We used the very handy equation (C) * (V1) = (C2 )* (V2) to calculate our final

Q: We used the very handy equation (C) * (V1) = (C2 )* (V2) to calculate our final

a. C1= 50 mM C2=? V1= 200 microlitre= 0.002 ml V2= 10 ml C2= V1*C1/V2 = 0.01 mM b) V1=? C2=2.5 mM V2=10 ml C1= 50 mM V1= 0.5 ml c) concentration= 50 mM=0.05 moles that means 0.05 moles present in 1000 ml moles present in 25 ml= (0.05/1000)*25 = 1.25x10^-3 moles

ID: 980184 • Letter: W

Question

We used the very handy equation (C) * (V1) = (C2 )* (V2) to calculate our final concentrations in our tubes. In this equation, C1 is the concentration of the solution that we are given (diluting) and C2 is the concentration after diluting. Please consider a slightly different situation in which we have a 50.0 mM solution and we are diluting it into a final volume of 10.0 ml. What would the final concentration be if we used 200 microliters of our starting solution with a 10.0 ml final volume? What volume of our starling solution would be need to use to get a final concentration of 2.5 mM in 10.0 ml? How much of the substance is present in 2.5 ml of the 50.0 mM starting solution?

Explanation / Answer

C1= 50 mM

C2=?

V1= 200 microlitre= 0.002 ml

V2= 10 ml

C2= V1*C1/V2

= 0.01 mM

V1=?

C2=2.5 mM

V2=10 ml

C1= 50 mM

V1= 0.5 ml

concentration= 50 mM=0.05 moles

that means 0.05 moles present in 1000 ml

moles present in 25 ml= (0.05/1000)*25 = 1.25x10^-3 moles

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We used the very handy equation (C) * (V1) = (C2 )* (V2) to calculate our final

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