A sample of 17.0 M concentrated H2SO4 stock solution with a volume of 25.0 cm3 was diluted to final concentration of 5.0 M H2SO4 solution. Calculate, what is the amount of water that would be required to dilute the concentrated H2SO4 solution to a final concentration of 5.0 M?

60 cm³ of water

Explanation:

We'll begin by calculating the volume of the diluted solution. This can be obtained as follow:

Concentration of stock solution (C₁) = 17 M

Volume of stock solution (V₁) = 25 cm³

Concentration of diluted solution (C₂) = 5 M

Volume of diluted solution (V₂) =?

C₁V₁ = C₂V₂

17 × 25 = 5 × V₂

425 = 5 × V₂

Divide both side by 5

V₂ = 425 / 5

V₂ = 85 cm³

Thus, the volume of the diluted solution is 85 cm³

Finally, we shall determine the volume of water needed to dilute the solution. This can be obtained as follow:

Volume of stock solution (V₁) = 25 cm³

Volume of diluted solution (V₂) = 85 cm³

Volume of water =?

Volume of water = V₂ – V₁

Volume of water = 85 – 25

Volume of water = 60 cm³

Therefore, 60 cm³ of water is needed to dilute the solution.

c, liquids evaporate, creating a gas

2b2t

explanation:

2b2t