Write balanced net ionic equations for all precipitation reactions observed. ard.com/webapps/assessment/take/launch.jsp?course_assessment_id=_282182_1&uestion Completion Status:Record your observations in the data table below. If no precipitate forms write NR for no reactioAGNO3 (Ag*)Pb(NO3)2 (Pb2*)f. Whitea. PinkNazCO3 (CO32)b. Dark Browng. BlackNazs (s2)NaOH (OH-)C. Brownh. NRd. NRi. NRNazSO4 (SO42)NaCl (CI")e. Whitej. WhiteQUESTION 2Record your observations in the data table below. If no precipitate forms write NR for no reactioCa(NO3)2 (Ca2*)k. WhiteNazCO3 (CO32)Nazs (s2)I. NRNaOH (OH-)m.WhiteNa2SO4 (SO42)n. NRNaCI (CI")o. NRQUESTION 3Click Save and Submit to save and submit. Click Save All Answers to save all answers.

ard.com/webapps/assessment/take/launch.jsp?course_assessment_id=_282182_1= estion Completion Status: Record your observations in the data table below. If no precipitate forms write NR for no reactic AGNO3 (Ag*) Pb(NO3)2 (Pb2*) а. Pink f. White NazCO3 (CO32) Na2s (s2) b. Dark Brown g. Black NaOH (ОH-) c. Brown h. NR NazSO4 (SO42) d. NR i. NR NaCI (CI") e. White j. White

ard.com/webapps/assessment/take/launch.jsp?course_assessment_id=_282182_1= estion Completion Status: Record your observations in the data table below. If no precipitate forms write NR for no reactic AGNO3 (Ag) Pb(NO3)2 (Pb2) а. Pink f. White NazCO3 (CO32) Na2s (s2) b. Dark Brown g. Black NaOH (ОH-) c. Brown h. NR NazSO4 (SO42) d. NR i. NR NaCI (CI") e. White j. White

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.18QAP

See similar textbooks

Similar questions

A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-Nickel ion required 11.70 mL of 0.002146 M EDTAWhat is the percentage of NaBr (102.894) in the 1.000 g sample?
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA. Calculate mmol Ni in the 50.00 mL aliquot. Calculate mmol Br- in the 50.00 mL aliquot. Calculate the percentage of NaBr (102.894) in the 1.000 g sample.
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA The other 50.00 mL remaining solution was also analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) g) Compute for Eind. h) Compute pBr in the 50.00 mL aliquot. i) Compute for % NaBr ( in the potentiometric technique). j) Calculate the error between the obtained % NaBr fr the EDTA titration technique and the % NaBr from the potentiometric technique.
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-50.00 mL remaining solution was analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. a) Write the cell notation of the potentiometric set-up with SCE as the reference electrode. b) Write the Nernst equation that describes the indicator electrode set-up. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) c) Compute for Eind. d) Compute pBr in the 50.00 mL aliquot. e) Compute for % NaBr ( in the potentiometric technique).
A sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data: Wt of sample = 0.5000g; Vol of AgNO3 added = 35.00ml; M of AgNO3 = 0.1157; Vol of SCN- used for back titration = 14.71ml; M of SCN- = 0.08598; Atomic wts: Ag = 107.87, N = 14.00, Cl = 35.5, O = 16.00
A limestone sample weighing 400 mg was dissolved in acid treated with excess sodium oxalate. The solution was made basic and the resulting calcium oxalate was filtered, washed and redissolved in dilute acid. This solution required 14.0 mL of 0.00865 M KMnO4. What is the % Ca of the limestone. CaC2O4(s) + 2H+ ⇌ Ca2+ + H2C2O45H2C2O4 + 2MnO4- + 6H+ ⇌ 10CO2 + 8H2O + Mn2+
When I was a boy, I watched Uncle Wilbur measure the iron content of runoff from his banana ranch. He acidified a 25.0-mL sample with HNO3 and treated it with excess KSCN to form a red complex. (KSCN itself is colorless.) He then diluted the solution to 100.0 mL and put it in a variablepathlength cell. For comparison, he treated a 10.0-mL reference sample of 6.80 3 1024 M Fe31 with HNO3 and KSCN and diluted it to 50.0 mL. The reference was placed in a cell with a 1.00-cm pathlength. Runoff had the same absorbance as the reference when the pathlength of the runoff cell was 2.48 cm. What was the concentration of iron in Uncle Wilbur’s runoff ?
A (3.6500 g) of impure ammonium aluminium sulfate (NH4Al(SO4)2)) was treated with ammonia (NH3(aq)) producing hydrous alumina Al2O3.xH2O. The collected precipitate was filtered, washed, and ignited at 1000 °C to give 0.4935 g Al2O3 (Mw 101.9635 g/mol). Determine: a. % Al2O3 b. %Al c. Express concentration of Al in ppm.
A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.
The bismuth (AW 208.98) in 0.6805 g of an alloy was precipitated as BiOCl (FW 260.43) and separated from the solution by filtration. The washed precipitate was dissolved in nitric acid and treated with 15.02 mL of 0.1498 M AgNO3, causing the precipitation of AgCl. The excess AgNO3 required 14.04 mL of 0.1008 M KSCN for titration. Calculate %Bi in the sample.The bismuth (AW 208.98) in 0.6805 g of an alloy was precipitated as BiOCl (FW 260.43) and separated from the solution by filtration. The washed precipitate was dissolved in nitric acid and treated with 15.02 mL of 0.1498 M AgNO3, causing the precipitation of AgCl. The excess AgNO3 required 14.04 mL of 0.1008 M KSCN for titration. Calculate %Bi in the sample.
A solid sample containing chloride and with a mass equal to 6.000 g was dissolved in water and transferred to a 100.0 ml flask. A 50.0 mL aliquot of this solution was diluted to 250.0 mL. In the titration of 20.0 mL of the diluted solution, 32.0 mL of 0.2000 mol L-1 AgNO3 standard solution were used. Calculate the % of impurities in the analyzed sample. Data: Cl = 35.45
Complex Ion Formation and Precipitation Reactions i. A 1-L water sample was submitted for determination of chloride ion. 100.00mL the sample was analyzed using the Volhard method. 50.00 mL of 0.0929N AgNO3 was added to the sample and was back titrated with 12.50mL of 0.0510N KSCN solution to reach the end point. Find ppm Cl- in the water sample. ii. Using Mohr method, the chloride content of a mineral water was determined. 50.00mL of the sample was titrated with 10.80mL of 0.05N AgNO3 solution to reach end point. Determine the concentration of Cl- in ppm. iii. Calculate the hardness of a water sample such that 100.00mL of the sample required 35.00mL of 0.1051M EDTA solution to reach the end point.