Part A: The standardized HCl solution being used is 0.198 M. Trial 1: Using a volumetric pipette, you pipet exactly 20.00mL of the standardized HCl solution into a 250-mL Erlenmeyer flask. You then add 2-3 drops of phenolphthalein. Trial 2: Using a volumetric pipette, you pipet exactly 10.00mL of the standardized HCl solution into

Part A: The standardized HCl solution being used is 0.198 M. Trial 1: Using a volumetric pipette, you pipet exactly 20.00mL of the standardized HCl solution into a 250-mL Erlenmeyer flask. You then add 2-3 drops of phenolphthalein. Trial 2: Using a volumetric pipette, you pipet exactly 10.00mL of the standardized HCl solution into

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.108E

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H2. How would you prepare 100 mL of a 0.05 M aqueous solution of iron from a 0.7 M solution? It includes a flow diagram of all the steps, the volumetric materials to be used, it includes the disposal of waste (after having used the solution for a colorimetric analysis). Step 1. Take aliquot of: ____ ml Express your result with a decimal and without units.
CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) A laboratory is well-stocked with 1.0 M H2SO4 and 6.0 M H2SO4, but 500 mL of 2.5 M H2SO4 areneeded for an experiment. Unfortunately, the water supply has been temporarily cut off, so the 2.5M solution must be made from the existing solutions. How many milliliters of 1.0 M and 6.0 MH2SO4 must be mixed in order to prepare 500 mL of 2.5 M solution?
A student made 10.0 mL of a 0.750 M solution in the following way. First, the student took some 16.0 M aqueous stock solution and diluted it in a 200.0 mL volumetric flask with deionized water. Secondly, the student took 5.00 mL of this diluted solution, and further diluted it to 10.0 mL in a test tube. In order to make the final 10.0 mL solution, how much stock solution did the student need to add into the 200.0 mL volumetric flask? a) 33.0mL b) 5.00mL c) 46.9mL d) not enough information is provided e) 18.8mL
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).
A student used a pipette to place 25.00 mL of HCl into an Erlenmeyer flask. Then the student diluted the acid with distilled water and added a few drops of phenolphthalein to the flask. The sample was titrated with a sodium hydroxide solution until a faint pink color became permanent. The procedure was repeated 4 more times. The following results were obtained: Volumes of NaOH used for each trial: Trial 1 37.22 mL Trial 2 36.14 mL Trial 3 36.13 mL Trial 4 36.15 mL Trial 5 36.12 mL Which of the following is the most probable explanation for the variation in the student's results for Trial 1? A. Water in the pipette B. Water in the burette C. Water in the flask D. Misread a 7 for a 6 on the burette.
Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake.A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant.1. What is the concentration of hydroxide ions in the solution? Note: Use the scientific notation of 0.00012 = 1.2e-4 2. Determine s and Ksp of Mg(OH)2.Note: Use the scientific notation of 0.00012 = 1.2e-4
Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake. A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant. What is the concentration of hydroxide ions in the solution? Determine solubility s.
Show your complete solution and round-off your answers to four decimal places. A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 N AgNO3, the sample was back titrated with 0.05781 N KSCN, requiring 27.36 mL to reach the end point. Calculate the % purity of the Na2CO3 sample. Answer = _% Na2CO3
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1531 M0.1531 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 16.75 mL16.75 mL of the standard solution. What is the concentration of the original sulfuric acid solution?
A student begins a titration experiment by filling her first buret with unknown acid to the 1.12 mL level. She fills her second buret with base, NaOH, and records an initial volume of 0.08 mL. At the end of the titration experiment and after the pale pink endpoint is obtained, she records her final volume of acid in the buret as 18.85 mL, and the final volume of base in the second buret as 28.74 mL. In the first blank below, please indicate the volume of acid used in her experiment. In the second blank, please indicate the volume of base used. For both answers, please report your answer WITH the correct number of significant figures or decimal places, and WITHOUT a unit. Question 1 options: ___________ answer #1 ___________answer #2
A solution is prepared by pipetting 25.00 mL of 3.0 x 10-4 M CaCl2 into a 750.00 mL volumetric flask and then adding water to the calibration mark. What is the concentration?
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1463 M0.1463 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 18.47 mL18.47 mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration: ___________M