Different masses of aspirin (e.g 10mg, 100mg, 1000mg) used in an acid base titration. what could be the reason for the differences in percentage purity?
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- In the procedure below for a weak diprotic acid titation experiment what are the independent, dependent, and controlled variables? Prepare your Buret• Condition a 50 mL buret (2x with DI H2O followed by 2x standardized NaOH)• Fill the buret with the standardized NaOH close to but not exactly 0.00 mL Prepare Your Analyte • Your analyte will need to be placed in a 250 mL beaker and should contain thefollowing:*0.5 – 0.75 g KHP** About 100 mL DI water* Magnetic stir bar• Once all contents are in the 250 mL beaker, stir for at least 5 minutes to dissolve. Ifneeded, add a bit more water.* For unknown diprotic acids, use the mass provided by the instructorNext Run the Titration (note you will need to run the titration several times for data collection so you are able to use the average molar mass to find the unknown diaprotic acid).In RPLC, The retention of a basic analyte in RPLC decreases as the mobile phase pH increases. True or False?The retention of a carboxylic acid analyte in HILIC will decrease as the pH of the buffer component of the mobile phase is increased, true or false?
- At any stage of the saponification experiment of ethyl acetate, when the 25mL sample taken from the mixture is taken into a flask containing 0.05M 15mL HCl and titrated with 0.05M NaOH, if the consumption is 10mL, calculate the remaining NaOH concentration without reacting over the reactions.If the test tube used in the determination of the ΔHrxn for nitric acid (neutralization with NaOH) was still wet with water, will the magnitude of ΔHrxn increase, decrease, or remain the same?Please explain.Suppose your colleague was relying on receiving your purified product in order to prepare a dilute aqueous standard solution of benzoic acid e.g. for a titration. She takes 160 mg of your benzoic acid and dissolves it in just enough water so the solution exactly fills a 250 mL volumetric flask. Given that the acid dissociation constant of benzoic acid Ka = 6.3 x 10-5, calculate the pH of her resulting solution.
- how to find culculated ka and literature Ka for acetic acid?Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.What is a 3 point calibration in titration?
- Iodometric titration of vitamic C with sodium thiosulfate Why was the known excess of iodine generated using iodate rather than weighing out a known excess of iodine?What factor affects the ‘strength’ of a buffer? Why was benzoic acid used as a solvent when making up the glucose stock standard solution?In how much volume of diluted sulfuric acid should you dissolve a multivitamin tablet of approximately 1700 mg of Vitamin C to back analyze 10.00 mL of that solution, with 25.00 mL of 0.01 M KIO3 and 0.04 M thiosulfate to use approximately 8-10 mL of titrant ? You have 25, 50, 150, 250 and 500 mL flasks.