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 %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A prospector wants to know how much gold is in the ore that he has been mining. A sample weighing 11.2456 grams is dissolved in Aqua Regia (a mixture of HCl and HNO3). That sample is then transferred to a 200.00 mL volumetric flask and diluted to the mark with water. This is called solution 1. A volumetric pipet is used to transfer 10.00 mL of solution 1 to a second 500.00 mL volumetric flask. The second flask is filled to the mark resulting in solution 2. 5.00 mL of solution 2 is analyzed and found to contain 13.45 ppm Au. Answer each of the questions below. 1. What is the concentration of Au in solution 1. The units should be ppm 2. How many micrograms of Au are in the 5.00 mL sample that was measured? 3. How many micrograms of gold were in the 500.00 mL flask containing solution 2. 4. How many grams Au were in the flask containing solution 1 5. What is the %Au in the original sample?
Solid residue weighing 7.158 g from an aluminum refining process was dissolved in acid to give Al3+ in solution. The solution was treated with 8-hydroxyquinoline to precipitate (8-hydroxyquinoline)3Al (FM 462.462 g/mol), which was ignited to give Al2O3 (FM 101.961 g/mol) weighing 1.178 g. Find the weight percent of Al (FM 26.982 g/mol) in the original mixture.
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 :
A student determined the chloride content of a commercial salt by using the Mohr method. A 0.7725 -g sample of the salt was dissolved in distilled water and diluted to a final volume of 250. mL. A 25.-mL aliquot of the analyte solution was then titrated against a standard 0.0347 M AgNO3(aq) solution to the chromate end-point. A blank-corrected volume of 25.96 mL was recorded. Calculate the percent chloride in the sample.
A student determined the chloride content of a commercial salt by using the Mohr method. A 0.7725 -g sample of the salt was dissolved in distilled water and diluted to a final volume of 250. mL. A 25.-mL aliquot of the analyte solution was then titrated against a standard 0.0347 M AgNO3(aq) solution to the chromate end-point. A blank-corrected volume of 25.96 mL was recorded. Calculate the percent chloride in the sample. Provide your answer to two decimal places and without units.
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 percent of iron in the sample :
An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)
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 :
The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the 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.
If a second brass washer of 0.6003 grams had been dissolved in nitric acid, diluted to 50.00 mL and then its absorbance measured at 0.450, what would be the concentration of Cu(NO3)2 in the solution? What would be the mass percent of copper in the second brass washer? Use equation of the line as y = 3.1295 x + 0.0055.
Give typed full explanation A stock solution of lithium phosphate (Li3PO4, MM= 115.794361 g/mol) is prepared by dissolving 295.8 g Li3PO4 in deionized water to a final total volume of 1.000 L. Suppose a 1.000-mL aliquot is taken from this stock solution and transferred to a new container to which deionized water is added until the total volume is 50.00 mL. A new 1.000-mL aliquot is taken from this 50.00 mL solution and transferred to a third container to which deionized water is added until the total volume is 25.00 mL. Calculate the number of individual lithium ions (Li+) in the final 25.00-mL solution. Note that lithium phosphate is a strong electrolyte that completely dissociates in water (note that (aq) means the species is a solute in an aqueous solution): Li3PO4 (aq) 3 Li+ (aq) + PO43– (aq) Report your answer to two significant figures. Use scientific notation. Example: 1.0*10^23 (this notation means 1.0 1023)