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Asked Oct 4, 2019
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How to solve number 69? Please explain from the basic :)

69. A solution of potassium permanganate reacts with oxalic acid, H2C20
to form carbon dioxide and solid manganese (IV) oxide (MnO2).
(a) Write a balanced net ionic equation for the reaction
(b) If 20.0 mL of 0.300 M potassium permanganate is required to
react with 13.7 mL of oxalic acid, what is the molarity of the oxalic
acid?
(c) What is the mass of manganese(IV) oxide formed?
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69. A solution of potassium permanganate reacts with oxalic acid, H2C20 to form carbon dioxide and solid manganese (IV) oxide (MnO2). (a) Write a balanced net ionic equation for the reaction (b) If 20.0 mL of 0.300 M potassium permanganate is required to react with 13.7 mL of oxalic acid, what is the molarity of the oxalic acid? (c) What is the mass of manganese(IV) oxide formed?

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Expert Answer

Step 1

(a) A balanced net ionic equation for the reaction between potassium permanganate and oxalic acid to give carbon dioxide and solid manganese oxide is given below.

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2Mno (aq)+3C02 (aq) +8H* (aq)-»2MnO2 (s)+6CO2 (g)+4H20(1)

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Step 2

(b) From the above balanced chemical equation, it can be stated that 2 moles of KMnO4 is reacting with 3 moles of oxalic acid to pro...

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Moles of potassium permanganate mol x 20.0mL x L 1L =0.006mol -Molarity x Volume = 0.300- 1000mL 3 Moles of oxalic acid = -x0.006 mol = 0.009mol 2 Molarity of охаlic acid Moles of solute 0.009mol =0.657M 1 1L Volumeof the solution 13.7mL x 1000 mL Therefore, the molarity of 13.7 mL of oxalic acid is 0.657 M.

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