Pre-lab exercise 1) The table below from Part 1 illustrates the dilution processes required for creating the dilute standard solutions. Given that the stock solution was made from 0.050 g quercetin in a 250 mL volumetric flask, calculate the quercetin concentration in the initial stock solution and show your working below on how the dilution processes below resulted in the stated quercetin concentrations ranging from 4-32 mg/L. Concentration of quercetin (mg/L) 0 (blank) 4 8 16 24 32 Dilution with deionised water Pure deionised water 1 mL of stock solution to 50 mL 2 mL of stock solution to 50 mL 4 mL of stock solution to 50 mL 6 mL of stock solution to 50 mL 8 mL of stock solution to 50 mL
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- 1. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1500 M CaCh2 Solve for the concentration of the stock solution in M. 2. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1200 g CaCl2 Solve for %w/v CaCl2 in the stock solution.Chromatography: Evaluating Pen Inks PreLab Questions Name Section 1. Observe the following picture of several known indicator dye solutes spotted on the stationary phase, phenol red, bromocresol purple and bromothymol blue respectively. Which solute spot would most likely cause problems with the chromatography process and why? Explain. Treral Bed Erom Cresol Parpie Gromm BlueStandardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…
- "Solution 1" is made from the addition of water to a portion of the 0.0500 M Fe3+ " prototype" solution. Water is added to "prototype" as stated in the "dilution one" lab step to create a more dilute Fe3+ solution called "Solution 1". If you follow the lab procedure in the dilution one lab step, what will be the resultant molarity of Fe3+ in "Solution 1"?Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…A 0.1 g amine-containing compound is dissolved in water then diluted to 100 mL. You subject it to spectroscopic analysis, in order to get the concentration of amine in this compound. Next, you get 1 mL of the previously diluted sample then dilute it again to 250 mL for measurement. Then, you fill 3/4 of a 1-cm cuvette with this diluted sample, and you run an analysis using an AAS. The recorded absorbance is 0.545 at 410 nm. What is the molecular weight of the compound? (The molar absorptivity is 1.23 x 104 cm-1 mol-1 L.)
- Part 1: Preparation of the Primary Citric Acid Standard 1. Mass of Citric Acid: 4.05 g 2. Volume of Citric Acid Solution: 0.75 ml (at the equivalence point) 3. Moles of Citric Acid: (Molar Mass = 192.0 g/mol) 4. Molarity of Citric Acid Solution: Part 2: Titration of the Sodium Hydroxide Solution (Show your work on page 4) 1. Volume of Citric Acid at the Equivalence Point 2. Moles of Citric Acid at the Equivalence Point: 3. Moles of NaOH at the Equivalence Point 3 NaOH + H.CaHsO, → Na:CH.O, + 3 H,O 4. Volume of NaOH 10.0 mL 5. Calculated Molarity of NaOH: Do not use the dilution equation to calculate the molarity of the sodium hydroxide. The dilution equation cannot be used when a reaction is occurringProcedure A: Molarity (M=g/MM/L) Step 1. Place one-eighth of a teaspoon (this weighs approximately 0.5 grams) of NaCl (table salt) in the graduated cylinder provided. Then add distilled water to that graduated cylinder until the level of the water reaches 45.00 mL. Mix thoroughly about 1 minute. Pour solution into a somewhat clear cup. Remember what this looks like for Procedure B. Questions: Is this a saturated solution? Why or why not? Take a picture and insert a picture (compress your image) of your solution here. Save this solution for Step 2. Calculations: Determine the Molarity of this solution using the formula M = g/MM/L. You know the grams (one-eighth of a teaspoon weighs approximately 0.5 grams), look up the Molar Mass of NaCl, and convert your mL to L to solve the problem.) Show your calculations for Molarity here. C % 31 D < hp & * ✔Help me please
- Describe how you would make 1L of the following solution using the stocks given below. Please include how much of each stock you will use, as well as how much water you will add to the solution at the end. Stocks: Acrylamide powder Desired final solution:15% acrylamide (w/v)1. a) "Solution 1" is made from the addition of water to a portion of the 0.0500 M Fe3+ " prototype" solution. Water is added to "prototype" as stated in the "dilution one" lab step to create a more dilute Fe3+ solution called "Solution 1". If you follow the lab procedure in the dilution one lab step, what will be the resultant molarity of Fe3+ in "Solution 1"? b) The Fe3+ "Solution 2" is made by using water to dilute the Fe3+ "Solution 1". Using the dilution scheme described in your lab manual as "Dilution 2" to calculate the new, even more dilute, Fe3+ level in "Solution 2". Remember to use the molarity for the Fe3+ in " Solution 1 as your initial molarity for this calculation (see your value from question above). c) The Fe3+ "Solution 3" is made by using water to dilute the Fe3+ "Solution 2". Using the dilution scheme described in your lab manual as "Dilution 3" to calculate the new, even more dilute, Fe3+ level in "Solution 3". Remember to use the molarity for the Fe3+ in…Enter your answer in the provided box. A volume of 36.2 mL of a 0.568 M Ca(NO3)2 solution is mixed with 75.5 mL of a 1.696 M Ca(NO3), solution. Calculate the concentration of the final solution. M Prev 39 of 45 Next > T:T.. 26°C M o search