1. A student synthesized 3.214g of Ni(NH3),Cl2 from 4.023g of NiCl2 6H₂O. He dissolved 0.81g of Ni(NH3) nCl2 in 40 mL of 1.0M HCl to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 17; H₂O 18. (1) A 0.20M Ni²+ standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = εbc.
1. A student synthesized 3.214g of Ni(NH3),Cl2 from 4.023g of NiCl2 6H₂O. He dissolved 0.81g of Ni(NH3) nCl2 in 40 mL of 1.0M HCl to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 17; H₂O 18. (1) A 0.20M Ni²+ standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = εbc.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 10E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...
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Transcribed Image Text:(2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample.
Calculate the mass percent of NH3 in the product.
Transcribed Image Text:1.
A student synthesized 3.214g of Ni(NH3),C2 from 4.023g of NiCl2•6H2O. He dissolved 0.81g of
Ni(NH3)nCl2 in 40 mL of 1.0M HCl to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 17;
H2O 18.
(1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of
0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A
= ɛbc.
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