Question

A chemist prepares a solution of iron(II) bromide FeBr2 by measuring out 224.g of iron(II) bromide into a 300.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mo/L of the chemist's iron(II) bromide solution. Round your answer to 3 significant digits.

Answer 1

Answer: The molarity of iron(II) bromide solution is 3.46 M

Explanation:

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

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

We are given:

Given mass of iron(II) bromide = 224. g

Molar mass of iron(II) bromide = 215.65 g/mol

Volume of solution = 300. mL

Putting values in above equation, we get:

$\text{Molarity of solution}=\frac{224\times 1000}{215.65g/mol\times 300}\\\\\text{Molarity of solution}=3.46M$

Hence, the molarity of iron(II) bromide solution is 3.46 M