Name Formula lonic/Covalent Soluble/Insoluble Electrolyte/Precipitate Ammonium Sulfide (NH4)2S Phosphorus Pentachloride PCI5 Silver Bromide AgBr Barium Sulfide BaS Strontium Sulfate SrSO4 Lithium Chlorite LICIO2 Iron (II) Sulfate FESO4 Sodium Na2Cr207 Dichromate Silver Acetate AGC2H3O2 Dinitrogen Pentahydride N2HS

Name Formula lonic/Covalent Soluble/Insoluble Electrolyte/Precipitate Ammonium Sulfide (NH4)2S Phosphorus Pentachloride PCI5 Silver Bromide AgBr Barium Sulfide BaS Strontium Sulfate SrSO4 Lithium Chlorite LICIO2 Iron (II) Sulfate FESO4 Sodium Na2Cr207 Dichromate Silver Acetate AGC2H3O2 Dinitrogen Pentahydride N2HS

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Show the clear and complete solution
Prepare 1.0 L of a 50.00 ppm iron solution from the solid Fe(NH4)2(SO4)2 of the80.0% purity. Clearly describe how to prepare this solution. If doneChlorimetric iron analysis using the calibration curve method, specify theform of preparation of 100.0 ml of each of the following standard solutions withcontents of 1.00, 5.00, 15.00 and 20.00 ppm of Fe respectively from the solutionmother (It suppose that the answers are: 0.3180, 2.00, 10.00, 20.00, 30.00 and 40.00 ml of the mother solution and dilute exactly to 100.0 mL with deionized water)
It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.
Solution of Pb(NO3)2 and NaCl are combined, resulting in concentrations of 0.0050 M Pb(NO3)2 and 0.00250 M NaCl immediately upon mixing. select the correct description of the final solution, given that the Ksp of PbCl2 is 1.7x10^-5. A) NaNO3 Precipitates B) All solutes reamin soluable C) Pb(NO3)2 precipitates D) PbCl2 precipiates E) All Solutes precipitate.
What is the molarity of a solution in which 150g of CaO are dissolved in 1900mL of solution? (Use thefollowing given information: overline MW:Ca=40g/mol , O=16g/molA. 1.41 mol/LB. 0.0014 mol/LC. 0.0014 MD. 1.41 m
The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
1. The standard solutions of iron(III) thiocyanate (solutions of known concentration) were prepared for you by mixing the solutions as shown in Table 1.a. Because of the very high concentration of KSCN used in each test tube, you can assume essentially all of the Fe(NO3)3 that has been added has reacted to form FeSCN2+ (by Equation 2, in the Background). Calculate the molar concentration of Fe(NO3)3 in each standard after it is diluted with the other solutions, which equals the concentration of FeSCN2+ formed in each sample (show your work for at least one of these calculations).These are the concentrations that were used in the standard curve. I have the table and the equation 2 on the top attached
When 25.00 mL of unknown were passed through a Jones reductor, molybdate ion (MoO4^2-) was converted into Mo3+. The filtrate required 16.43 mL of 0.010 33 M KMnO4 to reach the purple end point. MnO4- + Mo3+ --> Mn2+ + MoO2^2+. A blank required 0.04 mL. Balance the reaction and find the molarity of molybdate in the unknown.
Which among these is/are properties for the type of precipitate required in gravimetric analysis? Hygroscopic Known composition Reactive with atmospheric constituents Large particles
The salt content was extracted from a 12.0000 g junk food sample. The extract was diluted to 100.00 mL. From this solution, 15.00 mL was taken and required 23.75 mL of a 0.08943 M AgNO3 solution to reach the endpoint. What is the percentage by mass of salt as NaCl (58.45 g/mol) in the junk food sample?
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