Prepare 1.0 L of a 50.00 ppm iron solution from the solid Fe(NH4)2(SO4)2 of the 80.0% purity. Clearly describe how to prepare this solution. If done Chlorimetric iron analysis using the calibration curve method, specify the form of preparation of 100.0 ml of each of the following standard solutions with contents of 1.00, 5.00, 15.00 and 20.00 ppm of Fe respectively from the solution mother (It suppose that the answers are: 0.3180, 2.00, 10.00, 20.00, 30.00 and 40.00 ml of the mother solution and dilute exactly to 100.0 mL with deionized water)

Prepare 1.0 L of a 50.00 ppm iron solution from the solid Fe(NH4)2(SO4)2 of the 80.0% purity. Clearly describe how to prepare this solution. If done Chlorimetric iron analysis using the calibration curve method, specify the form of preparation of 100.0 ml of each of the following standard solutions with contents of 1.00, 5.00, 15.00 and 20.00 ppm of Fe respectively from the solution mother (It suppose that the answers are: 0.3180, 2.00, 10.00, 20.00, 30.00 and 40.00 ml of the mother solution and dilute exactly to 100.0 mL with deionized water)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

See similar textbooks

Similar questions

a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
A solution is made by mixing 500.0 mL of 0.04170 M Na₂HASO4 with 500.0 mL of 0.03037 M NaOH. Complete the mass balance expressions for the sodium and arsenate species in the final solution. [HASO]+ [Na] = M = M
0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)
A sample containing BaCl, 2H,0, KCI and inert material weighed 0.8417 g. After heating the sample at 160°C for 45 min, it weighed 0.8076 g. The sample was then dissolved in water and treated with a slight excess of AgNo,. The resulting precipitate was collected and found to weigh 0.5847 g. Calculate the % Bacl,-2H,0 and % KCI in the sample. 3.
A solution is made by mixing 500.0 mL of 0.04419 M Na₂HASO with 500.0 mL of 0.03835 M NaOH. Complete the mass balance expressions for the sodium and arsenate species in the final solution. [HASO²] + [Na] = M = M
A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO
E. Analysis of a mixture consisting of NaOH + NażCO3 + inert matter gives the following data: Sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample. 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mL
A mineral in a fine state of division (0.6324 g) was dissolved in 25.0 mL of 4.0 mol / L boiling HCl and diluted with 175.0 mL of H2O containing two drops of methyl red indicator. The solution was heated to 100 ° C and a heated solution containing 2.00 g of (NH4) 2C2O4 was added slowly to precipitate CaC2O4. Next, NH3 6.0 mol / L was added until the indicator changed from red to yellow, indicating that the liquid was neutral or slightly basic. After slow cooling for 1 hour, the liquid was decanted, the solid transferred to a crucible and washed five times with 0.10 wt% (NH4) 2C2O4 solution, until no Cl- was detected in the filtrate with the addition of AgNO3 solution. The crucible was dried at 105 ° C for 1 hour and then taken to an oven at 500 ° C ± 25 ° C for two hours. The mass of the empty crucible was 18.2311 g. The crucible mass with CaCO3 (s) was weighed 5 times to an average of 18.5467 g. Determine the percentage, by mass, of Ca in the mineral. Ca (40.078 g / mol); C (12.01078…
Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?
The Kjeldahl method was used to determine the nitrogen content of a protein. A 275 µL aliquot of a 47.0 mg/mL protein solution was digested in boiling sulfuric acid. The solution was made basic and the liberated NH, was collected in 5.00 mL of 0.0512 M HCl. A volume of 7.00 mL of 0.0174 M NaOH was required to react with the excess HCl. Calculate the weight percent of nitrogen in the protein. weight percent: wt% N
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na*B(C,H,). Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non-negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K,CO, and all ammonium is present as NH,Cl. A 5.045 g soil sample was dissolved to give 0.500 L of solution. A 125.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K* and NH ions completely. B(C,H,), + K* KB(C,H,),(s) Compound Formula mass 358.33 g/mol KB(C,H,), NH,B(C,H,), K, CO, B(C,H ), + NH NH,B(C,H,), (s) 337.27 g/mol 138.21 g/mol The resulting precipitate amounted to 0.247 g. A new 250.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH as NH,. NH,CI 53.492 g/mol The resulting solution was then acidified, and excess sodium…
(4) The amount of oxalic acid in a sample of 3+ rhubarb was determined by reacting with Fe as outlined in the following reaction. In a typical analysis, the oxalic acid in 10.62 g of rhubarb was extracted with a suitable solvent. The complete oxidation of the oxalic acid to 3+ CO, required 36.44 mL of 0.013 M Fe*.What is the weight percent of oxalic acid in the sample of rhubarb? 2FE3" (aq) + H2C,O,(aq) + 2H2O(1) → 2Fe?* (aq) + 2C02(g) + 2H;0 (aq)