Calcium sulfate, CaSO4, has a Ksp value of 7.10 × 10-5. Whathappens when calcium and sulfate solutions are mixed to give2.00 x 10-3 MCA²+ and 3.00 x 10–²MSO4?-?A precipitate forms because Q > Ksp .A precipitate forms because Q < Ksp.No precipitate forms because Q > Ksp.O No precipitate forms because Q < Ksp.

Given: Concentration of Ca2+, [Ca2+ ] = 2.00 × 10-3 M Concentration of SO42-, [SO42- ] = 3.00 × 10-2…

Calcium sulfate, CaSO4, has a Ksp value of 7.10 × 10¬³. What happens when calcium and sulfate solutions are mixed to give 2.00 × 10–³ M Ca²+ and 3.00 x 10-² MSO4²-? A precipitate forms because Q > Ksp. A precipitate forms because Q < Ksp. No precipitate forms because Q > Ksp. No precipitate forms because Q < Ksp.

Calcium sulfate, CaSO4, has a Ksp value of 7.10 × 10¬³. What happens when calcium and sulfate solutions are mixed to give 2.00 × 10–³ M Ca²+ and 3.00 x 10-² MSO4²-? A precipitate forms because Q > Ksp. A precipitate forms because Q < Ksp. No precipitate forms because Q > Ksp. No precipitate forms because Q < Ksp.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/L
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