Many labs keep bottles of 3.0M solutions of the common acid on hand. Given the following molarities of the concentrated acids, determine how many mL of each concentrated acid would be required to prepare 225mL of a 3.00M solution of the acid

Acid: HCl
Molarity of Concentrated Reagent: 12.1M

I'm guessing you use the M1V1=M2=V2 formula


M1 = 3.00M
V1 = 225mL
M2 = 12.1M
V2 = ?

(3.00M)(225mL)/12.1M = 55.8mL

Is that correct?

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  1. That looks ok to me.

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