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.
General Chemistry - Standalone book (MindTap Course List)
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ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter4: Chemical Reactions
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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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