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Calcium hypochlorite (Ca(OCI),, MW = 142.983 g/mol) is often used as the source of the hypochlorite ion (OCI, MW = 51.452 g/mol) in solutions used for water treatment. A student must prepare 50.0 mL of a 40.0 ppm OCI solution from solid Ca(OCI),, which has a purity of 91.0%. Calculate the mass of the impure reagent required to prepare the solution. Assume the density of the solution is 1.00 g/mL. mass: Which method would work best to accurately prepare 50.0 mL of the 40.0 ppm OCI solution? Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Then, use a graduated cylinder to measure out 50.0 mL of water. Combine the reagent and water in a 50.0 mL volumetric flask and mix it thoroughly. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a pipet to transfer a portion of the concentrated solution to a separate 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a graduated cylinder to transfer a portion of the more concentrated solution to a 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Transfer the reagent to a 50.0 mL volumetric flask, add water to the line, and mix thoroughly. CD g

Calcium hypochlorite (Ca(OCI),, MW = 142.983 g/mol) is often used as the source of the hypochlorite ion (OCI, MW = 51.452 g/mol) in solutions used for water treatment. A student must prepare 50.0 mL of a 40.0 ppm OCI solution from solid Ca(OCI),, which has a purity of 91.0%. Calculate the mass of the impure reagent required to prepare the solution. Assume the density of the solution is 1.00 g/mL. mass: Which method would work best to accurately prepare 50.0 mL of the 40.0 ppm OCI solution? Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Then, use a graduated cylinder to measure out 50.0 mL of water. Combine the reagent and water in a 50.0 mL volumetric flask and mix it thoroughly. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a pipet to transfer a portion of the concentrated solution to a separate 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a graduated cylinder to transfer a portion of the more concentrated solution to a 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Transfer the reagent to a 50.0 mL volumetric flask, add water to the line, and mix thoroughly. CD g

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 98AP
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Calcium hypochlorite (Ca(OCI),, MW = 142.983 g/mol) is often used as the source of the hypochlorite ion (OCI, MW = 51.452 g/mol) in solutions used for water treatment. A student must prepare 50.0 mL of a 40.0 ppm OCI solution from solid Ca(OCI),, which has a purity of 91.0%. Calculate the mass of the impure reagent required to prepare the solution. Assume the density of the solution is 1.00 g/mL. mass: Which method would work best to accurately prepare 50.0 mL of the 40.0 ppm OCI solution? Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Then, use a graduated cylinder to measure out 50.0 mL of water. Combine the reagent and water in a 50.0 mL volumetric flask and mix it thoroughly. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a pipet to transfer a portion of the concentrated solution to a separate 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a graduated cylinder to transfer a portion of the more concentrated solution to a 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Transfer the reagent to a 50.0 mL volumetric flask, add water to the line, and mix thoroughly. CD g
Transcribed Image Text:Calcium hypochlorite (Ca(OCI),, MW = 142.983 g/mol) is often used as the source of the hypochlorite ion (OCI, MW = 51.452 g/mol) in solutions used for water treatment. A student must prepare 50.0 mL of a 40.0 ppm OCI solution from solid Ca(OCI),, which has a purity of 91.0%. Calculate the mass of the impure reagent required to prepare the solution. Assume the density of the solution is 1.00 g/mL. mass: Which method would work best to accurately prepare 50.0 mL of the 40.0 ppm OCI solution? Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Then, use a graduated cylinder to measure out 50.0 mL of water. Combine the reagent and water in a 50.0 mL volumetric flask and mix it thoroughly. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a pipet to transfer a portion of the concentrated solution to a separate 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out an amount of reagent larger than what was determined in the first part of the question. In a volumetric flask, combine the reagent and water to create a solution with a concentration greater than 40.0 ppm. Use a graduated cylinder to transfer a portion of the more concentrated solution to a 50.0 mL volumetric flask and dilute to the line with water to create a solution with a concentration of 40.0 ppm. Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Transfer the reagent to a 50.0 mL volumetric flask, add water to the line, and mix thoroughly. CD g
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