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

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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Consider a 1.000-L stock solution of 9.69 M Na3PO4. A 2.000-mL aliquot is taken from this stock solution and diluted to a final volume of 1.000 L. A 5.000-mL aliquot is then taken from this new solution and further diluted to make a new solution with a final volume of 750.0 mL. Calculate Na+ in the final solution.
Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
Chemistry A group of students was tasked with synthesizing dibenzalacetone (DBA) in the lab. They used acetone as limiting reagent, calculated their TY to be 8.0 g DBA, obtained 14.0 g crude product (wet) and their % Yield was 65%. What was the actual yield for their final product (recrystallized, dry DBA)? What was the minimum volume (ml) of ethanol they needed to recrystallize their wet crude? What was the amount of impurities (side products, moisture,...) contained in their wet crude?
If a solution is made by adding 8g of (NH4)2SO4 to a 100 ml volumteric flask and enough water is added to bring the total volume to 100ml, what would the density of the solution be? This is a straightforward question but I just wanted some clarification. When we bring the total volume to 100ml, does that mean we added 100ml of water? Will the mass of the water be 100 g regardless of the amount of solute added?
(A) if both sentences are true,(B) if both sentences are false,(C) if the first sentence is true but the second is false, and(D) if the first sentence is false but the second is true. 1. In the Winkler Titration Method, sodium thiosulfate is standardized against a known concentration of magnesium iodate. The normality (N) of a solution is always equal to its molarity (M). 2. In the experiment on determining the dissolved oxygen concentration of a water sample, the compound used to acidify the sample was hydrochloric acid. An acidic solution will have a pH greater than 7. 3. Radioactive wastes, like uranium, must be handled and disposed of according to special regulations designed to protect people and the environment. Nuclear power plants produce too much greenhouse gases due to the burning of uranium.
In this station, you will find a sample of table salt; the chemical formula of table salt is NaCl. Using the balance, weigh out 6.00 g of NaCl and dissolve in 50 mL of deionized (d.i.) water. Once com-pletely dissolved, add additional d.i. water to make the final volume of solution 100.0 mL. What is the mass percent NaCl in the solution? What is the molarity of the solution
I need to make a solution containing 0.025 grams per liter. However, I do not want to weigh 0.025 grams and put this in one liter of solvent. I want to make a stock solution of 0.25 grams in 500 ml of solvent and take a unknown aliquot and dilute this in 500ml of solvent instead of 1000 ml of solvent. How do I calculate the volume of aliquot from the stock solution to achieve a final concentation of 0.025 grams per liter? What is the proper equation(s) required to figure out the proper aliquots required?
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)
You have been tasked with determining the wastewater solids generated by a community. To determine solids, you collect two effluent samples of 100 mL each. The first sample was placed, unfiltered, in a crucible and dried at 105 ̊C overnight. The weight of the dried sample and crucible was 5.6112 g, while the weight of the crucible was 5.6000 g. The second sample was filtered. The filter and drying dish were dried overnight at 105 ̊C after which they weighed 2.1085 g. The filter and drying dish were then placed in a muffle furnace at 550 ̊C for 30 mins, after which they weighed 2.103 g. The drying dish weighs 1.6000 g and the filter weighs 0.5 g. a) Determine the concentration of TS, TSS, VSS, FSS and TDS in mg/L: b) Does TSS concentration meet the federal effluent regulations? If not, what removal techniques would you recommend and what minimum percent must be removed prior to discharge?
Five standard solutions of HBr are prepared by serial dilution in which, at each stage, 10.00 mL are diluted to 120.00 mL. Given that the concentration of the most dilute solution is 3.52 × 10−6 M, determine the concentration of the original HBr stock solution.
BSA for concentration measurements is often prepared as a 10 mg/mL stock solution. Suppose you wish to prepare a series of 10 mL solutions of BSA at 1.0, 0.8, 0.6, 0.4, and 0.2 mg/mL. Using the dilution equation C1 × V1 = C2 × V2, you plan to do this by transferring a calculated volume (V1) of the 10 mg/mL (C1) into a clean test tube, then adding water in sufficient volume to produce 10 mL (V2) at the desired concentration (C2). Complete the table below, showing the volume of stock 10 mg/mL solution you need to add to each tube, and the volume of water you need to add to each. Also, convert the desired mg/mL concentration values to their equivalent in μM (micromolar; 10-6 M).
1) How much total glucose is present in a 75 Kg female person? (a normal person (70 kg BW) has approximately 43L body fluid).2) Please express the normal salt (NaCl) concentration in body fluid into molarity (mM).3) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9% solution. Please convert it into molarity.4) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.5) The above reaction has the product Ammonia, which when dissolved in 650 mL ethanol makes an alkaline ethanolic solution. Find its molarity (M).6) Calculate the adult dose as per the BW of the baby. (Child dose-50 mg and the BW of the baby is 48 lb (British pound) (1lb=0.453 Kg)