Activity 5 More on Solubility, and LeChatelier's Principle (5a) What is the molar solubility of CaF2 if the Ksp is 3.4 x 1011? (5b) What would happen if acid were added to this solution? What would happen if base were added? (Explain) (5c) What is the solubility of CaF2 in a 0.12 M solution of Nak. Explain the difference in your answer to this part and to 5a.

Activity 5 More on Solubility, and LeChatelier's Principle (5a) What is the molar solubility of CaF2 if the Ksp is 3.4 x 1011? (5b) What would happen if acid were added to this solution? What would happen if base were added? (Explain) (5c) What is the solubility of CaF2 in a 0.12 M solution of Nak. Explain the difference in your answer to this part and to 5a.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 76QAP

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Similar questions

How do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4 Change when 100 g of solid Ag2CrO4 is added to the system? Explain.
The solubility product of MgF, is 10-8.2 (A) What is the solubility of Mg²* at equilibrium with MgF2? (B) If MgF2 is dissolved in a solution of 0.011-molar F¯, how much will dissolve at equilibrium?
Lead (II) bromide, PbBr2, has Ksp= 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+and Br–at equilibrium.)
Lead (II) bromide, PbBr2, has Ksp = 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+ and Br– at equilibrium.)
(a) True or false: “solubility” and “solubility-product constant”are the same number for a given compound. (b) Writethe expression for the solubility-product constant for eachof the following ionic compounds: MnCO3, Hg(OH)2, andCu3(PO4)2.
If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
A chemistry graduate student Is glven 300. mL of a 1.50M trimethylamine ((CH, N solutlon. Trimethylamine Is a weak base with K,=7.4x 10 ". what 3. mass of (CH,NHBr should the student dissolve in the (CH, N solutlon to turn It Into a buffer with pH = 11.107 (CH), 3 You may assume that the volume of the solution doesn't change when the (CH,) NHBR Is dissolved In it. Be sure your answer has a unit symbol, and round It 3 to 2 significant digits. do Ar x10 Check Explanation 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility V I 3:55 hp 火 Ce & esc $4 8. #3 ! 4 3 t y r e W
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 Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed. (a) What is the molar solubility of BaSO4? (b) What is its solubility in grams per 100 g of water?
A chemistry graduate student is given 125. mL of a 1.00M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K = 7.4 × 10-4. What 3 mass of (CH3)2NHBr should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 10.91? You may assume that the volume of the solution doesn't change when the (CH3)₂NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 Ox x10 S
A nephrolith is formed due to Ca (II) oxalate, phosphate or urate precipitation. Will CaC204 precipitate if the concentration of oxalate anion C2042- in blood plasma increase to 3.8•10-4 mol/L; the concentration of Ca2+ in plasma blood is 1.8 · 10 mol/L, Ksp(CaC204) = 2,3 · 10-9 mol?/L2 4

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