1) A balanced chemical equation for the oxidation of oxalic acid using potassium
ID: 524858 • Letter: 1
Question
1) A balanced chemical equation for the oxidation of oxalic acid using potassium permanganate the oxidizing agent, in an acid solution. This reaction can be presented as a equation 2) many 0.020 M potassium permanganate solution calculation that predicts how milliliters o the balanced you will need to titrate an ~0.25 g sample of alic acid dihydrate, according to equation above 3) table for this first titration. Your data table should look like the data tables used in the other experiments that we've done this semester. Read the procedure before you set titration up your data table, though. You should put in blanks or spaces to record and to show sample calculations for results from the first part of the experiment 4) A balanced chemical equation for the oxidation of iron ll) ions using potassi permanganate as the oxidizing agent, in an acid solution. This reaction can be presented as a net ionic equation 5) A calculation for the part of the experiment that predicts h many milliliters of 0.020 M second potassium permanganate solution you will need to titrate a 1.300 g of Mohr's Salt, an iron (ll)-containing compound, according to balanced equation you write out for 4), just above 6) A data able for the second titration. The comments for the first data table (Point 3, above) apply here, tooExplanation / Answer
Ans 1. The reaction of oxalic acid and potassium permanganate takes place in the acidic medium . The acid used is sulfuric acid.
The net ionic equation is given as,
2MnO4- + 5H2C2O4 + 6H+ ---> 2Mn2+ +10CO2 + 8H2O
The hydrogen ion in the reactants side , as you may see comes from the sulfuric acid.
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