Cd and Fe (starting concentration 10 mol/L) should be separated by fractionated precipitation using H₂S. Does a pH range exist allowing to completely precipitate one metal (i.e. the remaining concentration of the precipitated ion has to be 10 mol/L or less) whereas the other stays in solution at its initial concentration? Please calculate this pH range whereby pH values below zero are set to zero! Please illustrate the situation graphically by plotting pH versus in solution/precipitating/fully precipitated for the two ions (9)

Cd and Fe (starting concentration 10 mol/L) should be separated by fractionated precipitation using H₂S. Does a pH range exist allowing to completely precipitate one metal (i.e. the remaining concentration of the precipitated ion has to be 10 mol/L or less) whereas the other stays in solution at its initial concentration? Please calculate this pH range whereby pH values below zero are set to zero! Please illustrate the situation graphically by plotting pH versus in solution/precipitating/fully precipitated for the two ions (9)

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 132IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...

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A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
A sample can contain any ion from groups I to IV. Adding 6M HCl does not produce precipitates.The H + concentrations are adjusted to 0.3M and the solution is saturated with H2S, no precipitate forms.However, when [ H+] is reduced to 10-9M and saturated again with H2S, precipitate appears. Subsequently, it is found that this precipitate is a group III hydroxide.In group IV analysis, a precipitate is formed by adding (NH4) 2CO3. What ions must be present from groups a) I, b) II, c) III d) IV ?
A 0.150 mol quantity of CoCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Co²+ ions at equilibrium? Assume the formation constant* of Co(NH,+ is 5.0 × 1031M-6. concentration:
If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 9.14e-08 g of Sc(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Sc(OH)3.Ksp = (c) The Ksp of Cu3(PO4)2 at 25 oC is 1.40e-37. What is the molar solubility of Cu3(PO4)2?solubility = mol/L
A solution contains 1.0 * 10-2 M Ag+(aq) and 2.0 * 10-2 M Pb2+(aq). When Cl-(aq) is added, both AgCl (Ksp = 1.8 * 10-10) and PbCl2 (Ksp = 1.7 * 10-5) can precipitate. What concentration of Cl-(aq) is necessary to begin the precipitation of each salt? Which salt precipitates first?
A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar solubility of magnesium hydroxide?
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K,,, data in the ALEKS Data tab. compound KCI Ca(OH), CaCl₂ Does solubility change with PH? yes Ono O yes Ⓒno yes O no pH-B 0 highest solubility pH = 7 X pH = 5 0 5
123 mL of a 0.352 M Ca(NO3)2 solution is mixed with 251 mL of a 0.254 M solution of NaF at 25ºC. Calculate Qsp for the precipitate formed.
2) If 25.0 mL strong electrolyte of 0.1 M BaCl₂ solution and 75.0 mL of 0.1 M Na₂CO3 solution are mixed, (a) Will the BaCO, precipitate? Show your answer by calculation. (b) Find the concentrations of Ba²* ions and CO2 ions in the system at equilibrium. (c) Calculate the solubility of BaCO; in this solution as mg/L. (Ksp for BaCO3 = 5.1×102, Molar mass of BaCO3 = 197.4 g/mol)
Magnesium can be found in drinking water at concentrations of less than 20 ppm or 0.00082 M or 8.2E-4 M. For an analysis of a water sample, the pH is to be increased to precipitate magnesium hydroxide. At what pH will Mg(OH), be expected to precipitate with this Mg* concentration? The Ksp of Mg(OH)2 is 5.61x10-12. Use the corresponding Ksp expression and pOH equation. Note that you probably have to convert pOH to pH. Do not forget that the hydroxide ion concentration is raised to an exponent of 2.
The Kp for praseodymium (III) hydroxide, Pr(OH)3, is 3.39 x 10 24. What pH, to two places past the decimal, will just precipitate out praseodymium (III) hydroxide in a 0.659 M solution of Pr(NO;);?

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