ps 27. A solution contains 0.0497 M SO4 (aq) and 0.0894 M CO32 (aq). If Ag+ (aq) ions are slowly added, whichla compound (Ag2SO4 or Ag2CO3) will ppt first and at what [Ag]? (In other words, which of the following isalentirely correct?) (Suggestion: Write the dissolving equations and Ksp expressions for Ag2SO4 and Ag2CO3before starting this problem.)a. Ag2SO4 precipitates first at [Ag+] = 1.8 x 102 Mb. Ag2CO3 precipitates first at [Ag+] = 9.6 x 106 Mc. Ag2CO3 precipitates first at [Ag+] = 9.2 x 10-11 Md. Ag2SO4 precipitates first at [Ag+] = 3.2 x 104 Me. Ag2CO3 precipitates first at [Ag+] = 1.3 x 10-5 M0. bCarsidong01 1.8-0301-01 x 1.8-9 d100to squads llenavo odi staluple 08.0

To determine which compound precipitates first and at what concentration of Ag⁺, we need to compare…

Answered: ps 27. A solution contains 0.0497 M SO4…

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

Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.434 M in bothBr– andI–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur?AgBr mol/L AgI mol/L Which will precipitate first?Choose one AgBr AgI What percentage of the halide ion that is precipitated first remains in solution before the second begins to precipitate? % If complete separation is defined as there being less than 0.10% of a particular ion left in solution, does this method completely separate Br– from I–?Choose one: Yes No Cannot be determined
When silver chromate, Ag2CrO4, dissolves in otherwise pure water, what is the relation between [Ag+] and [CrO42-]? The solubility product of Ag2CrO4 is 1.9x10-12. Show that its solubility in pure water is 0.78x10-4 M.
K = CD [4 B Please calculate the molar solubility of Sn(OH)4when dissolved in a pH =9.12 solution, if the Ksp for Sn(OH)4 is Ksp = 1.0 × 10-37 Please input your answer in scientific notation to the second decimal place. (If you get back a whole number, like 5.67 just type in 5.67 *10^O) Type your answer.
If 50.0 g of barium arsenate (Ksp = 1.1 x 10 13) are placed in enough water to generate 500.0 mL of solution, calculate the following: %3D The molar solubility of the barium arsenate solution. b. The molar solubility of the barium ion if 30.0 mL of 0.400 M barium nitrate solution is added to the original solution. а. The molar solubility of the barium arsenic solution. b. The molar solubility of the barium ion if 30.0 mL of 0.400 M barium nitrate solution is added to the original solution.
A solution is prepared by combining 20.00ml of 0.150 molar Ba2+ and 25.00ml of 0.125 molar Cl- Using concentrations and volumes above, determine if a precipitate will form when these solutions are mixed at 25C. Provide a calculation to support your answer, keep in mind the system is not at standard state. Ba2+ (aq) -560.77 kJ/mol Delta Gfo Cl- (aq) -131.228 kJ/mol Delta Gfo BaCl2 -1296.32 kJ/mol Delta Gfo
Solubility of AgCl is 0.0000123 M. What is the solubility product, Ksp for AgCl?
Calculate the molar solubility of AgCl in a solution that already contains 0.10 M Cl- (aq).
The value of ?? for the reaction: AgBr (s) ⇋ Ag+(aq) + Br−(aq)It is 7.7 × 10−13 at 25 ° C. Determine the solubility of AgBr in:a) Distilled H2O.b) A 0.01 M solution in CaCl2
26. Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products) ( a) TICI (b) Ba * F_{2} (c ) A*g_{2} * C * r * O_{4} ( d) Ca * C_{2} * O_{4} * H_{2} * O (e) the mineral anglesite, PbS * O_{4}
What is the molar solubility of silver iodide, Agl, in 0.0325 M CH;NH,? For AgI Ksp = 8,52 x 10 "; for [Ag(CH;NH,)2]", Kf= 7.8 x 10°
3) a) AgI(s)⇄Ag+(aq)+I−(aq)Ksp=8.3×10−17at 298KThe dissolution of AgI is represented above. Which of the followingshows the mathematical relationship between the molar solubility, S , ofAgI andtheKspat 298K?a)S=8.3×10−17mol/L b) S=(8.3×10−17)mol/L2c) S=(8.3×10−17)1/2 mol/Ld) S= 2(8.3×10−17)1/2 mol/Lb) State which of the following salts is the most soluble in water. Salt KspCuS 8.5x10−45Ag2S 1.6x10−49Bi2S3 1.1x10−73
A 25.00 mL solution of 0.08010 M Nal is titrated with 0.05020 M AgNO,. Calculate pAg following the addition of the given volumes of AgNO,. The Kp of Agl is 8.3 × 10-17. 36.50 mL pAg V pAg = Incorrect 47.40 mL pAg 1.51 1.51 Incorrect 2.70 Incorrect

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS