Respuesta :
Answer:
328 ml
Explanation:
We have given final volume =575.2 ml=0.575 L
Final concentration = 0.8012 M
We know that moles of copper(II) nitrate = final volume ×final concentration =0.8012×.0575=0.4606 moles
We have to find initial volume
So initial volume [tex]=\frac{moles\ of \ copper(II)\ nitrate}{initial\ concentration}=\frac{0.4606}{1.403}=0.328L=328ml[/tex]
The volume of the copper(II) nitrate solution that must be diluted is 328.5 mL
Dilution
From the question, we are to determine the volume of copper(II) nitrate that must be diluted
Using the dilution law
M₁V₁ = M₂V₂
Where M₁ is the initial concentration
V₁ is the initial volume
M₂ is the final concentration
and V₂ is the final volume
From the given information
M₁ = 1.403 M
V₁ = ?
M₂ = 0.8012 M
V₂ = 575.2 mL
Putting the values into the equation, we get
1.403 × V₁ = 0.8012 × 575.2
[tex]V_{1} = \frac{0.8012 \times 575.2}{1.403}[/tex]
[tex]V_{1} = \frac{460.85024}{1.403}[/tex]
V₁ = 328.5 mL
Hence, the volume of the copper(II) nitrate solution that must be diluted is 328.5 mL
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