Question

How many of grams of CuSO4 are in 475ml of a 2.0M aqueous solution

Answer 1

Answer: The mass of copper sulfate present are 151.63 grams

Step-by-step 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}* 1000}{\text{Molar mass of solute}* \text{Volume of solution (in mL)}}`

We are given:

Molarity of solution = 2.0 M

Molar mass of copper sulfate = 159.61 g/mol

Volume of solution = 475 mL

Putting values in above equation, we get:

`2.0M=\frac{\text{Mass of copper sulfate}* 1000}{159.61* 475}\\\\\text{Mass of copper sulfate}=(2.0* 159.61* 475)/(1000)=151.63g`

Hence, the mass of copper sulfate present are 151.63 grams

Answer 2

151.63 g

Step-by-step explanation:

We first get the number of moles;

Moles = Molarity × volume

= 2.0 × 0.475

= 0.95 moles

1 mole of CuSO4 = 159.609 g/mol

Therefore;

Mass = moles × molar mas

= 0.95 moles × 159.609 g/mol

= 151.63 g