Toxic cyanide ions can be removed from wastewater by adding...

Toxic cyanide ions can be removed from wastewater by adding hypochlorite. $2 \mathrm{CN}^{-}(a q)+5 \mathrm{OCl}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow$ $$ \mathrm{N}_{2}(g)+2 \mathrm{HCO}_{3}^{-}(a q)+5 \mathrm{Cl}^{-}(a q) $$ a. If $1.50 \times 10^{3} \mathrm{L}$ of $0.125 M \mathrm{OCl}^{-}$ are required to remove the $\mathrm{CN}^{-}$ in $3.4 \times 10^{6} \mathrm{L}$ of wastewater, what is the $\mathrm{CN}^{-}$ concentration in the water in $\mathrm{mg} / \mathrm{L} ?$ "b. How many milliliters of $0.575 \mathrm{M} \mathrm{Ag} \mathrm{NO}_{3}$ would you need to add to a $50.00 \mathrm{mL}$ aliquot of the final solution (consider the volumes simply additive) to precipitate the chloride ions formed in the reaction?

Toxic cyanide ions can be removed from wastewater by adding hypochlorite. $2 \mathrm{CN}^{-}(a q)+5 \mathrm{OCl}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow$
$$
\mathrm{N}_{2}(g)+2 \mathrm{HCO}_{3}^{-}(a q)+5 \mathrm{Cl}^{-}(a q)
$$
a. If $1.50 \times 10^{3} \mathrm{L}$ of $0.125 M \mathrm{OCl}^{-}$ are required to remove the $\mathrm{CN}^{-}$ in $3.4 \times 10^{6} \mathrm{L}$ of wastewater, what is the $\mathrm{CN}^{-}$ concentration in the water in $\mathrm{mg} / \mathrm{L} ?$
"b. How many milliliters of $0.575 \mathrm{M} \mathrm{Ag} \mathrm{NO}_{3}$ would you need to add to a $50.00 \mathrm{mL}$ aliquot of the final solution (consider the volumes simply additive) to precipitate the chloride ions formed in the reaction?

Key Concepts

Reaction Stoichiometry

This concept involves using the balanced chemical equation to relate the number of moles of one substance to another. It is crucial for determining how many moles of reactants are needed or produced during the reaction and for converting between reactant and product amounts.

Molarity and Dilution

Molarity defines the concentration of a solution in terms of moles of solute per liter of solution. Understanding this concept allows one to calculate the total number of moles in a given volume of solution and is essential when working with reactions carried out in different volumes or when diluting solutions.

Unit Conversion

This involves converting between different units, such as moles to mass (mg, g), or liters to milliliters. It is important for expressing the final concentration in the required units, such as mg/L, and for working with various volume measurements in chemical calculations.

Precipitation Reactions

Precipitation reactions occur when two soluble salts react and one of the products is an insoluble solid. In this context, the formation of a precipitate with silver nitrate is used to remove or measure chloride ions in solution, which involves understanding the reaction between AgNO3 and Cl-.

Volumetric Analysis

This method uses the volumes of solutions of known concentration to determine the amount of an analyte. It is particularly useful in titration scenarios where the volume of a titrant required to completely react with a species (such as chloride ions) is measured, allowing for the calculation of its concentration.

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