Following dilutions will give you 200
M solution:
1) Dilute the 5.00 mL of the stock solution up to 250.0 mL.
Then dilute 10.00mL of the resulting solution up to 500.0 mL.
2) Dilute the 5.00 mL of the stock solution upto 500.0 mL.
Then dilute the 10.00mL of the resulting solution upto 250.0 mL.
3) Dilute the 10.00mL of stock solution upto 1000.0 mL.
Then dilute 10.00 mL of the resulting solution upto 250.0 mL.
Following dilutions will not give you 200
M solution:
4) Dilute the 5.00 mL of stock solution upto 100.0 mL.
Then dilute 10.00 mL of the resulting solution upto 1000.0 mL.
5) Dilute 10.00 mL of the stock solution upto 100.0 mL.
Then dilute 5.00 mL of the resulting solution upto 1000.0 mL.
Attempt 1 Question 11 of 14 > You want to prepare a solution with a concentration...
The recommended procedure for preparing a very dilute solution is not to weigh out a very small mass or measure a very small volume of stock solution. Instead, it is done by a series of dilutions. A sample of 0.8521 g of KMnO4 was dissolved in water and made up to the volume in a 500.0−mL volumetric flask. A 2.000−mL sample of this solution was transferred to a 1000−mL volumetric flask and diluted to the mark with water. Next, 10.00...
Start with a 1230.0 ppm Stock Zn solution. Prepare control 1 by diluting 2.00 mL of Stock Zn solution in a 200.0 mL volumetric flask and dilute to the mark. Prepare control 2 by diluting 2.00 mL of control 1 into a 100.0 mL volumetric flask. What is the Zn concentration (ppm Zn) in control 2? Report your answer to 4 decimal place.
Does someone mind helping me with this question? I'd really
appreciate it.
Thank you!
1. Assume that you have 1, 2, 5, and 10 mL pipets and a 25 mL volumetric flask. Describe in detail how you would prepare a solution with a concentration near o.100 M from a 0.650 M stock solution. Calculate the final concentration of the diluted solution (t won't be exactly 0.100 M). It should be within 10% of 0.100 M. (Please see the Lab skills...
A chemist needs to create a series of standard Cu" (aq) solutions for an absorbance experiment. For the first standard, he uses a pipet to transfer 20.00 mL of a 2.52 M Cu" (aq) stock solution to a 500.0 mL volumetric flask, and he adds enough water to dilute to the mark. He then uses a second pipet to transfer 10.00 mL of the second solution to a 100.0 mL volumetric flask, and he adds enough water to dilute to...
Hello, in the book: Quantitative Chemical Analysis (9th Edition) Ch. 18 question number 24. All parts I need the steps/answers to check. Thanks. Preparing standards for a calibration curve. Part A) How much ferrous ammonium sulfate (Fe(NH4)2(SO4)2 * 6H2O, FM 392.15) should be dissolved in a 500-mL volumetric flask with 1M H2SO4 to obtain a stock solution with 1000 microgram Fe/mL? Part B) When making, stock solution (a), you weighed out 3.627g of reagent. What is the Fe concentration in...
8. Describe briefly how you would prepare, with a minimum number of dilutions, a 1x 10 Msolution of NaOH given the following: a 0.08 M stock solution of NaOH; 2, 5, 10 mL pipettes; 10, 20, 50, 100 mL volumetric flasks. (Show your working)
8. Describe briefly how you would prepare, with a minimum number of dilutions, a 1x 10 Msolution of NaOH given the following: a 0.08 M stock solution of NaOH; 2, 5, 10 mL pipettes; 10, 20,...
Question 11 4 pts You want to prepare a certain concentration of salt solution from 50.0mL of 9.00 M stock solution. Calculate the volume (ml) you need to prepare to prepare the following concentration. Salt solution that is 6.00M [Choose] < Salt solution that is 5.00M [Choose] < Salt solution that is 1.00 M < [Choose] Salt solution that is 0.750 M < [Choose]
help
Describe in detail how you would make a series of four standards ranging from 1 to 100 ppm given the following constraints. a. Your stock solution is 1000 ppm. b. The available pipets have volumes of 2.00 mL, 3.00 mL, and 5.00 mL. c. The available volumetric flasks have volumes of 10.00 mL, 25.00 mL, 50.00 mL, and 100.00 mL. d. You need to make at least 10.00 mL of each of your four standards.
Ferric Thiocyanate Standard Solution In Part A of this experiment you are instructed to prepare a solution as follows Pipette 10.00 mL of 0.150 M Fe3 solution, and 5.00 mL of 5.00x 10-4 M SCN solution in a 25.00 mL volumetric flask. Dilute to the mark with 0.100 M HNO3 and mix well. Calculate and enter the concentration of FeSCN2+ in this solution and, also, write it in your notebook. (It will be required for your Report sheet.) [FesCN2+1 6M...
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