The question is incomplete, here is the complete question:
A chemist adds 370.0 mL of a 2.25 M iron(III) bromide solution to a reaction flask. Calculate the mass in grams of iron(III) bromide the chemist has added to the flask. Round your answer to 3 significant digits
Answer: The mass of iron (III) bromide is 246. grams
Explanation:
To calculate the mass of solute, we use the equation used to calculate the molarity of solution:
[tex]\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}[/tex]
We are given:
Molarity of solution = 2.25 M
Molar mass of iron (III) bromide = 295.6 g/mol
Volume of solution = 370.0 mL
Putting values in above equation, we get:
[tex]2.25M=\frac{\text{Mass of solute}\times 1000}{295.6\times 370.0}\\\\\text{Mass of solute}=\frac{2.25\times 295.6\times 370.0}{1000}=246.1g[/tex]
Hence, the mass of iron (III) bromide is 246. grams
