1. Preparation of the Sodium Thiosulfate secondary standard solution
Given 1M Sodium Thiosulfate
You should dilute the sodium thiosulfate solution to approximately 0.05M. Plan on making about 200mL of this solution.
1. Preparation of the Sodium Thiosulfate secondary standard solution Given 1M Sodium Thiosulfate You should dilute...
If you have a 1M stock solution and you want to dilute 1 :10 with water, how many mL of your stock are needed and how many mL of water, if you are making 100mL, 250mL and 500mL
Suppose you need to standardize a sodium thiosulfate solution for a titration experiment. To do so, you will react it with a solution of iodine. You add a 1.00 mL aliquot of 0.0200 M KIO3 solution to a flask, followed by 3 mL of distilled water, 0.2 g of solid KI, and 1 mL H2SO4. You then titrate the solution with sodium thiosulfate solution in order to determine the exact concentration of Na2S2O3. The end point of the titration is...
1. Given powdered sodium sulfate, how will you prepare 100mL of a 1M solution of sodium sulfate? Your solvent is 0.1M acetate Buffer. 2. Given a 1M solution of sodium chloride, how will you prepare 1000uL of 0.2M solution of sodium chloride. 3. Given a 100 mg/mL protein solution, how will you prepare 20uL of a 70 mg/mL protein solution? 4. What is lysozyme and where are they usually found? 5. What is the role of X-crystallography in structure identification?
You are given powdered sodium sulfate, how will you prepare 100 mL of a 1M solution of sodium sulfate? Your solvent is 0.1 M acetate buffer.
You are given sodium acetate, 1M HCl, NaHCO3, and Na2CO3. Determine which of these four would you need and then show calculations to make buffer pH=4.7 by the following: Strong Acid & Weak Base (mol/L)(g/mol)(L) = Weak Base Strong Acid: C1V1=C2V2 Assume making 100mL of a 0.1M buffer.
1. You are given 15 ml of a 45% solution and told to add (not dilute to) 175 ml. What will the final strength of the diluted solution be? 2. You need to make a 10% solution using 4 ml of a 70% stock solution. How much sterile saline do you need to add to make this product? 3. You are given 5 ml of a 65% solution. If you dilute the solution to make a 15% solution, what is...
Given this scenario: 1) If you dilute a solution by pipetting 10 mL of a pink solution into a 50 mL volumetric flask and you blow out the last drop from the pipet, then you dilute the solution until you reach the . 50 mL mark in the volumetric flask with water and mix it. The measured value for the absorbance should be _______ than the correct value? a) greater b) less c) equal to 2) If you prepare a...
Please answer pre lab question 4. Thank you!
3. Dilute the 0.1 g/L quinine standard solution by a factor of 10 in a 250.00 mL volumetric flask. Dilute to the mark with 0.05 M H2SOs, mix well. Calculate the concentration of this solution in mg/mL PrelabQuestion #4: What volume of the 0.1 g/L standard should you use? Show all work type of glassware should you measure this volume with?
To what volume should you dilute 133 mL of an 7.90 molL−1 CuCl2 solution so that 52.0 mL of the diluted solution contains 4.88 g CuCl2?
Calculate the concentration of the standard HCl solution you
prepared. Determine this
concentration for each trial and the average and standard
deviation for all three trials.
Part B-Preparation and standardization of an HCl Solution 1. Before you can titrate your saturated Ca(oH)a solutions, you must prepare and standardize a dilute solution of Hcl. With a graduated cylinder measure at least 6 mL of the stock Hcl lution, transfer it to a 125 mL Erlenmeyer, and dilute to approximately 100 mL...