The following data were obtained for a complex of nickel at 575 nm in a 1.00 cm cell. Using Microsoft Excel or some other graphing program, construct a calibration plot and accurately calculate the molar absorptivity (ε) for the nickel-complex at 575 nm. Standard # 1 2 3 4 A. 0.184 M-1cm-¹ B. 0.002 M-¹cm-¹ C. 5.425 M-¹cm-1 Nickel Complex Concentration (M) 0.01 0.02 0.04 0.06 D. Not Enough Information to Determine Absorbance 0.058 0.109 0.220 0.328

The following data were obtained for a complex of nickel at 575 nm in a 1.00 cm cell. Using Microsoft Excel or some other graphing program, construct a calibration plot and accurately calculate the molar absorptivity (ε) for the nickel-complex at 575 nm. Standard # 1 2 3 4 A. 0.184 M-1cm-¹ B. 0.002 M-¹cm-¹ C. 5.425 M-¹cm-1 Nickel Complex Concentration (M) 0.01 0.02 0.04 0.06 D. Not Enough Information to Determine Absorbance 0.058 0.109 0.220 0.328

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

Chapter23: Potentiometry

Section: Chapter Questions

Problem 23.23QAP: The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300...

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The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
Explain why ionic attractions are weaker in media with high dielectric constants, e. g.,water and aqueous buffers.
When 8.0 ml of 0.00200M KSCN is mixed with 2.0 ml of 0.00200M Fe(NO3)3, the measured absorbance (A) at 450 nm is 0.285. The cell’s pathlength (b) is 1.0 cm; the absorptivity (ε) constant is 4700M-1cm-1. Calculate Kf for Fe(SCN) +2.
A conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!
Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard cuvette (1.00 cm light path) of 0.382. Calculate the mass of Co(NO3)2 contained in the original 50.0 mL stock solution.
A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 10.0 mL of a 0.100 M stock solution was added to 90.0 mL of solvent to make 100.0 mL of the first calibration standard solution and, secondly, 80 mL of that first calibration solution plus 20.0 mL of solvent were mixed to make the second calibration standard. What is the concentration of the second calibration standard solution?
The resistances of a series of aqueous NaCl solutions, formed by successive dilution of a sample, were measured in a cell with cell constant (the constant C in the relation K = C/R) equal to 0.2063 cm-1 and the following values were found at 25°C: c/(mol | 0.00050 0.0010 0.0050 0.010 0.020 | 0.050 dm-3) R/W 3314 1669 342.1 174.1 89.08 37.14 Find the molar conductance of Nacl at 25°C at infinite dilution from the graph.
Calculate the molar concentration of FeSCN2+ in solution #3. The determined molar absorptivity of the solution at 448 nm is 333 L mol-1 cm-1.
Estimate the Ka of a weak acid from the data given below. One gram quantities of the acid were dissolved in equal quantities of the various buffer solutions and all solutions were measured under the same conditions. The anion of the acid is the only species that absorbs at the wavelength used. pH: Abs: 4 0.0 5 0.0 6 0.06 7 0.39 8 0.95 9 1.13 10 11 1.18 1.18
A calibration curve for the colorimetric determination of phosphorous in urine is prepared by reacting standard solutions of phosphate with molybdenum(VI) and reducing the phosphomolybdic acid complex to produce the characteristic blue color. The measured absorbance A is plotted against the concentration of phosphorus. From the following data, determine the linear least-squares equation and calculate ppm P in the urine sample: ppm P 1.00 A 0.205 2.00 0.410 3.00 0.615 4.00 0.820 Urine sample 0.625 2.
4)The absorption of a 0.01 M complex solution in a 2.5 cm cell is measured as 0.5. Since the absorption of another solution in a 2 cm cell is 0.5, this What is the concentration of the solution?
By employing a given conductivity cell with 0.1N potassium chloride at 18pC, an observed conductance of 0.025 mho was obtained. What is the cell constant if the specific conductance of KCL at 18°C is 0.0112 mho.