Chemistry

Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, , can be titrated against a solution of potassium permanganate, . The following equation represents the reaction:
2KMnO4+H202-> 3H2SO4->O2+2MnSO4+ K2SO4+4H2O

A certain amount of hydrogen peroxide was dissolved in 100.mL of water and then titrated with 1.68M KMnO4. How much H2O2 was dissolved if the titration required 12.3mL of the KMnO4 solution?

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
  1. moles KMnO4 = M x L = ??
    moles H2O2 = 1/2 x moles KMnO4.
    g H2O2 = moles H2O2 x molar mass H2O2.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩

Respond to this Question

First Name

Your Response

Similar Questions

  1. 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

  2. Chemistry

    7. 2Sr + O2  2SrO a) Determine what is oxidized and what is reduced b) Identify the oxidizing agent and the reducing agent 8. 2Cs + Br2  2CsBr a) Determine what is oxidized and what is reduced b) Identify the oxidizing agent

  3. chemistry

    In the following half equation, which is the oxidizing agent? NO3–(aq) + 4H+(aq) + 3e– NO(g) + 2H2O a. NO3– b. H+ c. e– d. NO e. H2O An oxidizing agent is a chemical compound that readily transfers oxygen atoms, or is a

  4. Chem Oxidation-Reduction Titrations

    H2O2→ O2 + 2H+ + 2e- OCl- + 2H+ + 2e-→ H2O+ Cl- H2O2(aq) + OCl-(aq) → H2O(l) + Cl- (aq) + O2(g)Assign oxidation numbers to the following atoms: O in H2O2 ________; Cl in OCl- __________The oxidizing agent for this RedOx rxn

  1. chemistry

    Identify the oxidizing and reducing agents in each of the following redox reactions: (4 points) a) 2 H2O (l) + Al (s) + MnO4 -1(aq) ---→ Al(OH)4 -1(aq) + MnO2 (s)

  2. Chem Check Please!!!

    1) Assuming the following reaction proceeds in the forward direction, 3 Sn4+(aq) + 2 Cr(s) ---> 3 Sn2+(aq) + 2 Cr3+(aq) a.Sn4+(aq) is the reducing agent and Cr(s) is the oxidizing agent. b.Cr(s) is the reducing agent and Sn2+(aq)

  3. Chem

    In the reaction 2HNO3(aq) + Cu(s) + 2H+(aq) �¨ 2NO2(g) + Cu2+(g) + 2H2O(l) Which of the following statements is correct? A.HNO3 is the reducing agent, and Cu is the oxidizing agent B.HNO3 is the reducing agent, and H+ is the

  4. Chemistry

    I dont quite understand how to find out if it's capable of reducing/oxidizing. My understanding is we check each potential and identify which is reduce = highest potential, oxidize = lowest potential. These are my predictions: yes

  1. chem!

    Arrange the three metals(Cu, Zn, and Mg) in order of their relative strengths as reducing agents, placing the strongest first. Arrange the three metallic ions ( Cu(No3)2, Zn(No3)2, and Mg(No3)2 ) in order of their relative

  2. chemistry

    Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction. 2Fe3+ + Sn2Fe2+ + Sn2+ species oxidized species reduced oxidizing agent reducing agent As

  3. Chemistry

    Choose and best oxidizing agent and the best reducing agent: Ni2+, Al, H+, and I- ??? I'm so confused, please help! I know the oxidizing agent is being reduced and the reducing agent is getting oxidized. But how do I use the

  4. Chemisry

    Potassium, a silvery metal, reacts with bromine, a corrosive, reddish liquid, to yield potassium bromide, a white solid. Write the balanced equation, and identify the oxidizing and reducing agents.

View more similar questions or ask a new question.