Chemistry, 07.05.2020 11:57 tapiamelissa6
A quantity of 25.0 mL of a solution containing both Fe2+ and Fe3+ ions is titrated with 23.0 mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe2+ ions are oxidized to Fe3+ ions. Next, the solution is treated with Zn metal to convert all of the Fe3+ ions to Fe2+ ions. Finally, the solution containing only the Fe2+ ions requires 40.0 mL of the same KMnO4 solution for oxidation to Fe3+. Calculate the molar concentrations of Fe2+ and Fe3+in the original solution. The net ionic equation is Mno4- +5Fe2+ + 8H+ >>>> Mn2+ + 5Fe3+ +4H2o
Answers: 3
Chemistry, 22.06.2019 04:00, amandasantiago2001
Which of the following ocean acidification? are the most likely side effects of a ph less than 7.0 in the ocean b. more metal salts altering the ocean chemistry c. dissolution of the shells of marine organisms d. both a & b e. all of the above.
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Chemistry, 22.06.2019 18:00, tatemelliott
Which three statements represent the benefits of performing experiments using computer simulations?
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A quantity of 25.0 mL of a solution containing both Fe2+ and Fe3+ ions is titrated with 23.0 mL of 0...
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