2. Experiment: UV-vis experiment was done to determine the unknown concentration of an organic compound solution. First, a stock solution of a Compound A (Molar Mass 893.5 g/mol) was prepared by dissolving 0.500 g of Compound A in 250.0 mL of water. a) Calculate the molar concentration of this stock solution. Show your calculation here. b) Calculate the concentration of each of the standard solutions and complete the table below. Discuss these results on your report. Volume of Standard Concentration of Standard (M) Standard Absorbance Initial Volume of Stock used (mL) 0.00 Solution # prepared (mL) 25.00 0.00 0.000

2. Experiment: UV-vis experiment was done to determine the unknown concentration of an organic compound solution. First, a stock solution of a Compound A (Molar Mass 893.5 g/mol) was prepared by dissolving 0.500 g of Compound A in 250.0 mL of water. a) Calculate the molar concentration of this stock solution. Show your calculation here. b) Calculate the concentration of each of the standard solutions and complete the table below. Discuss these results on your report. Volume of Standard Concentration of Standard (M) Standard Absorbance Initial Volume of Stock used (mL) 0.00 Solution # prepared (mL) 25.00 0.00 0.000

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.6QAP

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Submit a clean, dry, and properly labeled 50-mL reagent bottle for your unknown solution. Pipet 20.00 mL of the sample in 250-mL Erlenmeyer flask. Add 5 mL of buffer and 5 drops of indicator. Titrate the solution until it turns light blue. If the titration consumes more than 50 mL of the titrant, dilute the sample accordingly. Compute for ppm of CaCO3 using the following table. Mean Molarity = 2.487 x 10^-3 MBlank correction = 0.015 Formula = V (mL) titrant x Mean Molarity of Titrant x Molecular weight of CaCO3 x 1/V (L) sample
Based first from the first photo (table 3-2). Answer A (3 only) answer B (1,2,3)thanks with complete solutions
2 Trial 1: [4] Volume of NaOH, dispensed (mL) Trial 1: [5] Molar concentration of NaOH (mol/L) Trial 2: [4] Volume of NaOH, dispensed (mL) How Trial 2: [5] Molar concentration of NaOH (mol/L) Trial 3: [4] Volume of NaOH, dispensed (mL) Trial 3: [5] Molar concentration of NaOH (mol/L)
Draw and upload here as an attachment a molecular-level representation of ammonium chloride (NH4Cl) before the dissolution process occurs. Include a key to differentiate the ammonium cation (NH4*) and the chloride anion (Cl- ). (Remember, no .heic files!) Describe what forces are holding the particles in NH4Cl together.
Part Il: Determination of Standard Solutions mL of 0.200 mL H20 added M Cuso, diluted Tube # M Cuso4-5 H20 added Absorbance about 3 0.200 1.346 3. 4.00 1.00 0.945 4 3.00 2.00 0.715 2.00 3.00 0.469 6. 1.00 4.00 0.281 show calculation for Tube #3 diluted concentration:
Along with the drawing of the solution, please explain the solution as well. I am really suck on this one.
1. A 0.1250-g sample of pure (100%) of K2Cr2O7 was dissolve in 250-mL volumetric flask, and dilute to volume, producing a concentration of 1.700 × 10-3 M. The resulting solution is an example of a standard solution prepared from a primary standard. Select one: a. True b. False 2. Which of the following is not an example of a standard solution? a. 1000 ppm Lead Nitrate solution b. 1.000g pure sodium carbonate dissolved in 1L of solution c. 3:4 nitric acid: hydrochloric acid solution d. NaOH solution standardized using KHP e. 0.104 M NaOH
Assume you have 0.1 M NaOH Trial 1: 22.5 mL NaOH Trial 2: 25.6 mL NaOH Trial 3: 24.4 mL NaOH
Determination of unknown acid concentration Trial 1 Trial 2 Trial 3 Unknown Acid number Volume of acid used (mL) 25 mL 25 mL 25 mL Initial buret reading (mL) 50 mL 50 mL 50 mL Final buret reading (mL) 14.8 mL 15 mL 14.5 mL Volume of NaOH used (mL) 50 mL 50 mL 50 mL Molarity of NaOH Calculated molarity of HCl (M) Show a sample calculation of HCl molarity AVERAGE MOLARITY OF Unknown HCl Show a sample calculation of NaOH molarity
A. Standardlzatlon of thlosulfate solutlon Trial 1 Trial 2 Trial 3 Initial volume of thiosulfate (mL) 0.00 20.05 2.3 Final volume of thiosulfate (mL) 20.05 40.05 22.15 Volume of thiosulfate used (mL) Molarity of thiosulfate Average Molarity of thiosulfate Calculate the molarity of the thiosulfate solution using the formula: 6 mmol S20,²- 1 mmol 10, Ms,0,2- 0.004167 M 10,- 20.00 ml Vol S20,²- used (mL)
1. Prepare 50-mL of a 50 mM H,PO, solution in a 50-ml conical tube. Molar mass of NaH2PO4 H2O used is 138 moles 2. Check the pH of this solution and record. 3. A5 M NAOH solution has been provided. 4. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. 5. Add 205 µl of 5M NaOH into the 50 mM H2PO4 solution. Check the pH and record. 6. Add 205 µL more of 5M NaOH into the 50 mM H2PO, solution. Check the pH and record. 7. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. Complete the following table "predicted pH." Please show all work on a separate sheet of paper and attach. Note that the pK, of H2PO, is 7.2. What would be the predicted pH's? Would they be similar to the actual pH's from procedure? After 45 µl of 5 | After 205 µl more of 5M NaOH Original After 205 µl more After 45 µl more solution M NaOH of 5M NaOH of 5 M NaOH Actual pH 4.30 6.05 6.90 11.01 11.29 Predicted pH
A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500. mL of solution. What is the bromide ion concentration in this solution? 20 Multiple Cholce X 0206:02 9.19 x 10-3 M 230 x 10-2 M 272 x 10-3 M 1.84 x 10-2 M 1.25 x 10-1 M Mc Graw Hill Type here to search 近 C