You want to make a solution of loading dye with a final concentration of 0.35% bromophenol blue, 0.15% xylene cyanol FF, and 0.25% glycerol in water. If bromophenol blue and xylene cyanol FF are powders and if glycerol comes in a 95% solution, how much of each reagent is needed to make 60 milliliters (ml) of loading dye? Include the amount of diluent in your final answer. Round answers to the correct number of significant figures. 0.35% Bromophenol Blue = 0.15% Xylene cyanole FF = 0.25% Glycerole = g ml Water = mL

You want to make a solution of loading dye with a final concentration of 0.35% bromophenol blue, 0.15% xylene cyanol FF, and 0.25% glycerol in water. If bromophenol blue and xylene cyanol FF are powders and if glycerol comes in a 95% solution, how much of each reagent is needed to make 60 milliliters (ml) of loading dye? Include the amount of diluent in your final answer. Round answers to the correct number of significant figures. 0.35% Bromophenol Blue = 0.15% Xylene cyanole FF = 0.25% Glycerole = g ml Water = mL

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...

See similar textbooks

Similar questions

The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
Chemistry Rx Cocaine HCl 1.5% (E = 0.16) Eucatropine HCl 1.5% (E = 0.18) Chlorobutanol 0.5% (E = 0.24) Make isotonic Disp: 30 mL a) How much sodium chloride should be added to make the above solution isotonic? b) If boric acid (E = 0.52) was used to make the solution isotonic how many grams should be used?
Preparation of a standard solution of copper(II) sulfate pentahydrate 1. Weigh out accurately 9.99 g of copper(II) sulfate pentahydrate (CuSO4·5H2O) by taring using a clean and dry empty 250-ml beaker. 2. Add tap water to the beaker to reach the 50-mL mark on the side of the beaker. 3. Dissolve all the crystals of CuSO4·5H2O in the water using a clean glass rod for stirring. 4. Then using a glass funnel transfer all the blue solution to a 100-mL volumetric flask. Rinse the beaker with about 10 mL of water and transfer the solution to the volumetric flask. Repeat the rinsing of the beaker with another 10 mL of water and transfer the solution to the volumetric flask. This is called quantitative transfer of the solution. 5. Then add enough water to reach the calibration mark of the volumetric flask. (You will need to use a dropper to add the last few drops of water to ensure the meniscus is on the calibration mark). Close the volumetric flask with a stopper and mix the solution well (so…
Indicate the appropriate protocol below to prepare the required solution. a) Solution 5 Preparation: Prepare: 10 mL of 23% mannitol From: solid mannitol Procedure: b) Solution 2 Preparation: Prepare: 0.5 liters of 0.01 mg/mL ascorbic acid From: solid ascorbic acid , MW = 176.1 g/mol Procedure: C) Solution 3 Preparation: Prepare: 1 liter of 150 mM Tris From: 1 Molar Tris stock solution Procedure:
Prepare 150 mL of a 3% agarose gel solution. Specify the following quantities necessary for this preparation: mL ddWater ___ mL 40x TAE ___ grams Agaros Gel ___
Emmett, a sophomore chemistry major, was trying to separate an unknown mixture. His instructor told him that there was a carboxylic acid, phenol, and amine present in the mixture. He dissolved 3 g of the unknown in 10 ml of t-butyl methyl ether. He then added 10 ml of 3M sodium hydroxide to the mixture. He used a separatory funnel to separate the layers and collected the aqueous layer in an Erlenmeyer flask labeled fraction 1. Then he added 10 ml of 1.5M sodium bicarbonate to the remaining ether. He separated the layers, and collected the aqueous layer in an Erlenmeyer flask labeled fraction 2. Finally he added 10 ml of 1.5 M hydrochloric acid to the ether, and separated the aqueous later in an Erlenmeyer flask labeled fraction 3. Emmett neutralized the respective fractions. He obtained precipitate in fraction 1, and fraction 3. He ran an IR of the solid obtained in fraction 1 and saw a broad absorption at 3500-3300 cm-1 and a sharp absorption at 1710 cm-1. Fraction 3 showed…
why would you add 10 mL of concentrate to 490 mL of water if you were instructed to dilute the concentrate 1:50 with water and you were was using a bottle with a 500 mL capacity
5.00 ml of the 1.0 x 10-4 M CV stock solution is first diluted to 100.ml. Then 1.00 ml pf this solution is diluted again to 50.0 ml. What is the final concentration?
Determine a procedure to accurately create a 1.5•10^-6 mg Fe/mL solution using a 0.0500 mg Fe/mL standard solution and only having access to 100.0 mL volumetric flasks and 1.00, 2.00, 3.00, 4.00, 5.00 and 10.00 mL volumetric pipets. (You may have it make more than one solution by dilution to accomplish this)
You have to make 50 mL of 0.05M HCl from a 10M HCl stock solution, but the only measuring devices available are 100mL graduated cylinders and 10mL serological pipets. How could you accurately make the dilute HCl solution (clearly explain)?
1. Which of the following is the best option for transferring 20 mL of a solution? a.Use a 5mL serological pipette 4 times b. Use a 10 mL Mohr pipette twice c. Use a 20 mL Mohr pipette once d. Use a 10 mL volumetric pipette twice 2. Which glassware is NOT used in preparing a solution from a solid sample? a. Funnelb. Beakerc. Volumetric pipette
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?