You want to prepare a ten-fold dilution of a 20% dye solution.

a) How much of the 20% dye do you need to use to make 1 mL total volume of the ten-fold dilution? 0.1 mL

b) What will the dye concentration of the dilution be? 2%

Question

You want to prepare a ten-fold dilution of a 20% dye solution.

a) How much of the 20% dye do you need to use to make 1 mL total volume of the ten-fold dilution? 0.1 mL

b) What will the dye concentration of the dilution be? 2%

BlackTom AI · Accepted Answer

To tackle a dilution problem, I’ll apply the C1V1 = C2V2 relationship, which connects the concentration and volume before and after dilution.

First part: determining how much 20% dye to add to reach a total 1 mL at the diluted concentration.
- Given: C1 = 20% (stock), C2 = 2% (diluted), V2 = 1 mL (final volume).
- Solve for V1: V1 = (C2 × V2) / C1 = (2% × 1 mL) / 20% = 0.1 mL.
- Therefore, you need 0.1 mL of the 20% dye and dilute it to a total volume of 1 mL.

Second part: confirming the dye concentration of the dilution.
- By design, this is a ten-fold dilution, which should reduce concentration by a factor of 10, from 20% to 2%. The calculation above also yields C2 = (C1 × V1) / V2 = (20% × 0.1 mL) / 1 mL = 2%, matching the stated goal.
- The result is consistent with the dilution factor: a ten-fold (10×) dilution of a 20% solution gives a 2% solution in 1 mL.

Common pitfall to avoid: assuming a different final volume or misreading the dilution factor could lead to incorrect V1 or C2. Keeping track of units and applying C1V1 = C2V2 helps prevent that error.

In summary, 0.1 mL of the 20% dye is required to make 1 mL of a 2% (ten-fold diluted) solution, and the resulting dye concentration is indeed 2%.

W25 BIOL D006B 01Y Cell & Molecular Biology Lab 1A Pre-lab Quiz

You want to prepare a ten-fold dilution of a 20% dye solution. a) How much of the 20% dye do you need to use to make 1 mL total volume of the ten-fold dilution? 0.1 mL b) What will the dye concentration of the dilution be? 2%

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