Instruction: Show your solutions. Observe significant figures.1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO,solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below.4(NH2)2CS + Hg² [(NH2)>CS]«Hg²•What is the percentage of (NH2)2CS in the sample?2. A 0.4912-g sample of a petroleum product was burned in a tube furnace, and the SO2produced was collected in H2O2.SO2@) + H2O2 - H2SO4A 25.00-mL portion of 0.00873 M NAOH was introduced into the solution of H2SO4, followingwhich the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfurconcentration in parts per million.3. A 100.0 mL sample of ground water was treated to convert the iron present to Fe2. Additionof 25.00 mL of 0.002412 M K2Cr2O7 resulted in the reaction below.6FE2+ + Cr2O,2+ 14H* → 6FE3+ + 2Cr³+ + 7H;OThe excess K2Cr2O7 was back-titrated with 8.12 mL of 0.00859 M Fe2• solution. What is theconcentration of Fe in the sample in parts per million?4. A 10.00 mL portion of an HCI solution required 11.01 mL of 0.09883 M NAOH to reach an endpoint with phenolphthalein.HCI + NaOH –→ NaCI + H2OCalculate the molar concentration of HCI.5. Describe the preparation of 2.50 L of 0.500 M HCIO4, starting with a 9.00 M solution of thereagent.

1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO, solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below. 4(NH2)2CS + Hg2 - [(NH2)2CS]«Hg² What is the percentage of (NH2)2CS in the sample?

1. The thiourea in a 1.455 g sample of an organic material was extracted into a dilute H2SO, solution and titrated with 37.31 mL of 0.009372 M Hg²* via the reaction below. 4(NH2)2CS + Hg2 - [(NH2)2CS]«Hg² What is the percentage of (NH2)2CS in the sample?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 10E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
4. A 0.1036-g sample containing only BaCl2 and NaCl is dissolved in 50 mL of distilled water. Titrating with 0.07916 M AgNO3 requires 19.46 mL to reach the Fajans endpoint. Report the %w/w BaCl2 in the sample.
what is the product of the reaction of concentrated ammonia and ammonium carbonate? NH3 + (NH4)2CO3=? to the product of the above reaction then slowly added to an aqueous solution of CoSO4∙H2O.(Cobalt sulfate) Initially, a precipitate formed? What would be the precipitate? It was not CuSO4.The question is asking about the CoSO4 An aqueous solution of ammonium carbonate was slowly added to concentration ammonia to make Solution A. Solution A was then slowly added to an aqueous solution of CoSO4∙H2O. Initially, a precipitate formed (Product 1), which dissolved upon further addition of Solution A, giving a red Solution B
Q5: A sample of 0.676g of an unknown compound containing barium ions (Ba+) is dissolved in water and treated with an excess of NazSO. If the mass of BasO, precipitate formed is 0.4105g. What is the percent by mass of Ba in the original unknown compound? Note: Mwt. of Ba =32, Mwt. of BaSo4 =233, Mwt. of Na2SO4=142
Directions: Solve the problem with a complete step-by-step solution. Titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? The chemical reaction is 2MnO4- + 5C2O42- + 16H+ + ----> 2Mn2+ + 10CO2 + 8H2O
1. Determine the mass of CaCl2·2H2O (MW 147.02 g/mole) to weigh out using a four- place analytical balance to prepare 100 mL of a 0.1005 M solution of Ca2+. 2. Determine the mass of KCI to weigh out using a four-place analytical balance to prepare 100 mL of a 1 M solution of KCI (MW 74.5513 g/mole). 3. Record the solubility of calcium carbonate in water (mg/L) in your notebook. 4. Calculate the amount of calcium carbonate (mg) not in solution if a tablet is dissolved in 250 mL of water and the tablet's label claim is 600 mg calcium / tablet.
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.
You may want to reference (Page 834) Section 18.3 while completing this problem. Part A If 130.0 mL of 0.0020 M Na2SO4 (aq) is saturated with CaSO4, how many grams of CaSO4 would be present in the solution? [Hint. Does the usual simplifying assumption hold?] Express your answer using two significant figures. VE ΑΣΦ ? m = 0.43 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining g
Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. How many moles of HCl was added initially to digest the limestone sample? How many moles of CaCO₃ is present in the limestone sample? What is the purity of the limestone in terms of %w/w CaCO₃?
A solution was prepared by dissolving 1210 mg of K3 Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate 1. the molar analytical concentration of K3Fe(CN)6 2. the molar concentration of K+ 3. the molar concentration of Fe(CN)2- 4. the weight/volume percentage of K3 Fe(CN)6 5. the number of millimoles of K+ in 50.0 mL of this solution 6. ppm Fe(CN)2- 7. the normal analytical concentration of K3Fe(CN)6 8. pK+ for the solution 9. pFe(CN)6 for the solution
Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the solubility in mol/L at 20oC and at 60oC? How many milliliters (mL) of 0.045 M Na2S2O3 will be required to titrate a 10.0-mL sample of saturated Ca(IO3)2 solution collected at 20oC and 60oC, respectively?
(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)