You were calculating the concentration of EDTA (MW 372.24 g/mol; Q = 98.45%). You weighed out 8.6731 g of dried EDTA into a 450.13 mL clean volumetric flask. You showed your lab instructor your calculated EDTA concentration of (no units in standard notation with proper number of significant figures) A M. You prepared your limestone sample (1.7737 g) by dissolving it in HCl, gently heating and then filling to the line in the 450.13 mL volumetric flask. You lab partner used a 12.55 mL volumetric pipette for the limestone sample, and from the titration you recorded 25.60 mL (wine colour), 25.63 mL (purple colour). 25.67 mL (blue colour), 25.72 mL (blue colour). The P/F ratio for this calculation is (in standard notation and to the proper number of significant figures) A/ and the % Mg in the limestone sample is (answer in standard notation with no units to the proper %

You were calculating the concentration of EDTA (MW 372.24 g/mol; Q = 98.45%). You weighed out 8.6731 g of dried EDTA into a 450.13 mL clean volumetric flask. You showed your lab instructor your calculated EDTA concentration of (no units in standard notation with proper number of significant figures) A M. You prepared your limestone sample (1.7737 g) by dissolving it in HCl, gently heating and then filling to the line in the 450.13 mL volumetric flask. You lab partner used a 12.55 mL volumetric pipette for the limestone sample, and from the titration you recorded 25.60 mL (wine colour), 25.63 mL (purple colour). 25.67 mL (blue colour), 25.72 mL (blue colour). The P/F ratio for this calculation is (in standard notation and to the proper number of significant figures) A/ and the % Mg in the limestone sample is (answer in standard notation with no units to the proper %

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.195QP

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0.4545 g CaCO3 was dissolved in HCl and the resulting solution was diluted to 0.25 L. Twenty-five mL aliquot of this solution required 35.2 mL of EDTA upon performing titrimetric analysis. Determine the mass of NaH2Y·2H2O to prepare 0.5 L titrant solution. NaH2Y·2H2O is a cmpound with MW = 372.2 g/mol Note: H2Y2- = EDTA
Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 9.000 mL V2, volume of standard NaOH required for second equivalence point : 15.90 mL Calculate the mass of iron in the sample :
The aluminium in a 1.2 g sample of impure NH4Al (SO4)2 was precipitated as hydrous Al2O3. The precipitate was filtered and ignited at 100° c to give anhydrous Al2O3 which weighed 0.1798 g. Calculate the % Al in the sample. (number of moles Al = 2; Al2O3 = 1)
Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the mass of iron in the sample : Calculate the percent of iron in the sample :
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)
A 0.6599-g sample of impure magnesite, MgCO3 (MW = 84 g/mole), was decomposed with HCl; the liberated CO2 (MW = 44 g/mole) was collected on absorbent and found to weigh 0.1673-g. Calculate the percentage of magnesium (MW = 24 g/mole) in the sample. MgCO3 (s) + 2 HCl (aq) →MgCl2 (aq) + CO2 (g) + H2O(l) Weight of pure magnesium in the sample is a. 0.1825 g b. 0.0913 g c. 0.3194 g d. 0.0456 g Percentage of magnesium carbonate in the sample is a. 24.20% b. 27.66% c. 48.40% d. 96.80%
A 1.00 g sample of limonite iron ore, 2Fe203 · 3H20, is dissolved, reduced to Fe2+ and titrated with 20.00 mL of 0.20 M cerium (IV). Calculate the percentage of 2FE203 · 3H20, (FM: 373.38 g/mol) in the sample. Titration reaction: Fe2+ + Ce*+ → Fe3+ + Ce3+
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 9.000 mL V2, volume of standard NaOH required for second equivalence point : 15.90 mL Calculate the mass of potassium in the sample :
A 5.70 g iron ore was dissolved in concentrated HCl. After the dissolution, the resulting solution was made basic by adding 6.0 M NaOH slowly until the solution is slightly turbid. Urea was then added and the solution was heated for 3 hours. The precipitate was filtered using an ashless filter paper and ignited to form Fe2O3 (159.69 g/mol). The mass of precipitate is 2.1 g. Find the % Fe3O4 (231.54 g/mol) in the iron ore sample.
Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the mass of potassium in the sample : Calculate the percent of potassium in the sample : Calculate the volume of standard NaOH that reacted with iron
Mass of KxFe(C2O4)y · zH2O : 5.10 g Mass of sample : 0.195 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 8.950 mL V2, volume of standard NaOH required for second equivalence point : 17.70 mL Calculate the mass of potassium in the sample : _____ g Calculate the percent of potassium in the sample : ______ % Calculate the volume of standard NaOH that reacted with iron : ______ mL Calculate the mass of iron in the sample : ______g Calculate the percent of iron in the sample : ________% Fe

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9781305580343

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