At a particular temperature, the solubility of In2(SO4)3 in water is0.0061 M.What is the value of Ksp?

Answered: Image /qna-images/answer/25440471-328e-413c-9885-51bc980bb595.jpg

Answered: At a particular temperature, the…

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 14.70QE

See similar textbooks

Similar questions

The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
The solubility of silver sulfate, Ag2SO4, in water has been determined to be 8.0 g/L. What is the solubility in 0.45 M sodium sulfate, Na2SO4?
Use the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.
Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
Calculate the solubility (in grams per liter) of silver chloride in the following. (a) pure water (b) 0.025 M BaCl2 (c) 0.17 M AgNO3
. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
A scientist was interested in how soluble rust is in acidic soils, so she set up an idealized problem to get an initial feel for the situation. A fairly acidic soil has a pH of 4.50. Also, rust is essentially Fe(OH)3. Therefore, she considered the following problem: Suppose a 1.00-g sample of iron(III) hydroxide is exposed to 1.00 L of a buffer with a pH of 4.50. She then calculated the nanograms of Fe3+ that dissolve in a liter of this buffer. Show how you would do this problem. Explain your work.
Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions. b. Lets study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S=[H+]3Ksp/Kw3+KKw/[H+] where S = solubility = [Al3+] + [Al(OH)4] and K is the equilibrium constant for Al(OH)3(s)+OH(aq)Al(OH)4(aq) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 1032. Plot the solubility of Al(OH)3 in the pH range 412.
Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
Calculate the solubility (in grams per liter) of magnesium hydroxide in the following. (a) pure water (b) 0.041 M Ba(OH)2 (c) 0.0050 M MgCl2

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

SEE MORE TEXTBOOKS

At a particular temperature, the solubility of In2(SO4)3 in water is 0.0061 M. What is the value of Ksp?