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- 6. The mercury in a 0.839 g sample was precipitated with an excess paraperiodic acid, H¿IO, 5Hg + 2H,IO, → Hg;(IO,); + 10H The precipitate was filtered, washed free of precipitating agent, dried and weighed, 0.3408 g being recovered. Calculate the percentage of Hg,Cl, in the sample.6-20. A 4.476-g sample of a petroleum product was burned in a tube furnace, and the SO, produced was col- lected in 3% H,O2. Reaction: SO-(g) + H;O, → H,SO4 A 25.00-mL portion of 0.00923 M NaOH was intro- duced into the solution of H,SO,, following which the excess base was back-titrated with 13.33 mL of 0.01007 M HCI. Calculate the parts per million of sulfur in the sample.7-11. Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.541 3 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCI, and heating to dissolve the solid and expel CO2: CACO3 (s) +2H* → Ca²* +CO,T +H2O Calcium carbonate FM 100.086 The excess acid required 39.96 mL of 0.100 4 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.
- The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.Tiame tests, the yello w colour oT sodium lons can mask the coIour of otner lons. Explain why blue glass is used to ldentity ions in the presence of sodium. Saved Normal B|I|U fx | | D E li Delete columnA 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
- mass Br- = 5.32 * 103* 79.904 = 0.4255 g. Os : What concentration Of Fez(SO4)3 (aq) is required for the olution to have [Fe*3 lag)] = 0.32M ? ) 0.16 M. %3D 0.080 M. 0.32 M.m/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take OWiv |Awgnment | Fir X OWI2 | Orline teaching x [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, K., for the following reaction is 1.80×104at 298 K. NH,HS(s) NH3(g) + H,S(g) If an equilibrium mixture of the three compounds in a 5.08 L container at 298 K contains 2.00 mol of NHLHS(s) and 0.339 mol of NH3, the number of moles of H,S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining Previous Next 11:2 10/15 ho 112 prt sc delete homeCaustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?
- Illegal mining affected many rivers with extremely high deposits of heavy metals and particulate matter in the river of America making them unwholesome for drinking. With the help of your knowledge on analytical separation and analysis outline suitable analytical protocol that can be employed to recover polluted river bodies and make them wholesome for drinking.What is the balanced equation for the combustion of C8H7NO2SBrCl in aC,H,N,S elemental analyzer?QUESTION 4 To prevent inclusion from occurring during precipitation, the technique to follow is I. fiter precipitate with less porous paper II. crystal growth be made to occur more slowly III. use of dilute analyte with concentrated precipitant IV. addition of soluble electrolyte O lonly IV only O I| & IV O I & III Il only