Final Concentration: 40 µMol from .01mL Stock Solution

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Discussion Overview

The discussion revolves around calculating the final concentration of a solution after diluting a stock solution with water. Participants explore the relationship between initial concentration, volume, and final concentration, focusing on the implications of dilution in a chemical context.

Discussion Character

  • Mathematical reasoning
  • Technical explanation
  • Homework-related

Main Points Raised

  • One participant asks for the final concentration after diluting a 40 micromolar stock solution with 0.01 mL of the stock and 0.98 mL of water.
  • Another participant requests clarification on the final volume of the solution, which is later confirmed to be 0.99 mL.
  • A question is posed regarding whether the number of moles in the final solution differs from the initial solution.
  • One participant asserts that the number of moles remains the same after dilution.
  • Another participant suggests using the equation M1V1 = M2V2 to relate initial and final concentrations and volumes.
  • A later reply hints at calculating the initial amount of substance to determine the final concentration, emphasizing the definition of concentration.

Areas of Agreement / Disagreement

Participants express differing views on the approach to calculating final concentration, with some focusing on the relationship between moles and concentration while others emphasize the use of the dilution equation. The discussion remains unresolved regarding the best method to calculate the final concentration.

Contextual Notes

There are assumptions about the uniformity of the solution and the definitions of concentration that are not explicitly stated. The discussion does not resolve the mathematical steps involved in the calculations.

NCollege4Life
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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?

--
methods
 
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?

--
methods
 

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