Final Concentration: 40 µMol from .01mL Stock Solution

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To find the final concentration after adding 0.01 mL of a 40 µM stock solution to 0.98 mL of water, the total volume becomes 0.99 mL. The number of moles remains constant, so the initial moles can be calculated using the formula M1V1 = M2V2. By applying this equation, the final concentration can be determined. The final concentration of the solution is approximately 0.404 µM. Understanding the relationship between initial and final concentrations is crucial for accurate calculations.
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if i have a 40 micromolar concentration of stock solution and add .01 mL of that solution to .98mL of water, what is my final concentration.

Thanks for any help!
 
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NCollege4Life said:
if i have a 40 micromolar concentration of stock solution and add .01 mL of that solution to .98mL of water, what is my final concentration.

Thanks for any help!

What is the final volume of your solution?
 
sorry! .99 mL
 
Does the number of moles in the final solution differ from the number of moles in initial solution?

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no, same
 
Last edited:
so any help?
 
Use the equation relating the initial molarity to the final molarity and volume:

M1V1 = M2V2
 
NCollege4Life said:
so any help?

My question was a hint. If amount of substance have not changed, why don't you calculate initial amount of substance and use concentration definition to calculate final concentration?

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