Question

A chemist prepares a solution of copper(II) sulfate by measuring out of copper(II) sulfate into a volumetric flask and filling the flask to the mark with water. Calculate the concentration in of the chemist's copper(II) sulfate solution. Round your answer to significant digits.

Answer 1

0.5000

Step-by-step explanation:

We can measure the concentration of the copper sulfate solution as 1.000 mol/L. Since the tank contains one half liter, the solution contains 0.5000 moles of copper sulfate.

Answer 2

The question is incomplete, here is the complete question:

A chemist prepares a solution of copper(II) sulfate
`(CuSO_4)` by measuring out 69.2 g of copper(II) sulfate into a 400. mL volumetric flask and filling the flask to the mark with water.

Calculate the concentration in mol/L of the chemist's copper(II) sulfate solution. Round your answer to 3 significant digits.

Answer: The molarity of copper (II) sulfate solution is 1.08 mol/L

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 copper (II) sulfate = 69.2 g

Molar mass of copper (II) sulfate = 159.6 g/mol

Volume of solution = 400. mL

Putting values in above equation, we get:

`\text{Molarity of solution}=(69.2* 1000)/(159.6* 400)\\\\\text{Molarity of solution}=1.08M`

Hence, the molarity of copper (II) sulfate solution is 1.08 mol/L