How would you prepare 1.00 L of a 0.400 M solution of copper(II) sulfate, CuSO\(_4\)?

We need to dilute 0.400 mol of copper (II) sulfate, how do we know, how many weigh of C u S O 4 ​ we have to dilute??
It's simple.
η = MM m ​
Using a periodic table we can find the molar mass of C u , S an d O
M M C u S O 4 ​ ​ = 153.9 g / m o l
Then
m = η ∗ MM
now we can replace it
m = 0.400 ∗ 159.6
m = 63.84 g ​ ​
Then we have to dilute 63.84 grams of copper (II) sulfate in 1 L of water to obtain a solution with 0.400M

Answered by D3xt3R | 2024-06-10

To calculate the number of moles for given molarity, we use the equation:
Molarity of the solution = Volume of solution (in L) Moles of solute ​
Molarity of copper(II)sulfate solution = 0.400 M
Volume of solution = 1.00 L
Putting values in above equation, we get:
0.400 M = 1.00 L Moles of copper(II)sulfate ​ Moles of copper(II)sulfate = ( 0.400 m o l / L × 1.00 L ) = 0.400 m o l
To calculate the mass of copper(II)sulfate for given number of moles, we use the equation:
Number of moles = Molar mass Given mass ​
Molar mass of copper(II)sulfate = 159.61 g/mol
Moles of copper(II)sulfate = 0.400 moles
Putting values in above equation, we get:
0.400 m o l = 159.61 g / m o l Mass of copper (II) sulfate ​ Mass of copper (II) sulfate = ( 0.400 m o l × 159.61 g / m o l ) = 63.8 g
Hence, to prepare the solution of given molarity, we add 63.8 g of copper (II) sulfate to the solution.

Answered by Anonymous | 2024-06-12

To prepare a 0.400 M solution of copper(II) sulfate, weigh 63.85 grams of CuSO₄, dissolve it in less than 1.00 L of water, and then dilute the solution to a total volume of 1.00 L. This ensures that you achieve the desired molarity. Finally, always label your solution correctly for future reference.
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Answered by D3xt3R | 2024-12-23