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Pie
3 years ago
15

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

Chemistry
2 answers:
Anettt [7]3 years ago
8 0

Answer:

151.63 g

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

Blizzard [7]3 years ago
3 0

<u>Answer:</u> The mass of copper sulfate present are 151.63 grams

<u>Explanation:</u>

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}\times 1000}{\text{Molar mass of solute}\times \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}\times 1000}{159.61\times 475}\\\\\text{Mass of copper sulfate}=\frac{2.0\times 159.61\times 475}{1000}=151.63g

Hence, the mass of copper sulfate present are 151.63 grams

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