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what are the significant applications of extraction in the industry.
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- A sample of 1.55g of iron ore is dissolved in a acid solution in which the iron is converted into Fe2+. The solution formed is the titration with KMnO4 which oxidises Fe2+ to Fe3+ while the MnO4 ions are reduced to Mn2+ ions.92.9 mL of 0.020 M KMnO4 is required for titration to reach equivalence point. Write the balanced equation for titration.What is the role of zinc metal in the extraction of silver?Name the chief ores of aluminium and zinc.
- A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.what is the Gravimetric analysis? how we can use it to determine the Phosphorus content of commercial plant food?6. Cite application of the acid sulfate solution in plating the different metals commonly used in industry.
- Write a chemical equation for the reaction of CO2 and limewater (Ca(OH)2). Write a physical description of the products formed.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 1.047 g sample of canned tuna was analyzed by the Kjeldahl method; 24.61 mL of 0.1180 M HCl were required to titrate the liberated ammonia. Calculate the percentage of nitrogen in the sample. 1. 03.89% 2. O2.99% 3. O39.9% 4. O9.38% 5. O2.10%