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 HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 17, Н.О 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.

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 HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 17, Н.О 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.

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

1.
A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of
Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T;
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.
(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.

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