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You wish to make a 0.310 M hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Submit Answer Retry Entire Group 9 more group attempts remaining

You wish to make a 0.310 M hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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You wish to make a 0.310 M hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Submit Answer Retry Entire Group 9 more group attempts remaining
Transcribed Image Text:You wish to make a 0.310 M hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Submit Answer Retry Entire Group 9 more group attempts remaining
In the laboratory you dilute 4.85 mL of a concentrated 12.0 M hydrobromic acid solution to a total volume of 175 mL. What is the concentration of the dilute solution? M Submit Answer Retry Entire Group 9 more group attempts remaining
Transcribed Image Text:In the laboratory you dilute 4.85 mL of a concentrated 12.0 M hydrobromic acid solution to a total volume of 175 mL. What is the concentration of the dilute solution? M Submit Answer Retry Entire Group 9 more group attempts remaining
Expert Solution
Step 1

To solve this problem we will use the formula of dilutions law , which is given as 

M1V1 = M2V2 

Where, M1 = molarity of initial solution

              V1 = volume of initial solution

              M2 = molarity of final solution 

              V2 = volume of final solution 

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