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Q: Balance the reactions below using the change in oxidation number method. KBr + KClO2+ H2SO4 → Br2 +…
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- The Ostwald process for the commercial production of nitric acid involves the following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) 2NO(g)+O2(g)2NO2(g) 3NO2(g)+H2O(l)2HNO3,(aq)+NO(g) a. Which reactions in the Ostwald process are oxidationreduction reactions? b. Identify each oxidizing agent and reducing agent.A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?A stock solution containing Mn2+ ions was prepaned by dissolving 1.584 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution: For solution A, 50.00 mL of stock solution was diluted to 1000.0 mL. For solution B, 10.00 mL of solution A was diluted to 250.0 mL. For solution C, I 0.00 mL of solution Bwas diluted to 500.0 mL. Calculate the concentrations of the stock solution and solutions A,B, and C.
- 1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution.1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution. Box the final answer.A 350 mg sample containing KClO3 was carefully reduced and treated with excess AgNO3. The resulting AgCl (MW = 143 g/mole) weighed 185 mg. Calculate the percentage of KClO3 (MW = 122 g/mole) in the sample
- A sample of magnetite (impure Fe3O4) weighing 0.5000 g is fused with oxidizing flux and the ferric compound formed is eventually precipitated as ferric hydroxide and ignited to ferric oxide (Fe2O3 MM 159.70 g/mol) which weighs 0.4980 g. Calculate % Fe.A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate. a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?A sample containing NaCl, NaBr, & inert material weighs 1.000 g. Excess of AgNO3 gave a whiteprecipitate consisting of only AgCl and AgBr which weighs 0.5260 g. By heating the precipitate in a currentof Cl2 gas, the AgBr (187.78 g/mol) is converted to AgCl (143.32 g/mol) and the precipitate weighs 0.4260g. Find the % NaCl (58.44 g/mol) and % NaBr (102.909 mol) in the original sample.
- A 0.5 g sample of an alloy containing 30% (m/m) iron (MM 55.84 g/mol) is dissolved in acid and diluted to 1 L with deionized water. A 10 mL aliquot was taken for analysis, conveniently diluted and included with an excess of ammonium hydroxide, which led to the formation of a reddish solid. After filtration and washing, the solid was calcined to Fe2O3 (MM 159.69 g/mol). Calculate the mass of this final product.An ore is treated with concentrated nitric acid and potassium chlorate to convert all S (32.06 g/mol) to sulfate. The nitrate and chlorate are then removed by repeated furning with concentrated HCl, and the sulfate is precipitated and weighed as BaSO4 (233.40 g/mol). What is the % (w/w) S in an ore, 2.5000 g of which yields 0.6255 g BaSO4 . 3.44 % (w/w) 3.34 x 10-3% (w/w) 18.21 % (w/w) 24.31 % (w/w)The amount of protein in a sample of cheese is determined by a Kjeldahl analysis for nitrogen. After digesting a 0.9814g sample of cheese, the nitrogen is oxidized to NH4+, converted to NH3 with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1047 M HCl. The excess HCl is then back titrated with 0.1183 M NaOH, requiring 22.84 mL to reach the bromothymol blue end point. Report the %w/w protein in the cheese given that there is 6.38 g of protein for every gram of nitrogen in most dairy products.