(a)
Interpretation:
The equation for
Concept introduction:
The equation for
Here,
(b)
Interpretation:
The total charge needed to strip the silver from the electrode needs to be determined. Also, the volume of the solution used to deposit the silver needs to be determined,
Concept introduction:
The equation for
Here,
(c)
Interpretation:
The experiments need to be suggested to show whether all the
Concept introduction:
Linear scale voltammetry is used to compare the data for the metal reduction in the deposition step.
(d)
Interpretation:
Whether it matters when the shape of the drop is hemisphere or not needs to be explained.
Concept introduction:
Visual measurement of droplet which is spherical or hemispherical in shape.
(e)
Interpretation:
The alternative method for testing against the proposed method needs to be suggested.
Concept introduction:
Volume of the sphere or volume of the hemisphere can be calculated as follows-
Where
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Principles of Instrumental Analysis
- A conductivity cell was calibrated using 0.01 M KCl (κ = 1.4087x10-3 S/cm) and the measured resistance was 688 Ω. a. Determine the cell constant (include units). b. Determine the molar conductivity, Λm for a 0.0100 M AgNO3 solution in the same cell with a resistance reading of 777Ω.arrow_forward) 0.025 M CH3COOH solution has a specific conductance of 2.33X10-4 Scm-1,and molar conductivity at infinite dilution is 364.13 S.Cm2.mol-1. What is itsdegree of dissociation?arrow_forwardIs a quantitative separation of Zn2+ and Ag+ by electrolytic deposition feasible in principle? If so what range of cathode potential versus that saturated calomel electrode can be used? Assume that the solution is initially 0.1000M in each ion and that quantitative removal of an ion is realized when only 1 part in 1000 remains undeposited E0reduction of Zn2+ = -0.76V E0oxidation of Ag = -0.8Varrow_forward
- A sample of steel (0.506 g) was digested in acid and the solution made up to 100 cm3 with deionised water. Aliquots (25.0 cm3) of this solution were transferred into two volumetric flasks (100 cm3) labelled A and B. Flask A was made up to volume with deionised water. To flask B was added 10.0 cm3 of a 260 ppm standard solution of Mn2+ which was then also made up to volume with deionised water. The following absorbance results were obtained: Solution A = 0.356, Solution B = 0.578. Use these results to calculate the percentage (% w/w) of manganese in the steel sample.arrow_forwardAn ion selective electrode is utilised to determine the concentration of Ca2+ in the presence of Mg2+. The selectivity coefficient for the electrode kij is 0.015. If the concentrations of Ca2+ and Mg2+ are 50 and 500 ppm, respectively, calculate the change in potential (in mV) when the temperature of the measurement cell is increased from 20oC to 40oC.arrow_forwardHow long will it take to dissolve 2 mg of metal A (atomic weight 100) in a solution containing A2+ from a metal electrode with area of 1.5 cm2 at an overpotential of = 0.2 V? The exchange current density (j0) for A is 3x10-3 A/cm2, the temperature T=298 K and the symmetry factor =0.4.arrow_forward
- b) In one conductivity cell, the resistance of a 0.1 M KCl solution is 1.5x102 Ω. The knownmolar conductivity of the solution is 101 Ω-1 cm2 mol-1 . Calculate the cell constant, Kcell. (Kcell unit is cm-1).arrow_forward1) Name the applications of glass electrodes in potentiometric measurements (please write correctly and concisely).arrow_forwardThe classical dissociation constant of propionic acid, C2H5CO2H, is 1.34 x10-5 moldm-3 at 250C and the limiting molar conductivities at zero concentration of hydrogen and propionate ions are 349.8 and 35.8 ohm-1 cm2 mol-1 respectively. Calculation of the resistivity of 0.100 M solution of propionic acid.arrow_forward
- The resistances of a series of aqueous NaCI solutions, formed by successive dilution of a sample, were measured in a cell with cell constant (the constant C in the relation κ = C/R) equal to 0.2063 cm-1. The following values were found: c/(mol dm-3) 0.00050 0.0010 0.0050 0.010 0.020 0.050R/Ω 3314 1669 342.1 172.5 89.08 3714(a) Verify that the molar conductivity follows the Kohlrausch law and find the limiting molar conductivity. (b) Determine the coefficient κ, (c) Use the value of κ (which should depend only on the nature, not the identity of the ions) and the information that λ(Na+) = 5.01 mS m2 mol-1 and , λ(I-) = 768 mS m2 mol-1, to predict (i) the molar conductivity, (ii) the conductivity,(iii) the resistance it would show in the cell, of 0.010 mol dm-3 Nal(aq) at 25 °C.arrow_forwardThe reciprocal of molar conductivity is plotted as a function conductivity for a data set. The slope ofthe fitted line is 35800 S−2 m−1 mol, while its intercept is 42.3 S−1 m−2 mol. Calculate the dissociationconstant of the weak acid.arrow_forwardThe conductivity of 0.20 M solution of KC1 at 298 K is 0.025 S cm-1. Calculate its molar conductivity.arrow_forward
- Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning