For a solution in which µ = 7.5 × 10−², calculate K'sp fora. AgSCN-12(Ksp (AgSCN) = 1.1 × 10−¹K'SP=K'b. Pbl2(Ksp (PbI₂) = 7.9 × 10-⁹, apb²+-9spK'SPc. La(IO3)3(Ksp (La(IO3)3) = 1.0 × 10-¹¹"=dAgt="=== 0.25, ascN- = = 0.35): 0.45, araLa³+==0.3)0.9, απ03-= 0.35)=

a. Ksp of AgSCN = 1.1 x 10-12 , b. Ksp of PbI2 = 7.9 x 10-9 , c. Ksp of La(IO3)3 = 1.0 x 10-11 ,

For a solution in which µ = 7.5 × 10-², calculate K'sp for a. AgSCN (Ksp (AgSCN) = 1.1 × 10−¹², KSP = a Ag+ = 0.25, ascN- = = 0.35) b. Pbl2 -9 (Ksp (PbI2) = 7.9 × 10-⁹, αpb²+ K'SP c. La(IO3)3 (Ksp (La(IO3)3) = 1.0 × 10−¹¹ K'sp = 3 = 0.45, a₁ = 0.3) aLa³+ = 0.9, α103- - = 0.35) =

For a solution in which µ = 7.5 × 10-², calculate K'sp for a. AgSCN (Ksp (AgSCN) = 1.1 × 10−¹², KSP = a Ag+ = 0.25, ascN- = = 0.35) b. Pbl2 -9 (Ksp (PbI2) = 7.9 × 10-⁹, αpb²+ K'SP c. La(IO3)3 (Ksp (La(IO3)3) = 1.0 × 10−¹¹ K'sp = 3 = 0.45, a₁ = 0.3) aLa³+ = 0.9, α103- - = 0.35) =

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter15: Solubility And Complex Lon Equilibria

Section: Chapter Questions

Problem 110IP

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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 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)
. 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.
The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.
Magnesium hydroxide, Mg(OH)2, is the active ingredient in die antacid TUMS and has a Ksp value of 8.9 1012. If a 10.0-g sample of Mg(OH)2 is placed in 500.0 mL of solution, calculate the moles of OH ions present. Because the Ksp value for Mg(OH)2 is much less than 1, not a lot of solid dissolves in solution. Explain how Mg(OH)2 works to neutralize large amounts of stomach acid.
Given that the Gf for Pb2+(aq) and Cl-(aq) is -24.3 kJ/mole and -131.2 kJ/mole respectively, determine the solubility product, Ksp, for PbCl2(s).
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
A Boric acid and glycerin form a complex B(OH)3(aq) + glycerin(aq) B(OH)3 glycerin(aq) with an equilibrium constant of 0.90. If the concentration of boric acid is 0.10 M, how much glycerin should be added, per liter, so that 60.% of the boric acid is in the form of the complex?
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?
Consider the solutions presented: (a) Which of the following sketches best represents the ions in a solution of Fe(NO3)3(aq)? (b) Write a balanced chemical equation showing the p10ducts of the dissolution of Fe(NO3)3.
You are browsing through the Handbook of Hypothetical Chemistry when you come across a solid that is reported to have a Ksp value of zero in water at 25C. What does this mean?
Most barium compounds are very poisonous; however, barium sulfate is often administered internally as an aid in the X-ray examination of the lower intestinal tract (Figure 15.4). This use of BaSO4 is possible because of its low solubility. Calculate the molar solubility of BaSO4 and the mass of barium present in 1.00 L of water saturated with BaSO4.

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