cedstock. To begin, you’ll make 20 mL of a 10% solution of your assigned fuel. a. How many grams of fuel will you need to make your solution? Hint: The definition of a 10% solution is 10 grams of solute (fuel in this case) in 100 mL of solution. b. You will then pour 10 mL of your 10% solution into an empty beaker. How much water (in mL) should you add to the beaker to create a 5% solution? Hint: Assume all of your

cedstock. To begin, you’ll make 20 mL of a 10% solution of your assigned fuel. a. How many grams of fuel will you need to make your solution? Hint: The definition of a 10% solution is 10 grams of solute (fuel in this case) in 100 mL of solution. b. You will then pour 10 mL of your 10% solution into an empty beaker. How much water (in mL) should you add to the beaker to create a 5% solution? Hint: Assume all of your

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 120QRT

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2. Use the formula listed below to calculate how much of each ingredient should be used to make 20,000 ml of Chigger Dope that is used to treat chigger insect bites. Add your solution below the table. Original Conversion New Orange Syrup Formula Factor Formula Benzocaine 400g Methyl Salicylate 160mL Salicylic acid 40g Isopropyl Alcohol NF, 99% 5840mL Pure water qs ad 8000mL Solution:
3A. Determine the Molarity of the Sodium ion in a solution of Na2SO4.10H20 if you add 3.041 grams to a final volume of 150 ml. Add 3.041 g of Na2SO4.10H20 in a beaker pour upto 150ml of water to achieve 0.063 Molar. Calculation Na2SO4.10H20 MW = 322.03g/mol Grams = 3.041 g Vf = 150ml = 0.15L M= mols of solute/ L of solution (3.041g/1) (1mol/ 332.2g) = 0.00915mol Na2SO4.10H20 0.00915mol N22SO4.10H20/ .15l= 0.061 M 2 Na = 2*0.061mol/L = 0.126 mol/L Answer the question below Make a 1:100 solution of Na2SO4.10H20 in 100 ml of water from your previous solution. What is the final concentration of the Sodium lon?
Step 1: In tube 1, you add 100 ul of plasma to 900 ul of distilled water. Step 2: In tube 2, you then take 100 ul from tube 1 and add 900 ul of distilled water. Step 3: In tube 3, you then take 100 ul from tube 2 and add 900 ul of distilled water. What is the final/total dilution factor in tube 3 at the end of step 3?
Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices
You want to determine the concentration of NaCl in a water. In preliminary analysis, it appears to be saline water with a NaCl content of approximately 4%. Should you dilute the sample if your titrant has a concentration of 0.1 M and you want to spend 25 mL of sample? Solution: You must dilute approximately ten times, taking 10 mL of sample and making up to 100 mL. In this way, 17.20 mL of titrant will be spent.
. Prepare 50 mL of an aqueous solution of 2.5% (w/v) NaCl (sodium chloride, salt).Determine how many grams of sodium chloride are required. Show all steps for this calculation, using dimensional analysis with units clearly identified.2. Prepare this aqueous solution, using a volumetric flask for the precise final volume measurement. It is not a problem to use tap water.3. Clearly write the procedure (step by step) for making this solution
you can only work on it for 90 mins Instructions Multiple Attempts Not allowed. This test can only be taken once. Force Completion This test can be saved and resumed later. Your answers are saved automatically. * Question Completion Status: A Moving to another question will save this response. Question 28 10 Calculate the molarity of the resulting solution prepared by diluting 25.0 mL of 18.0% ammonium chloride, NH 4CI, (density = 1.05 g/mL) to a final volume of 80.0 mL. O a. 0.0536M O b.0.00105 M OC. 1.10 M O d.0.059 M O e.0.292 M » A Moving to another question will save this response. acer
2. You desire a sweeter tasting Kool-Aid. You've already saturated the Kool-Aid with sugar. In order to make it sweeter, you need to increase the solubility of the sugar in the water. You can do this by a. cooling down the water b. heating the water c. stirring the sugar and water more vigorously d. grinding the sugar into a fine powder so more will dissolve
A. Calculate the concentration of sugar in this solution using the volume percent equation. For the purpose of this exercise, it can be assumed that the weight of the drink mix is 0.00 g. The volume of the solution is 3 and 1/3 cups. Calculate and record the volume percent (g/mL). (Note that 1 cup = 236 mL). Volume %=Volume of Solute / Volume of Solution ×100% I used 1/2 cup of granulated sugar and 1/2 tsp of the drink mix, and 3 cups of water. B. Calculate the concentration of each diluted solution using the equation below and the volumes in Table. C1V1=C2V2 Where: C1=concentration of stock solution V1=volume of stock solution C2=concentration of diluted solution V2=volume of diluted solution (This is all the information that I have)
How do you prepare 200 ml 5% (w/v) CuCl2 mixture in water? Select one: a. Adding 190 ml ethanol to 200 mol volumetric flask and make up the volume with water b. Adding 10 gr ethanol to 200 ml volumetric flask and make up the volume with water C. Adding 10 ml ethanol and 190 ml water to volumetric flask d. Adding 10 ml ethanol to 200 ml volumetric flask and make up the volume with water
Page < 2 of 2 ZOOM + 8. Determine the final molarity for the following dilutions. a. 24.5 mL of 3.0 M solution diluted to 100.0 mL b. 15.3 mL of 4.22 M solution diluted to 1.00 L с. 1.45 mL of 0.034 M solution diluted to 10.0 mL d. 2.35 L of 12.5 M solution diluted to 100.0 L 9. Determine the initial volume (in mL) needed to generate each of the following desired solutions by dilution. а. 10.0 L of 0.45 M solution from 3.0 M solution b. 1.50 L of 1.00 M solution from 11.7 M solution с. 100.0 mL of 0.025 M solution from 1.15 M solution d. 50.0 mL of 3.3×10-4 M solution from 0.25 M solution 10. Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume of concentrated sulfuric acid required to prepare 2.50 L of 1.50 M H2SO4 solution.
1. Iron (Fe) nail + CuSO4 solution ? turned into the rusty Iron (Fe) nail turned into black substance of Carbon No reaction 2. CuSO4.5H2O is a _______________. anhydrous copper sulfate hydrated copper sulfate dehydrated salt