assume you are preparing 25.00 mL of 0.0450 M CuCl2*2H2O solution by dissolving your calculate amount...
assume you are preparing 25.00 mL of 0.0450 M CuCl2*2H2O solution by dissolving your calculate amount of CuCl2*2H2O in a 25.00 mL volumetric flask. When you measure out the CuCl2*2H2O, you have 0.01 g of extra CuCl2*2H2O for your exact amount. Calculate the exact concentration of CuCl2*2H2O solution you prepared.
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assume you are preparing 25.00 mL of 0.0450 M CuCl2*2H2O
solution by dissolving your calculate amount...
1. Why would a chemist, when tasked with preparing a small volume of a dilute solution...
1. Why would a chemist, when tasked with preparing a small volume of a dilute solution use a dilution technique (i.e., prepare a dilute solution from a concentrated stock solution) rather than just weighing out the exact amount of solid material and dissolving it in the volumetric flask to make one solution only? 2. Calculate the number of grams of CuCl2.2H20 solid needed to prepare 25.00 mL of 0.0450 M CuCl2.2H2O solution. Show your work in the space below. 3....
A solution is made by dissolving 25.7 g of copper(II) chloride, CuCl2, in enough water to...
A solution is made by dissolving 25.7 g of copper(II) chloride, CuCl2, in enough water to make exactly 100 mL of solution. Calculate the concentration (molarity) of CuCl2 in mol/L (M). M CuCl2
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and...
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and a 25.00 mL aliquot of 0.150 M NH4Cl into a 100.00 mL volumetric flask and diluting to the mark. Using activities, calculate the pH of the buffer solution. Use the Davies equation to determine activity coefficients. (pKa of NH4+ = 9.245)
a.)Suppose you were preparing 1.0 L of a bleaching solution in a volumetric flask, and it...
a.)Suppose you were preparing 1.0 L of a bleaching solution in a volumetric flask, and it calls for 0.26 mol of NaOCl. If all you had available was a jug of bleach that contained 0.74 M NaOCl, what volume of bleach would you need to add to the volumetric flask before you added enough water to reach the 1.0 L line? Express the volume in milliliters to two significant figures b.) You need to prepare a 2.40 M solution of...
The recommended procedure for preparing a very dilute solution is not to weigh out a very...
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...
You have 659.3 mL of a stock solution 4.660 M HCl. For a particular experiment, your...
You have 659.3 mL of a stock solution 4.660 M HCl. For a particular experiment, your lab partner prepared a diluted solution for you to use. In her notes, you read: " Using a volumetric pipet, took 246.54 mL of stock solution and diluted it to 739.21 ml in a volumetric flask. Then, took 100.00 mL of that solution and diluted it to 194.63 mL in a second volumetric flask. " What is the concentration that you should report for...
As described in part A of the lab, you are preparing a solution by adding 2.00...
As described in part A of the lab, you are preparing a solution by adding 2.00 mL of 0.00200 M KSCN in HNO3 and 25.00 mL of 0.200 M Fe(NO3)3 in HNO3 into a clean, labeled 100.00 mL volumetric flask and diluting to the 100.00 mL mark with 0.25 M HNO3. Calculate the final concentration of KSCN in HNO3. 0.00200 M 0.000400 M 0.0000400 M 0.0000315 M 0.0500 M
(a) Potassium iodate solution was prepared by dissolving 1.022 g of KIO3 (FM 214.00) in a...
(a) Potassium iodate solution was prepared by dissolving 1.022 g of KIO3 (FM 214.00) in a 500 mL volumetric flask. Then 50.00 mL of the solution was pipetted into a flask and treated with excess KI (2 g) and acid (10 mL of 0.5 M H2SO4). How many millimoles of I3− are created by the reaction? ANSWER is 1.433 mmol (b) The triiodide from part (a) reacted with 37.54 mL of Na2S2O3 solution. What is the concentration of the Na2S2O3solution?
Calculate the concentration of a solution prepared by adding 15.00 mL of 1.98 × 10 −...
Calculate
the concentration of a solution prepared by adding 15.00 mL of 1.98
× 10 − 3 M K M n O 4 from a buret into a 50.00 mL volumetric flask,
which is then filled to the 50.00 mL graduation mark with distilled
water
1. Calculate the concentration of a solution prepared by adding 15.00 mL of 1.98 x 10-3M KMnO, from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation...
A 25.00-mL volume of commercial hydrogen peroxide solution was diluted to 250.0 mL in a volumetric...
A 25.00-mL volume of commercial hydrogen peroxide solution was diluted to 250.0 mL in a volumetric flask. Then 25.00 mL of the diluted solution were mixed with 200. mL of water and 20. mL of 3 M H2SO4 and titrated with 0.02177 M KMnO4. The first pink color was observed with 27.72 mL of titrant. A blank prepared from water in place of H2O2 required 0.07 mL to give visible pink color. Using the H2O2 reaction in the Analytical Applications...
1. Why would a chemist, when tasked with preparing a small volume of a dilute solution use a dilution technique (i.e., prepare a dilute solution from a concentrated stock solution) rather than just weighing out the exact amount of solid material and dissolving it in the volumetric flask to make one solution only? 2. Calculate the number of grams of CuCl2.2H20 solid needed to prepare 25.00 mL of 0.0450 M CuCl2.2H2O solution. Show your work in the space below. 3....
Calculate
the concentration of a solution prepared by adding 15.00 mL of 1.98
× 10 − 3 M K M n O 4 from a buret into a 50.00 mL volumetric flask,
which is then filled to the 50.00 mL graduation mark with distilled
water
1. Calculate the concentration of a solution prepared by adding 15.00 mL of 1.98 x 10-3M KMnO, from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation...
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