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What is the molarity of a 250ml KCl solution made by diluting 175mL of a 3.00 M solution?

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1 vote

Answer:

2.1 M

Step-by-step explanation:

The dilution equation is
M_(s) V_(s) = M_(d) V_(d).


M_(s) = the molarity of the sock solution


V_(s) = the volume of the sock solution


M_(d) = the molarity of the diluted solution


V_(d) = the volume of the diluted solution

The stock solution would be what is doing the diluting, so "175 mL of a 3.00 M solution". So
M_(s) = 3.00 M. Then: Converting 175 mL to liters:
175 mL * (1 L)/(1000mL) = 0.175 L (This is
V_(s))

And converting 250 mL KCl to liters:
250 mL * (1 L)/(1000mL) = 0.250 L (This will be
V_(d))

Then, we plug in our given into the dilution equation, resulting in:


3.00 M * 0.175 L = M_(d) * 0.250 L (divide both sides by 0.250 L, in order to get
M_(d) by itself)


(3.00 M * 0.175 L)/(0.250 L) = M_(d)


M_(d) = 2.1 M

So, the molarity of 250 mL KCl made by diluting 175 mL of a 3.0 M solution would be 2.1 M (mol/L).

Hopefully this helped you understand the topic a little bit better. I just finished molarity and dilutions in Chemistry last week. Good luck!

User Syd
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