queous solution of PbCl2 at 20°C is saturated when 7.2 g of this compound are dissolved in 1 L of solution. a) Calculate the activity coefficients of Pb2+ ions, Cl- ions. Use Extended Debye-Hückel equation. For aqueous solution, parameter A=0.52, B=0.33. Ion size parameter for Pb2+ is 4.5 Å. b) Calculate the activities of Pb2+ ions and Cl- ions in the saturated solution.

queous solution of PbCl2 at 20°C is saturated when 7.2 g of this compound are dissolved in 1 L of solution. a) Calculate the activity coefficients of Pb2+ ions, Cl- ions. Use Extended Debye-Hückel equation. For aqueous solution, parameter A=0.52, B=0.33. Ion size parameter for Pb2+ is 4.5 Å. b) Calculate the activities of Pb2+ ions and Cl- ions in the saturated solution.

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

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.22QAP: Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey...

See similar textbooks

Similar questions

The mean ionic activity coefficient for 0.1 M H2SO4 is 0.265. Calculate the activity of H2SO4
Calculate the solubility of the BaSO4 solid in 0.0167 M Ba (NO3) 2 solution, taking into account the activity. (Ksp for BaSO4, activity coefficients for 1.1x10^-10 Ba^2+ and SO4^2- ions are 0.46 and 0.44, respectively)
The mean activity coefficients of HBr in three dilute aqueous solutions at 25 °C are 0.930 (at 5.00 mmol kg−1), 0.907 (at 10.0 mmol kg−1), and 0.879 (at 20.0 mmol kg−1). Estimate the value of B in the Davies equation.
Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey Beer’s lawat 395 nm overa wide range. Provided the analytical concentration of the chelating reagent exceeds that of Ni(II) by a factor of 5 (or more), the cation exists, within the limits of observation, entirely in the form of the complex. Use the accompanying data to evaluate the formation constant Kf for the process Ni2++2BNiB22+
The standard potentials of Pb2+|Pb and Sn2+|Sn are −126 mV and −136 mV respectively at 25 °C, and the overpotential for their deposition are close to zero. What should the relative concentrations of Pb2+(aq) and Sn2+(aq) be in order to ensure simultaneous deposition from a mixture? You may assume that activities can be approximated by molar concentrations.
Given the following activity coefficient data: Ion Ion Size (pm) Ionic Strength (μ, M) 0.001 0.005 0.01 0.05 0.1 Zn2+ 600 0.870 0.749 0.675 0.485 0.405 Calculate the ionic strength of a solution that is 0.0213 M Mg(CN)2. Based on your results in part 1, what is the activity coefficient of Zn2+? 3. Zinc cyanide, Zn(CN)2, has a Ksp of 3.0 x 10−16. Using the activity coefficient you calculated in part 2, find the concentration of Zn2+ in a saturated solution of Zn(CN)2 in 0.0213 M Mg(CN)2. (Note: The activity coefficient for cyanide in at this ionic strength is 0.791.)
Calculate the activity coefficient (g) A).Mg+2 when its ionic strength (m) is 0.065M m γ 0.05 0.52 0.065 ? 0.1 0.44 B). SO4-2 when its ionic strength (m) is 0.038M m γ 0.01 0.661 0.038 ? 0.05 0.44
The mean activity coefficients of KCl in three dilute aqueous solutions at 25 °C are 0.927 (at 5.00 mmol kg−1), 0.902 (at 10.0 mmol kg−1), and 0.816 (at 50.0 mmol kg−1). Estimate the value of B in the Davies equation.
using the debye-huckel limiting law, calculate the activity coefficient of sulfate ion with u = 0.223 in an MGSO4 solution
Caffeine's solubility limit is about 2.2 %w/w in water at 25 Celsius degrees. Now, if I prepare a 5 %w/w PVA aqueous solution. Is the solubility limit increased or decreased (at room temperature) for this PVA solution? Why? Give me a very detailed explanation please.
Part a. Regarding micelles, do the electrostatic interactions between the sulfate head groups favor or destabilize micelle formation? How would dielectric interactions very in water vs ethanol if the dielectric constant of ethanol is 24.5 at room temperature. Part b. Why is the critical micelle concentration lower in a salt solution in terms of the Gibbs free energy?
Calculate the solubility of BaSO4 solid in 0.0167 M Ba(NO3)2 solution, taking into account its activity.(Ksp 1.1x10-10 for BaSO4; activity coefficients for Ba++ and SO42- ions are 0.46 and 0.44, respectively)