The question is incomplete, here is the complete question:
A chemist prepares a solution of copper(II) sulfate [tex](CuSO_4)[/tex] 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
Explanation:
To calculate the molarity of solution, we use the equation:
[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:
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:
[tex]\text{Molarity of solution}=\frac{69.2\times 1000}{159.6\times 400}\\\\\text{Molarity of solution}=1.08M[/tex]
Hence, the molarity of copper (II) sulfate solution is 1.08 mol/L
Answer:
0.5000
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.
