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3) An unknown sample weighing 0.2583 g is titrated to the end point with 47.28 mL of a 0.10 M AgNO3 solution. What is the weight percent of Cl- in the sample?

3) An unknown sample weighing 0.2583 g is titrated to the end point with 47.28 mL of a 0.10 M AgNO3 solution. What is the weight percent of Cl- in the sample?

Chemistry
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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**Name:** _______ **Date:** _______ **Section:** _______ **Prelaboratory Assignment: Analysis of an Unknown Chloride** 1. **A sample containing 0.175 g of Cl⁻ is dissolved in 50 mL of deionized H₂O. The solution is titrated to the equivalence point with a AgNO₃ solution. The final volume of the titrated sample is 75 mL.** a) What is the concentration of the AgNO₃ solution? *(Answer space: __________________________)* b) How many grams of AgCl are precipitated? *(Answer space: __________________________)* 2. **A student wishes to determine the mass percentage of barium in a 2.016 g sample. The student titrated the sample with 20 mL of 0.20 M H₂SO₄, producing a BaSO₄ precipitate.** a) How many moles of BaSO₄ were formed in the titration? *(Answer space: __________________________)* b) What was the mass of barium present in the original sample? *(Answer space: __________________________)* c) What was the mass percent of barium in the original sample? *(Answer space: __________________________)* 3. **An unknown sample weighing 0.2358 g is titrated to the endpoint with 47.28 mL of a 0.10 M AgNO₃ solution. What is the weight percent of Cl⁻ in the sample?** *(Answer space: __________________________)*
Transcribed Image Text:**Name:** _______ **Date:** _______ **Section:** _______ **Prelaboratory Assignment: Analysis of an Unknown Chloride** 1. **A sample containing 0.175 g of Cl⁻ is dissolved in 50 mL of deionized H₂O. The solution is titrated to the equivalence point with a AgNO₃ solution. The final volume of the titrated sample is 75 mL.** a) What is the concentration of the AgNO₃ solution? *(Answer space: __________________________)* b) How many grams of AgCl are precipitated? *(Answer space: __________________________)* 2. **A student wishes to determine the mass percentage of barium in a 2.016 g sample. The student titrated the sample with 20 mL of 0.20 M H₂SO₄, producing a BaSO₄ precipitate.** a) How many moles of BaSO₄ were formed in the titration? *(Answer space: __________________________)* b) What was the mass of barium present in the original sample? *(Answer space: __________________________)* c) What was the mass percent of barium in the original sample? *(Answer space: __________________________)* 3. **An unknown sample weighing 0.2358 g is titrated to the endpoint with 47.28 mL of a 0.10 M AgNO₃ solution. What is the weight percent of Cl⁻ in the sample?** *(Answer space: __________________________)*
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