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anonymous
 one year ago
When 0.1126g of pure iron wire was completely dissolves in H2SO4, the resulting acidic solution required 21.06 cm^3 of a solution of KMnO4 for complete reaction. What was the concentration of the KMnO4 solution?
anonymous
 one year ago
When 0.1126g of pure iron wire was completely dissolves in H2SO4, the resulting acidic solution required 21.06 cm^3 of a solution of KMnO4 for complete reaction. What was the concentration of the KMnO4 solution?

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taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1The first thing that we should do is create a balanced formula between the iron and the H2SO4 using the balanced equation we can find the number of moles of iron that gets dissolved in the reaction and use the ratio from the stoiciometric coefficients we can find how much our product has in it we can then make a second chemical formula this time including KMnO4 and the product from the first reaction contains the iron. Again we can relate the two compounds using the stoiciometric coefficients. We would know how many moles of the iron compound we would have, so we could determine how many moles of KMnO4 are required. Since we would have the moles of KMnO4 and we have the volume we can use the formula c=n/v, where n is the moles, v is the volume and you would solve for c which is the concentration of the KMnO4. I can do it step by step with you if you would like me to
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