Calculate the volume of ca. 0.1 M AgNO3needed to be added to have 25% excess in solution. If 25.00 ml of the sample (50% Cl m/m) is required to react with the precipitating reagent
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- Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3(Ksp=1.36107). (b) If the NiCO3 were a contaminant in a sample of COCO3(Ksp=1.01012), what mass of COCO3 would have been lost? Keep in mind that both NiCO3 and COCO3 dissolve in the same solution.A 0.6560 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water. AgNO3 was added to the solution, precipitating all of the CN− in solution as AgCN (MW=133.886 g/mol). The dried precipitate weighed 1.505 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt% = ~ 66.01 NaCN wt% = ?0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M'pure water, 2 M H2SO4 added, heating process and 8.4 mL titrant as a result of titration it's spin out. Calculate the actual concentration of potassium permanganate accordingly
- TOPIC: GRAVIMETRY SHOW THE SOLUTION The mercury in a 0.7152-g sample was precipitated with an excess of paraperiodic acid, H5IO6, according to the following reactions:5 Hg+2 + 2 H5IO6 ---> Hg5(IO6)2(s) + 10 H+The precipitate was filtered, washed free of precipitating agent, dried and found to weigh 0.3408-g. Calculate the percentage of Hg2Cl2 in the sample. Molar Masses: Hg5(IO6)2 = 1448.75 Hg2Cl2 = 472.09 Answer: 38.82% Hg2Cl2 An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron (III) was precipitated as the hydrous oxide Fe2O3·xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3. Calculate (a) % Fe, and (b) % Fe3O4 in the sampleMolar Masses: Fe2O3 = 159.69 Fe = 55.847 Fe3O4 = 231.54 Answer: 33.32% Fe and 46.04% Fe3O4The thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg2+ via the reaction. Calculate the percent (NH2)2CS (76.12 g/mol) in the sample. 4 (NH2)2CS + Hg2+ → [(NH2)2CS]4Hg2+How much alum product would be lost to the recrystallization solution if you had 42.5 mL of solution after filtration and the solubility of alum is approximately 2.62 g alum in 100. mL of 0oC acidic water?
- The solutbility constant for Ce(IO3)3 is 3.2x10^-10. What is the Ce3+ concentration in a solution prepared by mixing 50 mL of 0.0450 M Ce3+ with 50 mL of: A.) 0.0450 M IO3- ? B.) 0.0500 M IO3- ?100.0 mL of 0.60 M aqueous Pb(NO3)2 is mixed with excess aqueous KI. What mass of precipitate is formed?1,5419 g of magnetite (Fe3O4) ore; in concentrated HCL to form a mixture of Fe + 2 and Fe+3it's unraveling. By adding HNO3 to it, all Fe+2 s are upgraded to Fe+3. And the addition of FE+3 s NH3,with Fe (OH)3, precipitating into. The sediment is weighed as 0.8525 g in the form of Fe2O3 after the necessary operations. Calculate the percentage of Fe3O4 in the sample.
- 400 g sample containing chloride ions (MW=35.45 g/mol) was dissolved in 50.0mL of distilled water. A 15.0 mL aliquot was taken, and was further diluted to 50.0 mL using distilled water. The diluted solution was then titrated using a 0.0989 M AgNO3 solution, and it consumed a total of 31.9 mL of the titrant in order to reach the end point. What is the concentration of the undiluted chloride solution? Round off to three (3) significant figures. What is the % (w/v) concentration of the undiluted chloride solution? Round off to two (2) decimal points. What is the % (w/w) of Cl- composition of the sample? Round off to two (2) decimal points.A student weighed out 3.5689g of unknown nickel salt and carried out the gravimetric analysis in order to determine the % nickel in the unknown sample. The mass of one of the two bis(dimethylglyoximate) nickel(11) precipitates that was filtered was 0.1570g. How many moles of Ni 2+ are in the precipitate?A vinegar solution was prepared by diluting 25.00 mL of vinegar to 250.0 mL. From this solution, 50.00 mL portion was taken, and this required 30.00 mL of 0.1000M NaOH solution to reach neutralization end point. What is the percentage (w/v) of HOAc in the sample? Mol wt HOAc = 60.0 g/mol
