For a solution that is 0.1 M Cu 2+, 0.1 M Zn 2+, 0.3 M H 30 + and saturated with H 2S, which of the following are true statements? (Choose all that apply.) | ZnS will not precipitate because Q > Ksp. ) CuS will precipitate because Q < Ksp. Cus will precipitate because Q < Ksp. | ZnS will not precipitate because Q < Ksp. | ZnS will precipitate because Q > Ksp. Cus will precipitate because Q > Ksp. Cus will not precipitate because Q < Ksp. O ZnS will precipitate because Q < Ksp.

For a solution that is 0.1 M Cu 2+, 0.1 M Zn 2+, 0.3 M H 30 + and saturated with H 2S, which of the following are true statements? (Choose all that apply.) | ZnS will not precipitate because Q > Ksp. ) CuS will precipitate because Q < Ksp. Cus will precipitate because Q < Ksp. | ZnS will not precipitate because Q < Ksp. | ZnS will precipitate because Q > Ksp. Cus will precipitate because Q > Ksp. Cus will not precipitate because Q < Ksp. O ZnS will precipitate because Q < Ksp.

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

combine 500 ml of 0.01 M lead nitrate with 500 ml of 0.01M hydrochloric acid. Ksp of PbCl2 = 1.17 × 10-⁵ a) show through calculations, is the precipitate of PbCl2 formed?
questions number 19
Above what Fe2 + concentration will Fe(OH), precipitate from a buffer solution that has a pH of 9.52? The Ksp of Fe(OH), is 4.87x10-17. -9 5.1 x10 [Fe?*] = M
591. mL of 0.00499 M Nal (aq) is combined with 419. mL of 0.00325 M Pb(NO3), (aq). Determine if a precipitate will form given that the Ken of Pbl, is 1.40x10-8. Precipitation will occur because Qsp > Ksp O Precipitation will occur because Qsp = Kgp O Precipitation will not occur because Qsp Kep O0000
you are given a 1.00 ml solution of 0.100 m Cl- and told to verify the chloride concentration by gravimetric analysis. 1.00 ml of 0.500 m ag+ is added to this solution and the resultant AgCl quantitatively precipitated. based on the ksp expression, calculate the concentration of the cl- that remains in solution.
Solid NaBr is slowly added to a solution that is 0.012 M in Cu+ and 0.012 M in Ag+ Which compound will begin to precipitate first? AgBr NaBr What percent of Ag remains in solution at the point when CuBr just begins to precipitate?
Give answer all questions with explanation and answer no too
assume that 200 ml of 0.8 M KCl solution is mixed with 300 ml of 0.01 M AgNO3 solution. Knowing that Ksp of AgCl = 1.7 × 10-¹⁰ calculate whether precipitate will form?
Please explain this question to me with proper and detailed solution (Explain why), and dont use any cursive handwriting, thanks!
What you expect to observe on mixing 0.1M Zn(CO3)2 with 6M NaOH. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?
A 0.20 M sodium chloride solution is slowly added to a solution containing 0.40 M Pb2* and 0.40 M Ag* ions. What is the remaining concentration of the first ion at the point where the second ion just begins to precipitate? The Ksp of PbCl2 is 1.2x10-5, and the Ksp of AgCl is 1.8x10-10. 1.6x10-6 M 6.0x10-9 M ) 3.1x10-2 M 1.4x10-2 M 3.4x10-5 M
The Ksp of AgCI at 25 degrees Celsius is 1.6 * 10^-10. Consider a solution that is 1.0 * 10^-2 M in CaCI2 and 1.0 * 10^-8 M in AgNO3. A) Q > Ksp and a precipitate will form. B) Q < Ksp and a precipitate will not form. C) Q = Ksp The correct answer is Q > Ksp, but I need an explanation as to why that’s the answer please.