I'm not sure how to answer this question and how to set it up.
To what volume should you dilute 90mL of a 10.5M H2SO4 solution to obtain a 1.65M H2SO4 solution?
To find out the volume to which you need to dilute a 10.5M H2SO4 solution to obtain a 1.65M H2SO4 solution, you can use the formula for dilution:
\(C_1V_1 = C_2V_2\)
Where:
\(C_1\) = concentration of the initial solution
\(V_1\) = volume of the initial solution
\(C_2\) = concentration of the final solution
\(V_2\) = volume of the final solution
In this case:
\(C_1 = 10.5M\)
\(C_2 = 1.65M\)
\(V_1 = 90mL\) (or 0.09L)
To find \(V_2\), we can rearrange the formula:
\(V_2 = \frac{{C_1V_1}}{{C_2}}\)
Substituting the values we have:
\(V_2 = \frac{{10.5 \times 0.09}}{{1.65}}\)
\(V_2 \approx 0.571L\) (or 571mL)
Therefore, you should dilute 90mL of the 10.5M H2SO4 solution to a final volume of approximately 571mL (0.571L) to obtain a 1.65M H2SO4 solution.
To determine the volume needed to achieve a desired concentration, we can use the dilution formula:
C1V1 = C2V2
Where:
C1 = Initial concentration
V1 = Initial volume
C2 = Final concentration
V2 = Final volume
In this case, we are given:
C1 = 10.5 M (Initial concentration)
V1 = 90 mL (Initial volume)
C2 = 1.65 M (Final concentration)
We need to find V2, which is the final volume. Rearranging the equation, we have:
V2 = (C1 * V1) / C2
Plugging in the given values:
V2 = (10.5 M * 90 mL) / 1.65 M
Simplifying the equation:
V2 = 10.5 * 90 / 1.65
V2 = 577.5 / 1.65
V2 ≈ 350.91 mL
Therefore, to obtain a 1.65M H2SO4 solution, you should dilute 90 mL of a 10.5M H2SO4 solution with approximately 350.91 mL of solvent (usually water) to a total volume of 441 mL.