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?
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- 1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.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. A. How many moles of HCl was added initially to digest the limestone sample? B. How many moles of CaCO₃ is present in the limestone sample? C. What is the purity of the limestone in terms of %w/w CaCO₃?This is an unknown solution which comprises of several ions possible for analysis. From the given information, determine which ions are present. Use + for positive, - for negative, or ? for insufficient information. An unknown solution containing the ions listed to the right was found: For Group I Cations: 1). A white precipitate was generated when 2 drops of 6M HCl solution was added to the unknown solution test tube. 2). Di water was added to the solution from part 1, and then the ppt was separated from the supernatant. The ppt was then washed with DI water few times to make sure is ppt is clean. 3). On the ppt separated from part 2 excess 6M NH3 was added and as a result all the ppt was dissolved. For Group III Cations: 4). An addition of Excess 6M NH3 led to a basic solution and a ppt. The ppt was then separated from the supernatant. 5). When Excess 6M NaOH was…
- Prepare 100.00 mL of a solution with ALL the following chemicals into together; CHEMICALS PROVIDED solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations needed in the 100mL solution FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.Pls do fast and i will rate instantly for sure Solution must be in typed form A 25.0 mL volume of 0.0106 M KIO3 is pipetted into a 250-mL Erlenmeyer flask. The solution is titrated to the stoichiometric point with 16.25 mL of a sodium thiosulfate solution. What is the molar concentration of the sodium thiosulfate solution?
- What weight of the soda ash (impure Na2CO3) should be taken for analysis in order that the number of milliliters of 0.500 N acid used will be equal to one-half of the percentage of Na2CO3 in the sample? Note: Please include the complete solution. Thanks!1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.
- When standardizing two liters of a potassium permanganate solution with a primary standard solution of sodium oxalate, approximately 0.0100 M, it was planned to use between 30.00 mL and 45.00 mL of the titrated reagent. In which mass range (in grams) the primary standard should be weighed? Data: MM KMnO4 = 158.00 g/mol; MM Na2C2O4 = 134.00 g/mol 2CO2 + 2e- ↔ C2O4 2- Eo = -0,432 V MnO4 - + 8 H+ + 5e- ↔ Mn2+ + 4 H2O Eo = 1,52 VPrepare 1.0 L of a 50.00 ppm iron solution from the solid Fe(NH4)2(SO4)2 of the80.0% purity. Clearly describe how to prepare this solution. If doneChlorimetric iron analysis using the calibration curve method, specify theform of preparation of 100.0 ml of each of the following standard solutions withcontents of 1.00, 5.00, 15.00 and 20.00 ppm of Fe respectively from the solutionmother (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)The 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 below. Find the percentage of (NH2)2CS (76.12 g/mol) in the sample. 4(NH2)2CS + Hg2+= (NH2)2CS 4Hg2+