The gravimetric determination of Ni-*: Ni (58.7 g/mol) was precipitated as Ni(DMG) 2 (288.7 g/mol). The volume of unknown solution in the sample =30.00 mL. The mass of empty crucible =30.107 g, the mass of empty crucible and precipitate = 30.300 g. Calculate the concentration of Ni+ in the unknown in sample solution (in mg/L) is: 1. O2.62X103 2. O1.31X 103 3. 25.3X 104 4. 00.5X 105 Previous Next

The gravimetric determination of Ni-*: Ni (58.7 g/mol) was precipitated as Ni(DMG) 2 (288.7 g/mol). The volume of unknown solution in the sample =30.00 mL. The mass of empty crucible =30.107 g, the mass of empty crucible and precipitate = 30.300 g. Calculate the concentration of Ni+ in the unknown in sample solution (in mg/L) is: 1. O2.62X103 2. O1.31X 103 3. 25.3X 104 4. 00.5X 105 Previous Next

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
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