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

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

C1 * V1 = C2 * V2 C1 = 50 mM V2 = 10 mL a) V1 = 200 L = 0.2 mL C2 = 50 * 0.2 / 10 = 1 mM b) C2 = 2.5 mM V1 = 2.5 * 10 / 50 = 0.5 mL c) V1 = 2.5 mL C1 * V1 = 50 * 2.5 / 1000 mMol = 0.125 mMol

ID: 482395 • Letter: W

Question

We used the very handy equation (C) * (VI) = (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 starting solution would be need to use to get a final concentration c 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 * V1 = C2 * V2

C1 = 50 mM

V2 = 10 mL

V1 = 200 L = 0.2 mL

C2 = 50 * 0.2 / 10

= 1 mM

C2 = 2.5 mM

V1 = 2.5 * 10 / 50

= 0.5 mL

V1 = 2.5 mL

C1 * V1 = 50 * 2.5 / 1000 mMol

= 0.125 mMol

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

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