Calcium hypochlorite $)=(142\mathrm{.}983\frac{g}{m}ol$ is often used as the source of the hypochlorite ion

$51\mathrm{.}452\frac{g}{m}ol)$ in solutions used for water treatment. A student must prepare $50\mathrm{.}0mL$ of a $35\mathrm{.}0ppmOC{l}^{-}$solution from solid

$Ca(OCl{)}_2,$ which has a purity of $93\mathrm{.}0\%.$

Calculate the mass of the impure reagent required to prepare the solution. Assume the density of the solution is $1\mathrm{.}00\frac{g}{m}L.$

m

Incorrect

Which method would work best to accurately prepare $50\mathrm{.}0mL$ of the $35\mathrm{.}0ppmOC{l}^{-}$solution?

Use an analytical balance to weigh out the amount of reagent determined in the first part of the question. Transfer the

reagent to a $50\mathrm{.}0mL$ volumetric flask, add water to the line, and mix 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

$35\mathrm{.}0ppm.$ Use a graduated cylinder to transfer a portion of the more concentrated solution to a $50\mathrm{.}0mL$ volumetric

flask and dilute to the line with water to create a solution with a concentration of $35\mathrm{.}0ppm.$

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

$35\mathrm{.}0ppm.$ Use a pipet to transfer a portion of the concentrated solution to a separate $50\mathrm{.}0mL$ volumetric flask and

dilute to the line with water to create a solution with a concentration of $35\mathrm{.}0ppm.$

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 $50\mathrm{.}0mL$ of water. Combine the reagent and water in a $50\mathrm{.}0mL$ volumetric flask and

mix it thoroughly.