Question

A chemist adds 0.45 L of a 1.08 * 10M zinc oxalate (ZnC,0) solution to a reaction flask. Calculate the mass in milligrams of incolate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Answer 1

Answer: The mass of zinc oxalate, the chemist has added is $7.6\times 10^5mg$

Explanation:

To calculate the mass of solute, we use the equation used to calculate the molarity of solution:

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

We are given:

Molarity of solution = $1.08\times 10M=10.8M$

Molar mass of zinc oxalate = 155.4 g

/mol

Volume of solution = 0.45 L

Putting values in above equation, we get:

$10.8M=\frac{\text{Mass of zinc oxalate}}{155.4g/mol\times 0.45L}\\\\\text{Mass of zinc oxalate}=(10.8mol/L\times 155.4g/mol\times 0.45L)=7.6\times 10^2g$

To convert the calculated mass into milligrams, we use the conversion factor:

1 g = 1000 mg

So, $7.6\times 10^2g\times \frac{1000mg}{1g}=7.6\times 10^5mg$

Hence, the mass of zinc oxalate, the chemist has added is $7.6\times 10^5mg$