Answered

From health tips to tech hacks, find it all on IDNLearn.com. Our platform provides accurate, detailed responses to help you navigate any topic with ease.

A chemist must dilute 97.1 ml of aqueous magnesium fluoride solution until the concentration falls to 389 microMolarity . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to significant digits.

Sagot :

Jufsanabriasaidn

Answer:

0.302L

Explanation:

...97.1mL of 1.21m M aqueous magnesium fluoride solution

In this problem the chemist is disolving a solution from 1.21mM = 1.21x10⁻³M, to 389μM = 389x10⁻⁶M. That means the solution must be diluted:

1.21x10⁻³M / 389x10⁻⁶M = 3.11 times

As the initial volume of the original concentration is 97.1mL, the final volume must be:

97.1mL * 3.11 = 302.0mL =

0.302L

Thank you for contributing to our discussion. Don't forget to check back for new answers. Keep asking, answering, and sharing useful information. IDNLearn.com is your reliable source for accurate answers. Thank you for visiting, and we hope to assist you again.