You have an unknown dye solution whose concentration seems to lie between a 0.00

Question

You have an unknown dye solution whose concentration seems to lie between a 0.0006 M stock solution and a 0.0004 M stock solution. Therefore, you had planned to dilute the 0.0006 M stock to create your calibration standards. However, you see that there is no 0.0006 M stock left, but there is plenty of 0.0004 M stock.

a. How could you raise the concentration of some of the 0.0004 M stock to make 75 mL of a 0.0006 M solution without adding any more dye? Be sure to show calculations and indicate the volume of 0.0004 M required.

b. Draw a molecular view picture illustrating the moles of dye remaining constant during this process.

I have an idea of how to solve a. but I don't know how to draw the molecular view. Thank you so much in advance :)

Explanation / Answer

initial volume V1 = 75ml

initial molarity M1 = 0.0006M

final volume V2   =

final molarity M2 = 0.0004M

M1V1   = M2V2

V2    = M1V1/M2

      = 0.0006*75/0.0004   = 112.5ml

volume of water neede = 112.5-75 = 37.5ml only pure water no dye dissolve

        =

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