What is the molarity of a solution that is prepared by diluting 40.0 mL of a 0.200 M Fe2(SO4)3...

Question:

What is the molarity of a solution that is prepared by diluting 40.0 mL of a 0.200 M {eq}Fe_2(SO_4)_3 {/eq} solution to a volume of 1500 mL?

Dilution:

If you already have a solution prepared but the experiment or assay requires a solution with a lower concentration, dilution will be done. Here, an aliquot of the prepared solution will be mixed with a particular volume of the solvent. For quantitative purposes, dilution is done using a volumetric flask since a volumetric flask is calibrated to a specific volume.

Answer and Explanation: 1


The equation that will be used is:

{eq}C1V1 = C2V2 {/eq}

where:

  • C1 - concentration of the stock solution (0.200 M)
  • V1 - volume of the stock solution (40.0 mL)
  • C2 - concentration of the desired solution (unknown)
  • V2 - volume of the desired solution (1500 mL)

The equation will be rearranged such that the C2 will be isolated on one side of the equation. With that, the final concentration of the solution will be calculated.

{eq}C2 = \dfrac{C1V1}{V2} {/eq}

{eq}\rm C2 = \dfrac{0.200\ M \times 40.0\ mL}{1500\ mL} = \boxed{\mathbf{5.33 \times 10^{-3}\ M\ fe_2(SO_4)_3}} {/eq}


Learn more about this topic:

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Calculating Dilution of Solutions

from

Chapter 8 / Lesson 5
93K

Want to know how to calculate dilution factor? See dilution equations, the dilution formula, and learn how to dilute acid and how to dilute a solution.


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