Experiment 1. Determination of sulfate ions in potassium sulfate Precipitate sulfate ions of potassium sulfate as barium sulfate, filter it, burn it in a crucible, and find the weight by gravimetric analysis. 0.3951 g of K2SO, was weighed precisely, 2 mL of HCI (1+1) was added, and then it was dissolved completely by heating. A 1% BaCl2 solution was added slowly, and whether BaSO4 precipitated or not was checked. (1) Calculate the minimum amount (mL) of the 1% BaCl2 solution required to allow BaSO4 to completely precipitate. Suppose that the concentration of the BaCl2 solution is 1 wt/vol %.

Experiment 1. Determination of sulfate ions in potassium sulfate Precipitate sulfate ions of potassium sulfate as barium sulfate, filter it, burn it in a crucible, and find the weight by gravimetric analysis. 0.3951 g of K2SO, was weighed precisely, 2 mL of HCI (1+1) was added, and then it was dissolved completely by heating. A 1% BaCl2 solution was added slowly, and whether BaSO4 precipitated or not was checked. (1) Calculate the minimum amount (mL) of the 1% BaCl2 solution required to allow BaSO4 to completely precipitate. Suppose that the concentration of the BaCl2 solution is 1 wt/vol %.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 37QAP: An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is...

See similar textbooks

Similar questions

Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
2.23 gr sample taken from a bleaching powder is dissolved and completed to 250 ml. Taken from here 25One ml of sample is titrated with 33.02 ml of 0.1158 N Na2S2O3 solution after the necessary procedures. Bleachingactive chlorine in powder (OClCalculate the amount and percentage. (OCl: 51.5 g / mol)
A 12.63 g sample of calcium ore was dissolved in HCI and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 * H2O The precipitate was filtered. washed, dried, and ignited at 500 degrees C until the weight was constant, giving a final mass of 2.35 grams pure CaCo3 (100.087g /mol) Calculate the % Calcium 140.078g / mol in the sample.
3) 2.413 g sample contains Na CO̟, NaHCO and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO¸ and 3 Na CO in sample (Na CO_=106.0 g/mol, NaHCO_=84.02 g/mol). 3
WHAT VOLUME OF 0.107 N SILVER NITRATE IS REQUIRED TO TITRATE THE SODIUM CHLORIDE IN 4.0 G SAMPLE OF SODIUM LAURYL SULFATE? THE SAMPLE CLAIMS TO HAVE 6.8% NACL. WORKING FORMULA: %CONTENT = ((N X ML X MEQ)/WT.G) X 100
A solution of HClO4 was standardized by dissolving 0.4008 g ofprimary-standard-grade HgO in a solution of KBr: HgO(s) + 4Br- + H2O → HgBr4 2- + 2OH- The liberated OH2 consumed 43.75 mL of the acid. Calculate themolar concentration of the HClO4.
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
A 0.6560 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water. AgNO3 was added to the solution, precipitating all of the CN− in solution as AgCN (MW=133.886 g/mol). The dried precipitate weighed 1.505 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt% = ~ 66.01 NaCN wt% = ?
b) A solution was prepared by dissolving 1.5 g of Acetic acid (CH,COOH) in a 250cm solution. 50cm of this solution was allowed to react with 25cm of 0.1 NaOH solution (C-12, H-1, O-16) i) Determine the concentration of the acetic acid solution in moldm ii) iii) Write down an equation for the reaction. Calculate the number of moles of CH,COOH left unreacted and the number of moles of CH,COONA formed. iv) What name is given to the solution formed when all the NaOH has reacted? Calculate the Pp" of the solution in (iv) above (ka for CH,COOH = 1.8 x 10)
A 0.1064-g of aldrin pesticide sample was decomposed and the liberated chloride was extracted using water. It was titrated with 23.28 mL of 0.03337 M AgNO3 using a chromate indicator. Express results in % aldrin (C12H8Cl6, MM=365).
A solution contains 8.86×10-³ M ammonium carbonate and 5.11×10-³ M sodium fluoride. Solid lead acetate is added slowly to this mixture. What is the concentration of carbonate ion when fluoride ion begins to precipitate? [carbonate] M Submit Answer = Retry Entire Group 9 more group attempts remaining