Balance the equation in aqueous basic solution:
As2S3(s) + H2O2(aq) → AsO43-(aq) + SO42-(aq)

I normally understand how to balance redox equations, but this one confuses me because I would normally think that the As2S3 is being reduced to AsO4^3-, but since the As2S3 has a "S", do i also include the SO4^2-? but even when i do that, and try to balance the electrons for the half rxn, it seems to change into oxidation... I'm really confused!

  1. 👍
  2. 👎
  3. 👁
  1. I usually attack this type this way. Yes, both As and S are changing, As from +6(total of 2 atoms As) to +10(total of 2 atoms As). S is changing from -6 (total of 3 S atoms to +18(total of 3 atoms S). Most of the time it works out if one simply combines the As and S into one kind of reaction (add electrons algebraically). What has been omitted is the reaction of the H2O2. You'll see what to do when that is included.

    1. 👍
    2. 👎
  2. Here’s a hint. The half reactions that must be balanced are As₂S₃ —> AsO₄³⁻ + SO₄²⁻ (oxidation) and H₂O₂ —> ? (reduction). You can determine which ions to group by examining oxidation numbers. Note that since H₂O₂ consists of only hydrogen and oxygen, you can instantly balance the half reaction by adding water and H⁺/OH⁻ ions as you would for any half reaction once the non-hydrogen/non-oxygen species have been balanced by inspection. This explains why there is no obvious product in the half reaction (the product is water which is added in only when balancing).

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    When the equation for the following reaction in basic solution is balance, what is the sum of the coefficients? MnO2 + HO2^1-.....>MnO4^1- A=11 B=31 C=14 D=9

  2. Chemistry

    Hydrogen peroxide can act as either an oxidizing agent or a reducing agent, depending on the species present in solution. Write balanced half-reaction equations for each of the following: (a) H2O2(aq) acting as an oxidizing agent

  3. Chemistry

    Balance the following equation for a half reaction that occurs in basic solution. Use e– as the symbol for an electron. SO3^2- ---> S2O4^2-


    The reaction of aqueous iron(II) sulfate and aqueous barium nitrate is represented by the balanced net ionic equation. SO42-(aq) + Ba2+(aq) → BaSO4(s) Give the balanced formula equation for the reaction. Include the states.

  1. Chemistry

    Balance the equation in aqueous basic solution: NO2-(aq) + Al(s) → NH3(aq) + AlO2-(aq) I know how to balance equations in acidic solutions, but I get lost doing the basic one, please help?

  2. Balance each of the following redox reactions occu

    Balance each of the following redox reactions occurring in acidic solution a) SO32- (s) +MNO4- ---> SO42- +Mn2+ b) S2O32-+ Cl2 ---> SO42-+Cl-

  3. chemistry

    Balance the following redox equation occurring in a basic solution: AG + CN{-} + O2 = AG(CN)2{-} I tried...but this is wrong...2H2O+ AG + CN{-} + O2 = AG(CN)2{-}+4OH{-}... I am supposed to do half do I spit the

  4. chem

    Balance the following oxidation-reduction reaction in acid solution: SO32- + MnO4- --> SO42- + Mn2+ + H2O

  1. chemistry

    write a balanced equation for the reaction that occurs when an aqueous solution of iron(II) chloride is mixed with an aqueous solution o potassium hydroxide.

  2. chemistry

    An aqueous solution of barium nitrate and an aqueous solution of sodium sulfate are mixed together. Write the skeletal equation for the following reaction: Balance the completed chemical equation in .

  3. Chemistry

    After balancing the following redox equation(using small whole-number coefficients), add the coefficients of all species in the balanced equation. Bi(OH)3 + SnO2^(2-) → Bi + SnO3^(2-) (basic solution) --- I separated the

  4. Chemistry

    Balance the following equation in basic solution. Phases are optional. I{-}+IO4{-} --> I3{-}+IO3{-}

You can view more similar questions or ask a new question.