Question

Calculate the Volume needed to prepare 0.25 moles of a 3.52 M NH₄Cl solution

Answer 1

To prepare 0.25 moles of a 3.52 M NH4Cl solution, the volume needed is calculated by dividing the moles of solute by the molarity, resulting in 71.0 mL of solution.

Step-by-step explanation:

To calculate the volume needed to prepare 0.25 moles of a 3.52 M NH4Cl solution, we first need to use the definition of molarity (M). Molarity is the number of moles of a solute divided by the volume of solution in liters.

Step-by-Step Solution:

1. Determine the number of moles needed. We know we need 0.25 moles of NH4Cl.
2. Use the molarity equation:

Molarity (M) = Moles of solute / Volume of solution in liters (L)

We have the molarity (3.52 M) and the moles of solute (0.25 moles), so we can rearrange the equation to solve for volume:

Volume of solution in liters (L) = Moles of solute / Molarity (M)

Volume of solution in liters (L) = 0.25 moles / 3.52 M

Volume of solution in liters (L) = 0.0710 L

To prepare 0.25 moles of a 3.52 M NH4Cl solution, 71.0 mL of solution is needed (since 1 L = 1000 mL).