Asked by Chopsticks
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
Where
M1 = 3.00M
V1 = 225mL
M2 = 12.1M
V2 = ?
(3.00M)(225mL)/12.1M = 55.8mL
Is that correct?
Acid: HCl
Molarity of Concentrated Reagent: 12.1M
I'm guessing you use the M1V1=M2=V2 formula
Where
M1 = 3.00M
V1 = 225mL
M2 = 12.1M
V2 = ?
(3.00M)(225mL)/12.1M = 55.8mL
Is that correct?
Answers
Answered by
DrBob222
That looks ok to me.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.