25. Answer the following questions in order to find the conditions under which Cd2+ and Zn2+ can, in theory, be separated quantitatively with H2S from a solution that is 0.1 M in each cation. (We consider a precipitation to be quantitative when all but 1 part in 1000 of the ion has been removed from the solution.) Ksp for ZnS = 1,2x10^-23 Ksp for CdS = 1,08x10^-28 K1 = 9.6 x 10^-8 K2 = 1.3 x 10^-14 Find the [H30+] to start precipitation of Zn2+ cations?

25. Answer the following questions in order to find the conditions under which Cd2+ and Zn2+ can, in theory, be separated quantitatively with H2S from a solution that is 0.1 M in each cation. (We consider a precipitation to be quantitative when all but 1 part in 1000 of the ion has been removed from the solution.) Ksp for ZnS = 1,2x10^-23 Ksp for CdS = 1,08x10^-28 K1 = 9.6 x 10^-8 K2 = 1.3 x 10^-14 Find the [H30+] to start precipitation of Zn2+ cations?

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

I have a question. If the solubility product of CaF2 is 1.46 x 10 ^-10 mol3 dm^-9, what mass of calcium fluoride will dissolve in 500 cm3 of 0.10mol dm-3 sodium fluoride solution? The molar mass of CaF2 would be 78.1g mol^-1
Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.02 M KMnO4 solution was used for the titration. gH * + MnO 4 + 5Fe 2+ -> SFe 3+ + Mn 2+ + 4H 20 (MM Fe = 56 a/moll mass of iron compound (g) 0.604 initial buret reading (mL) 0.94 Tinal buret reading (mL 16.21
Taking the Ksp of Zn(OH)2 as 4.0 x 10-3 and the Kf of [Zn(NH3)6] 2+ as 9.9 x 108 , determine how many moles of Zn(OH)2 can dissolve in 0.6 L of 1.2 M NH3.
a. Calculate the molar solubility of AgI in pure water. Ksp for AgI is 1.5 x 10-¹6. Solubility= M b. Calculate the molar solubility of AgI in 3.3 MNH3. The overall formation constant for Ag (NH3)₂* is 1.7 x 107. Solubility= M c. Compare the calculated solubilities from parts a and b. O The solubility from (a) is greater. The solubility from (b) is greater. O The solubilities from (a) and (b) are the same.
1. The solubility of CuCl is 0.0391 g/L. Calculate the Ksp of CuCl. 2.Calculate the molar solubility of CdF2 in 0.120 M NaF. The Ksp of CdF2is 6.44× 10-3 3.Calculate the pH of a solution containing 0.00052 M Mg(OH)2 at 25 °C
I need some help with THE LAST PART of this chemical analysis question. Activity coefficients can be found in the second picture.
NaCl is added slowly to a solution that is 0.010 M each in Cu+1, Ag+1, and Au+1. Given: the Ksps: CuCl = 1.9x10-7, AgCl = 1.8x10-10, AuCl = 2.0x10-13 Which compound will precipitate first?
Calculate the solubility of Mg (OH) 2 in 0.50M NH4Cl. (Kps = 1.8 x 10-11 Kb NH3 = 1.8 x 10-5).
The concentration of Pb2+ in a solution saturated with Pb(OH)2(s) is 6.69 ✕ 10−6 M. Calculate Ksp for Pb(OH)2.
The formation constant K; for the complex ion Zn(OH),² is 2.8 x 1015. What is the concentration of zinc ion, Zn?+, in a solution that is initially 0.35 M in Zn(OH),2 ? 2- [Zn²+] =[ M