Question

An aqueous solution of iron(II) sulfate (FeSO4) is prepared by dissolving 2.75 g in sufficient deionized water to form a 150.00 mL solution. Calculate the molarity of the solution.

Answer 1

Answer: The molarity of iron(II) sulfate solution is 0.724 M

Step-by-step explanation:

To calculate the molarity of solution, we use the equation:

`\text{Molarity of the solution}=\frac{\text{Mass of solute}* 1000}{\text{Molar mass of solute}* \text{Volume of solution (in mL)}}`

We are given:

Given mass of iron(II) sulfate = 2.75 g

Molar mass of iron(II) sulfate = 152 g/mol

Volume of solution = 150.0 mL

Putting values in above equation, we get:

`\text{Molarity of iron(II) sulfate}=(2.75* 1000)/(152* 25.0)\\\\\text{Molarity of iron(II) sulfate}=0.724M`

Hence, the molarity of iron(II) sulfate solution is 0.724 M