The concentration of copper in a sample of sea water is determined by anodic stripping voltammetry using the method of standard additions. The analysis of a 100.0 mL sample gives a peak current of 0.905 μA. After adding a 5.00-μL spike of 25.0 mg.L-¹ Cu ²+, the peak current increases to 3.32 µA. Calculate the µg.L-¹ copper in the sample of sea water.

The concentration of copper in a sample of sea water is determined by anodic stripping voltammetry using the method of standard additions. The analysis of a 100.0 mL sample gives a peak current of 0.905 μA. After adding a 5.00-μL spike of 25.0 mg.L-¹ Cu ²+, the peak current increases to 3.32 µA. Calculate the µg.L-¹ copper in the sample of sea water.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A galvanic cell was constructed with a nickel electrode that was dipped into 1.3 M NISO4 solution and a chromium electrode that was immersed into a solution containing Cr³+ at an unknown concentration. The potential of the cell was measured to be 0.564 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr³+ in the solution of unknown concentration? [Cr³+] = i M
Determine the amount of time (in hours) that a 16.8 ampere current must be applied to a 2.0 ZnCl2(aq) solution to produce 435.2 g of Zn(s).
A hydrogen electrode is immersed in a 2.0 M solution of acetic acid at 25 °C. This electrode is connected to another consisting of an iron nail dipping into 2.0 M FeCl2. What will be the measured potential of this cell? Assume PH2 = 1.00 atm. Ecell = i V
1. A concentration cell is constructed using two metal (M) electrodes with M 2+ concentrations of 0.10 M and 1.00 × 10 –5 M in the two half-cells. Determine the reduction potential of M 2+ given that the potential of the cell at 25°C is 0.118 V.a. 0 Vb. +0.118 Vc. –0.118 Vd. Cannot be determined with the information given.e. None of the above.
A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for 15.5 h. What mass of Mg is produced? g
A pure organic acid sample (0.1516 g) is neutralized with OH- ions produced in a constant current of 0.401 A in 5 minutes and 24 seconds. Calculate the equivalent weight of the acid.
what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52 h?
In the electroplating of nickel from a solution containing Ni2+ ions what weight of nickel-metal will be produced at the cathode by a current of 4.02 A flowing for 100 min?
An unstirred solution of 2.00 M NaCl was electrolyzed for a period of 28.9 min and then titrated with 0.314 M HCl. The titration required 21.7 mL of the acid. What was the average current in amperes during the electrolysis?