To what volume should you dilute 150.0 ml of an aqueous 4.00 M potassium phosphate solution so that the final solution is 1.00 M? 1,200 mL 200 mL 0.0267 L 600 mL 0.150 L
To what volume should you dilute 150.0 ml of an aqueous 4.00 M potassium phosphate solution so that the final solution is 1.00 M? 1,200 mL 200 mL 0.0267 L 600 mL 0.150 L
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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To what volume should you dilute 150.0 ml of an aqueous 4.00 M potassium phosphate solution so that the final solution is 1.00 M?
1,200 mL |
||
200 mL |
||
0.0267 L |
||
600 mL |
||
0.150 L |
Expert Solution
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Step 1
The process of dilution is defined as the process in which a solution with a lower concentration is prepared from a solution with the higher concentration by adding an appropriate amount of water.
When a dilute solution is made, more solvent is added. The number of moles of the solute does not change, what changes is the concentration.
The dilution equation is,
M1V1 = M2V2
- M1 and V1 are the molar concentration and volume of the initial concentrated solution.
- M2 and V2 are the molar concentration and volume of the final dilute solution.
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