Please show me the complete solution. 3. A 12.5% (w/w) NiCl2 (129.61 g/mol) solution has a density of 1.149 g/mL. Calculatea. the molar concentration of NiCl2 in this solution.b. the molar CI concentration of the solution.c. the mass in grams of NiCl2 contained in each liter of this solution.4. What mass of MgNH4PO4 precipitated when 200.0 mL of a 1.000% (w/v) solution ofMgCl2 were treated with 40.0 mL of 0.1753 M Na:PO4 and an excess of NH4*? Whatwas the molar concentration of the excess reagent (Na3PO4 or MgCl2) after theprecipitation was complete?

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3. A 12.5% (w/w) NiCl2 (129.61 g/mol) solution has a density of 1.149 g/mL. Calculate a. the molar concentration of NiCl2 in this solution. b. the molar Cl concentration of the solution. the mass in grams of NiCl2 contained in each liter of this solution.

3. A 12.5% (w/w) NiCl2 (129.61 g/mol) solution has a density of 1.149 g/mL. Calculate a. the molar concentration of NiCl2 in this solution. b. the molar Cl concentration of the solution. the mass in grams of NiCl2 contained in each liter of this solution.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Please show me the complete solution.

3. A 12.5% (w/w) NiCl2 (129.61 g/mol) solution has a density of 1.149 g/mL. Calculate
a. the molar concentration of NiCl2 in this solution.
b. the molar CI concentration of the solution.
c. the mass in grams of NiCl2 contained in each liter of this solution.
4. What mass of MgNH4PO4 precipitated when 200.0 mL of a 1.000% (w/v) solution of
MgCl2 were treated with 40.0 mL of 0.1753 M Na:PO4 and an excess of NH4*? What
was the molar concentration of the excess reagent (Na3PO4 or MgCl2) after the
precipitation was complete?

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