The values for effective diameters and activity coefficients for ions at 25°C are given in the table below. Activity Coefficient at Indicated Ionic Strength Ion ax, nm 0.001 0.005 0.01 0.05 0.1 Ca2+, Cu2+, Zn2+, Sn2+, Mn2+, Fe 2+, Ni2+, Co2+, Phthalate² 0.6 0.870 0.748 0.676 0.48 0.40 Pb2+, CO3, SO32, C₂042 0.45 0.868 0.741 0.665 0.45 0.36 Al+, Fe+, Cr+, La+, Ce³+ 0.9 0.737 0.540 0.443 0.24 0.18 Th, Zr+, Ce+, Sn4+ 1.1 0.587 0.348 0.252 0.10 0.063 Use the Debye-Hückel equation 0.51Z√ -log Yx 1+3.3ax√√ to calculate the activity coefficient of a. Fe3+ at 0.024. Activity coefficient = b. Pb2+ at 0.013. = Activity coefficient = c. Ce at 0.089. = Activity coefficient =

The values for effective diameters and activity coefficients for ions at 25°C are given in the table below. Activity Coefficient at Indicated Ionic Strength Ion ax, nm 0.001 0.005 0.01 0.05 0.1 Ca2+, Cu2+, Zn2+, Sn2+, Mn2+, Fe 2+, Ni2+, Co2+, Phthalate² 0.6 0.870 0.748 0.676 0.48 0.40 Pb2+, CO3, SO32, C₂042 0.45 0.868 0.741 0.665 0.45 0.36 Al+, Fe+, Cr+, La+, Ce³+ 0.9 0.737 0.540 0.443 0.24 0.18 Th, Zr+, Ce+, Sn4+ 1.1 0.587 0.348 0.252 0.10 0.063 Use the Debye-Hückel equation 0.51Z√ -log Yx 1+3.3ax√√ to calculate the activity coefficient of a. Fe3+ at 0.024. Activity coefficient = b. Pb2+ at 0.013. = Activity coefficient = c. Ce at 0.089. = Activity coefficient =

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter11: Dynamic Electrochemistry

Section: Chapter Questions

Problem 10P

See similar textbooks

Similar questions

Calculate the ionic strength of a solution that is 0.0547M in Al2(SO4)3.
The metal cadmium tends to form Cd2+ ions. The followingobservations are made: (i) When a strip of zinc metal is placedin CdCl21aq), cadmium metal is deposited on the strip. (ii)When a strip of cadmium metal is placed in Ni1NO3221aq),nickel metal is deposited on the strip. (a) Write net ionicequations to explain each of the preceding observations.(b) Which elements more closely define the position of cadmiumin the activity series? (c) What experiments wouldyou need to perform to locate more precisely the position ofcadmium in the activity series?
Calculate the ionic strength of a solution that is 0.040 mol kg−1 in K3[Fe(CN)6](aq), 0.030 mol kg−1 in KCl(aq), and 0.050 mol kg−1 in NaBr(aq).
The cell SCE // Ag2CrO4 (sat'd), CrO42- (x M) / Ag is used for the determination of pCrO4. Calculate pCrO4 when the cell potential is 0.336 V.
Historically, chromium (Cr) has been used in numerous industrial processes, including leather tanning and metal plating operations. In these applications, if the water is mildly acidic, the Cr is typically present as bichromate (HCrO4) and/or dichromate (Cr2O72-) ions. These ions can be interconverted by the reaction: Cr₂O7²- + H₂O The standard Gibbs energies of formation of HCrO4, Cr2O72, and H₂O are -764.8, -1301, and -237.18 kJ/mol, respectively. Compute the equilibrium constant for the conversion of HCrO4 to Cr₂O7²-. 2HCrO4
The equilibrium constant for the ion-pairing reaction Mg+(aq) + SO (aq) MgSO,(aq) %3D is Kion pair 1.70 x 10. Consider a 0.0320 F solution of MgSO. Using the calculated [Mg+] as a starting point, calculate the ionic strength of the solution. Look up the activity cocfficients for Mg and So- in this table, interpolating as necessary, and then caleulate the concentration of Mg+ in solution using activity coeflicients. The activity coefficient of the ion pair (yMuso. ) can be taken as unity (1) because the ion pair is neutral. Repeat this procedure until the concentration of Mg- between iterations is stable. What is the concentration of Mg?t when activity coefficients are used? [Mg"] = 0.4554 M What percentage of this solution is ion paired? 45.54 percentage ion puired: What is the ionic strength of this solution? The calculated concentration of Mg2+ is 0.011M. Please help with the three questions below
Calculate the ionic strength of 0.5M Al2(SO4)3.
13.28 For the cell Pt,|Fe²*(a = 2.00), Fe**(a = 1.20):|I"(a = 0.100)|1½(s)|Ptg %3D %3D R (a) write the cell reaction; (b) calculate E298 assuming the net liquid-junction potential is negligible. (c) Which terminal is at the higher potential? (d) When the cell is connected to a load, into which terminal do electrons flow from the load?
The cell potential for Ag, AgCl | HCl (0.35M) || NaIO3 (0.70 M), HCl (0.010 M), I2 (0.25 M) | Pt is 1.28 V 0.98 V 1.44 V 0.81 V 1.14 V
See image below
calculate activity grams of ferric oxide ions in 1g ferric oxide in 20ml solution.
(a) Determine the equilibrium constant at 298.15 K for the cell 3+ Zn(s) | Zn2*(aq, a = 0.0120) || Mn³*(aq, a. 0.200), Mn2+(aq, az = 0.0250)| Pt(s) %3D %D (b) Is the cell reaction spontaneous as written? II