Assume the solubility product of Mg(OH)2 is 1.3 x 10 at a certain temperature. What minimum OHconcentration must be attained (for example, by adding NaOH) to decrease the Mg2+ concentration in asolution of Mg(NO3), to less than 1.2 x 10-10 M.3/2x 10M(Enter your answer in scientific notation.)Next >< Prev18 of 20****.*****

Given: The solubility product of Mg(OH)2 = 1.3 × 10-11 We have to calculate the minimum…

Answered: .Assume the solubility product of…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 84QRT

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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) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
The solubility-product constants, Kp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Кар FeCO3 2.10 x 10-11 CdCO3 1.80 x 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.03x10-2 M Fe2+ and 1.52x10-2 MCd2+. What concentration of CO² is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ▸ View Available Hint(s) [CO32] = Value Units Submit Part B Complete previous part(s) Part C Complete previous part(s) Provide Feedback ? Next >
The Solubility Product Constant for zinc carbonate is 1.5 × 10-¹¹. Solid potassium carbonate is slowly added to 125 mL of a 0.0359 M zinc nitrate solution. The concentration of carbonate ion required to just initiate precipitation is M.
59. Iron(II) hydroxide, Fe(OH)2, has a solubility in water of 6.0 x 10¹ mg/L at a given temperature. (a) From this solubility, calculate the Ksp of iron(II) hydrox- ide. Explain why the calculated K differs from the experimental value of 8.0 X 10-16. (b) Calculate the hydroxide concentration needed to precip tate Fe²+ ions such that no more than 1.0 µg Fe²+ per liter remains in the solution. 1x 10¹, in
The solubility-product constants, Ksp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10 x 10-11 CdCO3 1.80 × 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.02x10-2 MFe²+ and 1.48x10-2 M Cd²+. What concentration of CO3²- is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ► View Available Hint(s) [CO3²- ] = Submit μA Value Part B Complete previous part(s) Part C Complete previous part(s) Units ?
PbCl2; molar solubility = 1.43 x 10-² M Ksp = 1.17 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Note that Ksp is the solubility-product constant, the equilibrium constant for a chemical equation representing the dissolution of an ionic compound: Ksp = [Pb²+][C1-1² ■√ ΑΣΦ 10-8 Part C Prepare an ICE table (where I means initial, C means change, and E means equilibrium), where the equilibrium concentrations of the formed ions are expressed in terms of S (the number of moles per liter of PbCl2 dissolved) and substitute them into the expression for Ksp. Ksp CaF2; molar solubility = 3.32 × 10-4 M = Submit ΑΣΦ Request Answer
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I need help with Table 11-1. but I need something sorted so I can understand the answer.
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A pipette is used to add 41 mL of 0.2 M Pb(NO3)2 to a 268.0 mL solution of 0.2 M NaF. Determine the equilibrium concentration of Pb2+(aq) in the final solution. Ksp(PbF2)=3.6E-8Include at least 3 significant figures in your answer.
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.Assume the solubility product of Mg(OH)2 is 1.3 x 10 at a certain temperature. What minimum OH concentration must be attained (for example, by adding NaOH) to decrease the Mg2+ concentration in a М. solution of Mg(NO,), to less than 1.2 x 10-10 x 10 M (Enter your answer in scientific notation.)