Question

A chemist must dilute 73.6mL of 87.6mM aqueous potassium dichromate(K2Cr2O7)solution until the concentration falls to 54.0 mM . She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to significant digits

Answer 1

0.119 L

Step-by-step explanation:

To dilute the potassium dichromate solution, we can use the equation for dilution:

C1V1 = C2V2

Where:

C1 = Initial concentration of the solution (87.6 mM)

V1 = Initial volume of the solution (73.6 mL)

C2 = Final concentration of the solution (54.0 mM)

V2 = Final volume of the solution (to be calculated)

Let's plug in the given values into the equation and solve for V2:

(87.6 mM)(73.6 mL) = (54.0 mM)(V2)

(87.6 mM)(73.6 mL) / 54.0 mM = V2

V2 = (87.6 mM * 73.6 mL) / 54.0 mM

V2 ≈ 119.35 mL

Finally, we need to convert the volume from milliliters to liters:

V2 = 119.35 mL / 1000 mL/L

V2 ≈ 0.11935 L

Rounding to significant digits, the final volume is approximately 0.119 L.