How to Calculate the Amount of Iron(III) Chloride for Solution

How to calculate the amount of iron(III) chloride needed to make a specific molarity solution using water?

Given data: In the laboratory, you are asked to make a 0.149 M iron(III) chloride solution using 475 grams of water. How many grams of iron(III) chloride should you add?

Add 47.45 grams of iron(III) chloride to make a 0.149 M solution using 475 grams of water.

When calculating the amount of iron(III) chloride needed to create a specific molarity solution using water, there are a few key steps to follow. First, you need to determine the molecular weight of iron(III) chloride. In this case, the molecular weight is known to be 162.2 g/mol.

Next, you will need to calculate the number of moles of iron(III) chloride required to achieve a 0.149 M solution. Molarity is defined as the number of moles of solute per liter of solution. Since 475 grams of water are used, it needs to be converted to liters. This can be done by dividing the weight of water by the density of water, which is 1 g/mL or 1000 g/L.

After converting the weight of water to liters, the number of moles of iron(III) chloride needed can be calculated by multiplying the molarity by the volume of water in liters. Once the moles are determined, the grams of iron(III) chloride can be calculated by multiplying the number of moles by the molecular weight.

Subtracting the weight of water from the total weight of the solution will give you the final amount of iron(III) chloride needed. In this case, 47.45 grams of iron(III) chloride should be added to make a 0.149 M solution using 475 grams of water.