Question

An aqueous solution of ammonia is available that has a concentration of 13.4 m and an aqueous solution of perchloric acid is available with a concentration of 11.7 m.

Based on the mass of NH₄ClO₄ needed, as calculated in question 1, what volume of a 13.4 M NH₃ solution will be required to produce that amount of NH₄ClO₄?

Answer 1

To calculate the volume of a 13.4 M NH3 solution required, convert the mass of NH4ClO4 needed to moles using its molar mass.

Step-by-step explanation:

To calculate the volume of a 13.4 M NH3 solution needed to produce a certain amount of NH4ClO4. This is based on the stoichiometry of the reaction between NH3 (ammonia) and HClO4 (perchloric acid), which is a 1:1 ratio since one mole of NH3 reacts with one mole of HClO4 to produce one mole of NH4ClO4.

The mass of NH4ClO4 needed was calculated previously, so we divide that mass by the molar mass of NH4ClO4 to find the number of moles required. We then use the equation Molarity (M) = moles of solute/Liters of solution to find the volume of the NH3 solution.

If the exact mass of NH4ClO4 required is unknown, further data would be needed to provide a precise answer. However, the basic approach would be the same: convert the mass of NH4ClO4 to moles, and then use the molarity of the NH3 solution to find the required volume to produce that amount of NH4ClO4.