The solubility product (Ksp) for silver sulfate (Ag2SO4 (s)) is 1.2x10-5. Upon dissolving, Ag2SO4 (s) dissociates into Ag* and SO4²- ions. What will be the activity of Ag2SO4 (s) for a saturated solution at equilibrium, assuming the activity coefficients are all 1.0? Enter your numerical answer in the space available. Show your work on your paper or electronic file. What will be the concentration of Ag* in moles/L for a saturated solution at equilibrium, assuming the activity coefficients are all 1.0?

The solubility product (Ksp) for silver sulfate (Ag2SO4 (s)) is 1.2x10-5. Upon dissolving, Ag2SO4 (s) dissociates into Ag* and SO4²- ions. What will be the activity of Ag2SO4 (s) for a saturated solution at equilibrium, assuming the activity coefficients are all 1.0? Enter your numerical answer in the space available. Show your work on your paper or electronic file. What will be the concentration of Ag* in moles/L for a saturated solution at equilibrium, assuming the activity coefficients are all 1.0?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 37P

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Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
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