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To what volume should you dilute 65 mL of a 10.0 M [tex]H_2SO_4[/tex] solution to obtain a 1.55 M [tex]H_2SO_4[/tex] solution?

Express your answer in milliliters using two significant figures.

Answer :

To dilute 65 mL of a 10.0 M H₂SO₄ solution to obtain a 1.55 M H₂SO₄ solution, you should dilute it to a volume of 4.125L (liters) expressed to two significant figures.

Let us learn how to dilute a solution. Dilution is a process that can be used to reduce the concentration of a solution. A concentrated solution of a known concentration is often diluted with solvent to prepare a more dilute solution.

The following formula can be used to calculate the concentration of a solution after dilution: C₁V₁ = C₂V₂

Where,

C₁ = initial concentration of the solution

V₁ = volume of the initial solution

C₂ = final concentration of the solution

V₂ = final volume of the solution

To find the final volume of the solution, we can rearrange the formula as follows: V₂ = (C₁V₁) / C₂

Substituting the values given into the equation:

V₂ = (10.0 mol/L × 0.065 L) / 0.155 mol/L V₂ = 4.1935 L

We then round this value to two significant figures to get the final answer: V₂ = 4.19 L (rounded to two significant figures).

However, we must note that the volume of the concentrated solution must be larger than the volume of the diluted solution. Therefore, we can subtract the final volume from the initial volume to find the volume of solvent required to dilute the concentrated solution:

Volume of solvent = V₂ - V₁

Volume of solvent = 4.19 L - 0.065 LV = 4.125 L.

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