Part B Assume you fill a buret with your KMnO4 solution and the volume initally

Question

Part B Assume you fill a buret with your KMnO4 solution and the volume initally reads 0.15 mL (don't waste your time trying to fill it drip by drip to exactly 0.00 mL, just record the starting volume). After you use the KMnO4 solution to titrate your iron sample you notice the buret then reads 25.78 mL. What is the volume of KMnO4 used?

Part D

Looking at the stoichiometry of the reaction (see the lab manual), how many moles KMnO4 must have been delivered by the buret to react with that much Fe(NH4)2(SO4)2 · 6H2O? 8H+ + 5Fe+2 + MnO4 - --> Mn+2 + 5Fe+3 + 4H2O (Remember that all Group I salts are soluble - including KMnO4. Therefore moles KMnO4 = moles MnO4 -)

Part E

Considering the moles and volume of KMnO4 above, what must the true molarity of your KMnO4 solution be?

Explanation / Answer

Part B: Volume of KMnO4 used = Final burette reading(mL)-Initial burette reading (mL)= 25.78- 0.15= 25.63 mL

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