphate
  2. Silver nitrate in copper
  3. You react (elementary) bromine with iron. Bromine is in excess.
  4. [translation unavailable] in 1 M HCl
  5. How can silver be extracted from nitrate in solid form? Only acids or bases are permitted as auxiliaries.
  6. Gold is to be dissolved in a solution. Please specify a suitable variant.

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  October 16, 2026 at 4:42 am #9507
  Solution:

  1. Copper sulphate: CuSO₄ thus Cu²⁺ and SO2-4
         SO2-4 Viewers, not participating
         Ag + Cu²⁺ → Ag⁺ + Cu ??
         Redux table from left -> right to interpret
         Voluntary mountain reaction not possible
  2. Silver nitrate: AgNO₃ meaning Ag + and NO–3
         NO–3 Viewers not participating
         Cu + Ag⁺ → Cu²⁺ + Ag ??
         Redux table from left -> right to interpret
         Mountaineering, voluntary reaction
  3. Extract from the electrode potential table:
         Fe → Fe²⁺ (-0.44)
         2·Br^– → Br₂ (+1.07)
         thus: Fe + Br₂ → 2·Br^– + Fe²⁺
         But … it goes on and on .
         Fe²⁺ → Fe³⁺ (+0.75)
         thus: Fe + Br₂ → 2·Br^– + Fe³⁺
         Load balancing: 2·Fe + 3·Br₂ → 6·Br^– + 2·Fe³⁺
  4. As a reminder: 1 M HCl
               → Cl^– (viewers)
               → H₃O⁺
         Mg → Mg²⁺ (-2.37 V)
         H₂ + 2·H₂O → 2·H₃O⁺ (0.00)
         Mg + 2·H₃O⁺ → H₂ + 2·H₂O + Mg²⁺
         Mountaineering, voluntary reaction
         Magnesium dissolves to form H₂ gas
  5. Silver nitrate: AgNO₃ meaning Ag + and NO–3
         Required: Ag⁺ → Ag
         In our case , Ag⁺ is the oxidizing agent !
         Reducing agents are sought (acid or base)
         However, only the base (OH^-) is available.
         4 OH^– → O₂ + 2·H₂O (0.4 V)
         Ag → Ag⁺ (0.8 V)
         Reaction occurring: 4 OH^– + Ag⁺ → O₂ + 2·H₂O + Ag
         According to the Redox table, there are also the following voluntary mountain breaks under gold:
         Au → Au³⁺ (1.42 V)
         Mn²⁺ + 12 H₂O → MnO–4 + 8·H₃O⁺ (1.51 V)
         PbSO₄ + 5 H₂O → PbO₂ + HSO–4 + 3·H₃O⁺ (1.68 V)
         2 F^– → F₂ (2.87 V)
         According to exercise a solution is to be manufactured. The reaction with F₂ would be theoretically possible, but a salt is formed. Therefore, only the variants with 1.51 V or 1.68 V are correct.
         Au + MnO–4 + 8·H₃O⁺ → Au³⁺ + Mn²⁺ + 12 H₂O … Or
         Au + PbO₂ + HSO–4 + 3·H₃O⁺ → Au³⁺ + PbSO₄ + 5 H₂O

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