A chemist carries out an experiment to determine the number of moles of Cl– ions in a 1 L sample of salt water. The salt water reacts with excess AgNO3 solution. The resulting precipitate is collected, dried, and weighed. The mass of the AgCl precipitate is found to be 5.4 g. The chemical equation for the reaction is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) Calculate the moles of Cl– ions in the sample, and describe how the number of moles was found. Refer to the periodic table. Enter your answer in the space provided.
A chemist carries out an experiment to determine the number of moles of Cl– ions in a 1 L sample of salt water. The salt water reacts with excess AgNO3 solution. The resulting precipitate is collected, dried, and weighed. The mass of the AgCl precipitate is found to be 5.4 g. The chemical equation for the reaction is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) Calculate the moles of Cl– ions in the sample, and describe how the number of moles was found. Refer to the periodic table. Enter your answer in the space provided.
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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A chemist carries out an experiment to determine the number of moles of Cl– ions in a 1 L sample of salt water. The salt water reacts with excess AgNO3 solution. The resulting precipitate is collected, dried, and weighed. The mass of the AgCl precipitate is found to be 5.4 g. The chemical equation for the reaction is:
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Calculate the moles of Cl– ions in the sample, and describe how the number of moles was found. Refer to the periodic table.
Enter your answer in the space provided.
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