How much of a stock solution of 10.0 mg/L phosphate standard, do you need to use to make a final solution containing a volume of 3 mL and 5.8 mg/L phosphate? Enter your numerical answer to one decimal place and do not enter any text; the units are assumed to be milliliters.
Added by Cindy C.
Close
Step 1
We have a stock solution with a concentration of 10.0 mg/L. Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 62 other Biology educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
What volume of a 5.0 x 10^(-1) M stock solution of Na3PO4 must be used to make 250 mL of a solution that is 3.8 x 10^(-3) M in phosphate ions? 0.0075 mL 0.63 mL 1.9 mL 3.3 mL
Susan H.
If a chemist wishes to dilute a 1.000 Ă— 103 mg/L stock solution to prepare 5.000 Ă— 102 mL of a working standard that has a concentration of 4.500 mg/L, what volume of the 1.000 Ă— 103 mg/L standard solution is needed? mL
Jennifer H.
You have 50 mg of medication in 500 mL of normal saline solution. What is the concentration, in milligrams per milliliter, of the solution? (Calculate to the tenth place.) You have 1 g of a medication in 500 mL of normal saline solution. What is the concentration, in micrograms per milliliter, of the solution?
Kameswara Ramakrishna A.
Recommended Textbooks
Biology for AP Courses
Objective Biology for NEET
Introduction to General, Organic and Biochemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD