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Atomic weights are not provided, but please use rounded-off values to the nearest whole number.
(examples: 24.305, use "24"; 107.8682, use "108"; 1.00784, use "1"; 15.999, use "16")
Final answer in 3 decimal places
1. A fat sample with combination free fatty acids required 8mL and 5mL of standard hydrochloric acid for blank and sample titration, respectively. The normality of the standard hydrochloric acid is 0.93N and the weight of the sample is 3 grams. Calculate the saponification value.
2. A 500mg oil sample is taken from a conical flask and is dissolved in 50mL distilled alcohol. An indicator is added and is then titrated against 0.112N KOH until a slight pink color appears. It took 17.6mL of the titrant to reach the endpoint. What is the sample’s Acid Value?
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- 0.1890 grams of an unknown organic acid containing 2 carboxylic groups was dissolved in about 50 mL of water in a 250 mL Erlenmeyer flask and titrated against 0.1000 M NaOH solution using bromothymol blue indicator. 34.62 mL of titrant was used to achieve end point. Calculate the molar mass of the unknown. Write answer with two decimal places only. No units please.Table of chemicals and reagents with their physicochemical properties (name, molecular formula, molecular weight, pKa, melting point, boiling point, etc.) Write a short outline or a flow diagram of the procedure List and safety issues Read and understand the MSDS information for each chemical used in this practical Experimental procedure Please do not scratch the clear sides of the UV cuvettes as this will invalidate your results. Part 1: Preparation of a calibration curve A calibration curve should be constructed using at least five concentrations of the pure paracetamol standard supplied in the range 3-15 ug/mL as follows: Weigh about 150 mg of paracetamol accurately and transfer to a 200 mL volumetric flask. Add 50 mL of o.1 M NaOH and dilute to about 100 mL with deionised water (DI). Shake and make up to volume with DI water. Dilute 10 mL of the resulting solution to 100 mL (volumetric flask) with DI water (= stock solution). Prepare standard solutions containing 3, 6, 9, 12 and 15…To which sample solution the spike will be add? the distillate>130C the mass standard the distilled <130C
- Please don't provide hnad writtin solution.... I need explation solution and step solution...Q3/ A) 0.63 g of a sample containing Na CO,, NaHCO; and inert impurities is titrated with 0.2 M HCI, requiring 17.2 ml. to reach the phenolphthalein end point and a total of 43.5 mL to reach the modified methyl orange end point, How many grams Na CO, and NaHCO, are in the mixture?Answer the following: Maria was given a capsule of multivitamins and she was asked to determine the % by mass (w/w) of ascorbic acid present in the sample. The student analyzed 1.032 g sample using volumetric titration. Use the table as a reference of the data to be used for your solution. Given Choices: A. 66.0 % B. 54.6% C. 65.6% D. 7.30%
- what are possible sources of error in a soap making experiment? (non-human error) I want clear handwritten solution only....i will up voteSubmit 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) sampleStandardization 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.…
- 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.…Topic: Standardization of acid and base with back titration Note: Include up to 4 decimal places Kindly explain the process Thank you!Please don't provide hand writtin solution..... I need explation and step solution.....