insdelNAMEDATESECTIONPOSTLABORATORY ASSIGNMENT1. An "iodide/chloride/sulfate" unknown solution gave a yellow precipitate with aqueous AgNO3,.and after centrifuging, the supernate gave no reaction with aqueous Ba(NO3)2. The yellowprecipitate did not dissolve in aqueous NH4OH, and adding aqueous HNO3 gave no reaction.State the anion(s) confirmed present and absent in the unknown solution.Anion(s) presentAnion(s) absent2. An "iodide/chloride/sulfate" unknown solution gave a white precipitate with aqueous AgNO3,and after centrifuging, the supernate gave a white precipitate with aqueous Ba(NO3)2. Theoriginal white precipitate dissolved completely in aqueous NH,OH, and produced a whiteprecipitate after adding aqueous HNO3. State the anion(s) confirmed present and absent in theunknown solution.Anion(s) absentAnion(s) presentnonoatomic anions.

The precipitates which can be formed in this reaction are silver iodide, silver chloride or silver…

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.34QAP

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1S Refer 2. An "iodide/chloride/sulfate" unknown solution gave a white precipitate with aqueous AgNO3, and after centrifuging, the supernate gave a white precipitate with aqueous Ba(NO3)2. The original white precipitate dissolved completely in aqueous NH4OH, and produced a white precipitate after adding aqueous HNO3. State the anion(s) confirmed present and absent in the unknown solution. Anion(s) present Anion(s) absent
2.413 g sample contains Na2CO3, NaHCO3 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 NaHCO3 and Na CO in sample (Na CO =106.0 g/mol, NaHCO =84.02 g/mol)
[Review topics] Use the References to access important values if needed for this question. [References] When 22.0 mL of a 6.65×10-4 M iron(II) bromide solution is combined with 22.0 mL of a 6.38×10-4 M ammonium sulfide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to Submit Answer Retry Entire Group 9 more group attempts remaining
A mixture of NaBr, Nal and NaNO3 weighs 0.6500 g. With AgNO3, a precipitate of the two halides is obtained and is found to weigh 0.9390 g. When heated in a current of C12, the precipitate is converted entirely to AgCl weighing 0.6566 g. What is the %NaNO3 in the original sample?
The reaction Cu(s) + HNO3(ag) Cu(NOsh(ag) + 2 NO:) +2 H;O() is used to dissolve the copper metal Ifa 1.000 g sample of copper is used, and instructions say to use four times as much acid as the required amount, how many mL (to the nearest mL) of 15.0 M nitric acid would be used in the procedure for this sample? Select one: O a 10mL Ob 17ml O c.4mL O d 25ml O e 5mL
The level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.
A 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.
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?
17. Balance the following equation occurring in an acidic aqueous solution. Show all steps relating to the balancing method. (6) AsH3 + Zn²+ ->> H₂ASO4 + Zn
Explain in four ways what happens when 25 mL of unknown AgNO3 in an Erlenmeyer flask is added with NaCl solution until no further AgCl precipitate is formed. Describe the reaction.
0.890 g KIO3 was dissolved to give a 80.00 mL Iodate solution. 35.00 mL aliquot reactedwith the iodide to form triiodide. The liberated triiodide was titrated and consumed 11.65 mL of theS2O32- solution to reach endpoint. Calculate the concentration in molarity of the Na2S2O3solution.
(9) Carive the not ignic cavation for the reaction when aqueous Solution of barium Sulfide and zinemitrate. (b) Crive the net wonic cavation for Potassium Carbonate and aluminum acetate. GIVE EXPTAINED HANDWRITTEN ANSWER

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