The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HC1 is then neutralized with with NaOH. The reaction of HCl with Zn is shown. Zn(s) + 2 HCl(aq) - ->> > ZnCl₂ (aq) + H₂(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.94 mL of 0.530 M NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample? %w/w = % Zn

The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HC1 is then neutralized with with NaOH. The reaction of HCl with Zn is shown. Zn(s) + 2 HCl(aq) - ->> > ZnCl₂ (aq) + H₂(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.94 mL of 0.530 M NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample? %w/w = % Zn

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

The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess
HCI is then neutralized with with NaOH. The reaction of HCl with Zn is shown.
Zn(s) + 2 HCl(aq) ->> ZnCl₂ (aq) + H₂(g)
The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A
20.0 mL aliquot of the final solution required 8.94 mL of 0.530 M NaOH to neutralize the excess HCl. What is the mass
percentage (%w/w) of Zn in the ore sample?
%w/w =
% Zn

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