(a)
Interpretation:
Whether the reaction
Concept introduction:
Major objective of qualitative cation analysis is identifying the cations present in a mixture. In qualitative cation analysis, cations are categorized into 5 groups depending on the solubilities of their compounds. Pb2+, Hg22+, Ag+ belong to the first group which form insoluble chlorides when HCl(aq) is added. When the remaining solution is added with H2S in an acidic medium(0.3 M HCl), a group of sulfides precipitate. The remaining solution from this is next treated with H2S in a buffer mixture of NH3 and NH4+ ions which then gives a mixture of insoluble hydroxides and sulfides. Filtrate of above reaction mixture is then treated with CO32-. This yields carbonate precipitates of cations. In the final solution, all the water soluble cations include.
(b)
Interpretation:
Whether the reaction
Concept introduction:
Major objective of qualitative cation analysis is identifying the cations present in a mixture. In qualitative cation analysis, cations are categorized into 5 groups depending on the solubilities of their compounds. Pb2+, Hg22+, Ag+ belong to the first group which form insoluble chlorides when HCl(aq) is added. When the remaining solution is added with H2S in an acidic medium (0.3 M HCl), a group of sulfides precipitate. The remaining solution from this is next treated with H2S in a buffer mixture of NH3 and NH4+ ions which then gives a mixture of insoluble hydroxides and sulfides. Filtrate of above reaction mixture is then treated with CO32-. This yield carbonate precipitates of cations. In the final solution, all the water soluble cations include.
(c)
Interpretation:
Whether the reaction
Concept introduction:
Major objective of qualitative cation analysis is identifying the cations present in a mixture. In qualitative cation analysis, cations are categorized into 5 groups depending on the solubilities of their compounds. Pb2+, Hg22+, Ag+ belong to the first group which form insoluble chlorides when HCl(aq) is added. When the remaining solution is added with H2S in an acidic medium (0.3 M HCl), a group of sulfides precipitate. The remaining solution from this is next treated with H2S in a buffer mixture of NH3 and NH4+ ions which then gives a mixture of insoluble hydroxides and sulfides. Filtrate of above reaction mixture is then treated with CO32-. This yield carbonate precipitates of cations. The final solution includes all the water soluble cations.
(d)
Interpretation:
Whether the reaction
Concept introduction:
Major objective of qualitative cation analysis is identifying the cations present in a mixture. In qualitative cation analysis, cations are categorized into 5 groups depending on the solubilities of their compounds. Pb2+, Hg22+, Ag+ belong to the first group which form insoluble chlorides when HCl(aq) is added. When the remaining solution is added with H2S in an acidic medium (0.3 M HCl), a group of sulfides precipitate. The remaining solution from this is next treated with H2S in a buffer mixture of NH3 and NH4+ ions which then gives a mixture of insoluble hydroxides and sulfides. Filtrate of above reaction mixture is then treated with CO32-. This yield carbonate precipitates of cations. In the final solution, all the water soluble cations include.
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
General Chemistry: Principles and Modern Applications, Loose Leaf Version (11th Edition)
- A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forwardAt 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)arrow_forwardIn some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.arrow_forward
- An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forwardAn aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning