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- This lab used 6 M HCl that was diluted from a higher concentration. If your lab instructor asked you to make a solution of HCl with a concentration of 2.0 M from 50.0 mL of a 10.0 M stock solution of HCl, to what total volume would you have to dilute the portion of stock solution? Units as mL.A 480-pound alloy (which is just a mixture of metals ) containing 30% silver was mixed with an alloy containing 55% silver to get an alloy containing 40% silver. How many pounds of the 55% alloy were used?Your 50 mL beaker has a mass of 6.65 g. You add 10.00 mL to the 50 mL beaker and now the total mass is 17.45 g. You originally used 5.14 g of NaCl to make the solution. What is the percent composition of your solution? These calculations are described in the lab procedure in detail.
- 1. A solution is prepared by taking a clean and dry 50.0 ml volumetric flask. You are tasked to prepare a saline solution with your table salt placed in a watch glass. You measured the following in the laboratory. 147 g Mass of volumetric flask Mass of watch glass glass + salt Mass of watch glass after adding salt to the volumetric flask 30.0 g 23.5 g Some water is added to the flask. The solution is stirred until all salt is dissolved. The filled flask of the saline solution is then weighed again. Mass of filled flask 202 g What are the mole fractions of sodium chloride and water?Percent by Mass= Mass of Solute x100 Percent by volume and Percent by Mass calculations Mass of Solution Volume of Solute Name: Percent by Volume= -x100 Volume of Solution 1. 1. Calculate the percent by volume if 56.7 ml of alcohol is added to 540 ml of water. (Remember to add both solute and solvent to get the total volume of solution to put on the bottom.) 540 15.23 2 Calculate the percent by mass if 35.0 grams of NaC! is added to 455 grams of water to make a salt solution. 3. Calculate the percent by volume if 15.5 ml of HCI is added to 1.0 Liter of water. 4. Calculate the amount of water needed to make a 5% solution of alcohol, if you have 25 ml of alcohol? (Hint: first you will need to find the total amount of solution needed. then subtract the 25 ml from that.)When 50. mL of 5.4 M NaCl is diluted to a final volume of 300. mL, what is the concentration (M) of NaCl in the diluted solution? Report your numeric answer only and to the correct number of significant figures.
- Use the lab introduction to answer the following question. When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A beverage drink mix sample is prepared by mixing a packet of beverage powder in a gallon (3.78 L) of water. A sample for analysis is prepared by diluting 10.00 mL of this solution in a 50.0 mL volumetric flask. When measured using a colorimeter, this diluted solution has an absorbance of (3.4900x10^-1). The calibration curve for the experiment yielded a linear fit of y = (2.240x10^4)x+ (1.22x10^-2) and an R2 value of 0.9911. Determine the molar concentration of food dye in the analyzed sample.Solution 1 is diluted by combining 6 mL of Solution 1 with 64 mL of Solution 2. What is the dilution of solution 1? Report your answer in standard decimal notation rounded to two decimal places. For example, 4 mL added to 16 mL would be a 0.20 dilution. Include trailing zeros if necessary so your answer has two decimal places.How much water, in mL, needs to be added to 29.7 mL of 11.2 M HNO3 to make a 6.05 M solution with the same amount of moles of HNO3? Record 3 significant digits in your answer. Don't type units in. Round your answer to 3 significant figures.
- A chemist prepares a solution of calcium bromide (CaBr,) by measuring out 84.7 g of calcium bromide into a 150. mL volumetric flask and filling the mark with water. Calculate the concentration in mol/L of the chemist's calcium bromide solution. Round your answer to 3 significant digits. | molL ContinueA chemist prepares a solution of zinc nitrate mark with water. (Zn(NO3)2) by measuring out 22.6 g of zinc nitrate into a 200. mL volumetric flask and filling the flask to the Calculate the concentration in mol/L of the chemist's zinc nitrate solution. Round your answer to 3 significant digits. mol/L xA volume of 25.00 mL of the original solution was diluted to a total volume of 100.0 mL and then 10.00 mL of that diluted solution was diluted to a total volume of 15.00 mL to make the sample for analysis. If a student in lab found that the solution for spectroscopic analysis had a concentration of (4.0x10^-5) M, what was the concentration of the original solution, in units of M?