A domestic water pipe is suspected to be contaminating drinking water with lead.In order to test this hypothesis, a section of the pipe is leached for 24 hours using120.0 mL of 4% acetic acid. A 40.00-mL aliquot of the leachate is transferred toan electrochemical cell and 10.00 mL of a 0.200 mM standard solution of Cďd²+ isbo added (as an internal standard). A stripping analysis of the solution yields peakcurrents of 1.81 µA for lead and 2.18 µA for cadmium. Analysis of a standardsolution that is 0.0600 mM in Pb2t and 0.0500 mM in Cd2+ gives peak currents of2.39 µA and 2.71 µA, respectively, under the same conditions. What is theconcentration of Pb²+ in the original leachate?13.

A domestic water pipe is suspected to be contaminating drinking water with lead. In order to test this hypothesis, a section of the pipe is leached for 24 hours using J120.0 mL of 4% acetic acid. A 40.00-mL aliquot of the leachate is transferred to Man electrochemical cell and 10.00 mL of a 0.200 mM standard solution of Cď²+ is added (as an internal standard). A stripping analysis of the solution yields peak currents of 1.81 µA for lead and 2.18 µA for cadmium. Analysis of a standard solution that is 0.0600 mM in Pb2t and 0.0500 mM in Cd²* gives peak currents of 2.39 µA and 2.71 µA, respectively, under the same conditions. What is the çoncentration of Pb2+ in the original leachate? 13.

A domestic water pipe is suspected to be contaminating drinking water with lead. In order to test this hypothesis, a section of the pipe is leached for 24 hours using J120.0 mL of 4% acetic acid. A 40.00-mL aliquot of the leachate is transferred to Man electrochemical cell and 10.00 mL of a 0.200 mM standard solution of Cď²+ is added (as an internal standard). A stripping analysis of the solution yields peak currents of 1.81 µA for lead and 2.18 µA for cadmium. Analysis of a standard solution that is 0.0600 mM in Pb2t and 0.0500 mM in Cd²* gives peak currents of 2.39 µA and 2.71 µA, respectively, under the same conditions. What is the çoncentration of Pb2+ in the original leachate? 13.

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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The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?
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You have been asked to determine the empirical formula of an iron(?) nitrate salt, Fe(NO). You weigh out 4.1419 g of a solid iron(?) nitrate sample and dissolve it with DI-HO while filling to the calibration mark of a 250.00 mL volumetric flask. You then use an ion-selective electrode to determine the iron ion concentration, which gives a reading of 3910 mg Fe^?+/L . Calculate the empirical formula of your iron(?) nitrate sample. (Hint-Assume that the remaining percent of ions in solution are nitrate ions.)
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You have been asked to determine the empirical formula of an iron(?) nitrate salt, Fe(NO). You weigh out 4.1419 g of a solid iron(?) nitrate sample and dissolve it with DI-HO while filling to the calibration mark of a 250.00 mL volumetric flask. You then use an ion-selective electrode to determine the iron ion concentration, which gives a reading of 3910 mg Fe^7+/L . Calculate the empirical formula of your iron(?) nitrate sample. (Hint-Assume that the remaining percent of ions in solution are nitrate ions.)
Two Copper strips were used to determine the effect of electrolysis time and immersed in 3.080g of Cu (NO3)2 dissolved in 25mL of DI water. The weight of one copper strip act as an anode is taken before the reaction and after the reaction to calculate the change in mass. 1.0A of current and 7.50 V is used throughout the experiment Calculate the theoretical mass that should be obtained at each time interval and Compares the theoretical mass (mg) of copper and the actual mass deposited (obtained from the electrolysis, ∆m) by calculating the %error at different times. Briefly discuss the observed results. Is there any trend observed? Positive Anode (Copper strip): Cu(solid) ®Cu2+(aqueous)+2e- Negative Cathode(Copper strip ): Cu2+(aqueous)+2e- ®Cu(solid) Time interval (min) 2.5 5.0 7.5 10 Initial mass of strip (mg) 3432 3390 3297 3141 Final mass of strip (mg) 3390 3297 3141 2939 Mass change Dm (mg) 44 93 156 202 Michael Faraday…
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