Number of moles of Permanganate solution = 10.98/1000 * 0.01234 = 0.00013549 moles
Arsenic will go from oxidation state of +3 to +5, hence number of moles of arsenic will be
0.00013549 moles * 5/2 = 0.000338733 moles
Mass of arsenic = 0.000338733 moles * 74.92 gm/mol = 0.025377 gms
Percentage of arsenic in salt = 0.025377/0.1 * 100 = 25.37%
A sample of an arsenic salt weighing 100mg was dissolved and the arsenic converted to arsenite,...
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Question 10 (2 points) A 13.9800-g sample of a salt was analyzed for its iron content as follows: the entire sample was dissolved and diluted to 400.0 mL in a volumetric flask. A 80.00-ml aliquot of the solution required 25.38-mL of a 0.04119 M potassium permanganate solution to reach equivalence. A blank correction of 0.50 mL was required. Calculate the %(w/w) Fe in the sample. The net-ionic equation for the reaction is MnO4 (aq) + 8H+ (aq) + 5Fe2+(aq) -...
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The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 39.51 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per grams of steel (g Fe2+1 g steel). Mno, +8H+ + 5Fe2+ = Mn2+ + 5Fe'+ + 4H,0 Number g Fe2+1 g steel
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