Solid Na2 SO4 is added slowly to a solution that is 0.40M in Pb(NO3), and 0.75M in Ba (NO3)2. In what order will solid PBSO, and BaSO4 form? Calculate the percentage of Ba* that precipitates just before PbSO4 begins to precipitate. Assume that Ksp (PBSO4) =1.8 × 10 8 and Ksp (BaSO4) = 1.1 x 10 10 2+ %3D %3D will precipitate first. Percentage |3D

Solid Na2 SO4 is added slowly to a solution that is 0.40M in Pb(NO3), and 0.75M in Ba (NO3)2. In what order will solid PBSO, and BaSO4 form? Calculate the percentage of Ba* that precipitates just before PbSO4 begins to precipitate. Assume that Ksp (PBSO4) =1.8 × 10 8 and Ksp (BaSO4) = 1.1 x 10 10 2+ %3D %3D will precipitate first. Percentage |3D

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

Use the reaction quotient to predict whether a precipitate will form. If 15.0 mL of 9.93×104 M Pb(NO3)2 are added to 22.0 mL of 2.60×105 M (NH4)2SO4 will solid PbS04 (Ksp = 1.8×10) precipitate? If a precipitate will not form, what sulfate ion concentration will cause a precipitate of lead sulfate to form? If a precipitate will form, what is the minimum [SO42] that could have been present without initiating precipitation? Assume the total volume used in the above example. M
Solid cobalt(II) nitrate is slowly added to 50.0 mL of a 0.0541 M sodium hydroxide solution. The concentration of cobalt(II) ion required to just initiate precipitation is M. (Assume that Ksp (Co(OH)2)= 2.5 x 10^-16).
If 200 mL of 1.0 x 10^-8 M AgNO_3 is mixed with 200 mL of 1.0 x 10^-8 M Nal, what will occur? For Agl, Ksp = 8.5 x 10-17, Sodium iodide will precipitate. Sodium nitrate will precipitate. No precipitate will form. Silver iodide will precipitate Silver nitrate will precipitate.
If 14.00 mL of 0.10 M Ba(NO3), are added to 30.00 mL of 0.10 M Na,CO3 a precipitate of BaCO3 will form. O a precipitate of NaNO3 will form. O no precipitation occurs because both possible products are soluble. no precipitate forms because Q< Ksp-
A solution is 5.0 x 10-5 M in each of these ions: Ag+, SO;-, CF, and CO?-. Which precipitate will form? Ag,CO3 (Kp = 8.46 × 10-12) Ag,SO4 (Kp = 1.12 × 10-5) AgCI (Kp = 1.77 × 10-19)
Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOHKOH required for precipitation to begin in each case. 1. 0.010 MM CaCl2CaCl2 (Ksp=4.68×10−6Ksp=4.68×10−6 for Ca(OH)2Ca(OH)2) 2. 0.0020 MM Fe(NO3)2Fe(NO3)2 (Ksp=4.87×10−17Ksp=4.87×10−17 for Fe(OH)2Fe(OH)2) 3. 0.0016 MM MgBr2MgBr2 (Ksp=2.06×10−13Ksp=2.06×10−13 for Mg(OH)2Mg(OH)2)
A solution contains 0.021 M Cl- and 0.017 M I. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10-6, Ksp(Cul) = 5.1 × 10-12
Suppose 60.0 mL of 0.100 M Pb(NO3)2 is added to 30.0 mL of 0.150 M KI. How many grams of Pbl2 will be formed? Mass Pbl₂ = 1.037 Hint [K+] Your answer is correct. [1] What will be the molar concentrations of all the ions in the mixture after equilibrium has been reached? Record all answers to three (3) significant figures. Your answer is partially correct. [Pb²+] 0.05 i 0.05 g [NO3] 0.13 0.067 M M 3 3 M
18. If 25 mL of a 0.050 M CaCl2 solution and 50. mL of a 0.020 M Na2SO4 solution are mixed, will CaSO4 (Ksp = 2.4 x 10°) precipitate?
Will a precipitate form when 40.00 mL of 0.0122 M calcium nitrate solution is mixed with 60.00 mL of 0.00386 M potassium sulfate solution? (Ksp for calcium sulfate = 4.9 x 10-5)