Asolution of potassium permanganate reacts with oxalic acid, h2c2o4, to form carbon dioxide and solid manganese(iv) oxide (mno2). write a balanced net ionic equation for the reaction. if 20.0 ml of 0.300 m potassium permanganate are required to react with 15.0 ml of oxalic acid, what is the molarity of the oxalic acid? what is the mass of the manganese(iv) oxide formed

The molarity of oxalic acid is 0.6 M

There is 0.522 grams of manganese oxide formed.

Explanation:

Step 1: The balanced equation

MnO4- + 3e- +4H+ → MnO2 + 2H2O

H2C2O4 → 2CO2 + 2H+ + 2e-

2H+ + 2MnO4- + 3H2C2O4 → 2MnO2 + 6CO2 + 4H2O

Step 2: Data given

20.0 mL of 0.300 M potassium permanganate ( KMnO4)

volume of oxalic acid = 15.0 mL

Step 3:  Calculate moles of KMnO4

Number of moles KMn04 = Molarity KMnO4 * Volume KMnO4

Moles of KMnO4 = 0.300 M * 0.02 L = 0.006 mol KMnO4

Step 4: Calculate moles of H2C2O4

For 2 moles KMnO4 consumed, we need 3 moles of H2C2O4

For 0.006 moles of KMnO4, we need 0.006 *3/2 = 0.009 moles of H2C2O4

Step 5: Calculate molarity of H2C2O4

Molarity = moles / volume

Molarity = 0.009 moles / 0.015 L

Molarity = 0.6 M

Step 6: Calculate moles of MnO2

For 2 moles KMnO4 consumed, we need 3 moles of H2C2O4, to produce 2 moles of MnO2

So for 0.006 moles of KMnO4 we have 0.006 moles of MnO2

Step 7: Calculate mass of MnO2

Mass MnO2 = Moles of MnO2 * Molar mass MnO2

Mass MnO2 = 0.006 moles * 86.937 g/mol = 0.522 grams

There is 0.522 grams of manganese oxide formed.

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots

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