1. (a) What is the purpose of titration in volumetric analysis, and briefly explain how is it carriedout?(b) What is an indicator and why it is used in titrations?(c) What indicator will be used in this experiment and to which solution it is added?(d) In this experiment which solution is filled into the burette? Why must the burette be rinsedwith the solution before it is filled for the experiment?2. What is the purpose of the trial titration?3. Explain the purpose of washing the inside wall of the flask with deionized water during accuratetitration. Would this washing affect the outcome of the titration? Explain.4. In this experiment a 25.0-mL sample of vinegar is diluted to 100.0 mL; then, a 10.00-mL portionof the dilute vinegar solution is placed in an Erlenmeyer flask and titrated with standardizedNaOH solution. If 19.40 mL of 0.1065 M NAOH solution is required to reach endpoint, what is theconcentration of acetic acid in diluted vinegar? Calculate the molar concentration of acetic acid inthe original (undiluted) vinegar.

As per the bartleby guidelines we solved the first three parts of the given question. Analyte: A…

1. (a) What is the purpose of titration in volumetric analysis, and briefly explain how is it carried out? (b) What is an indicator and why it is used in titrations? (c) What indicator will be used in this experiment and to which solution it is added?

1. (a) What is the purpose of titration in volumetric analysis, and briefly explain how is it carried out? (b) What is an indicator and why it is used in titrations? (c) What indicator will be used in this experiment and to which solution it is added?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 65QAP: Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is...

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After studying the separation scheme for Group III cations and using your background knowledge on separation of Group I and Group II cations: (a) devise a flow chart or schematic diagram to separate and confirm the presence of the given ions in the solution below; (b) write the chemical formula of the precipitates formed; and (c) provide a brief explanation about your schematic diagram.
Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake.A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant.1. What is the concentration of hydroxide ions in the solution? Note: Use the scientific notation of 0.00012 = 1.2e-4 2. Determine s and Ksp of Mg(OH)2.Note: Use the scientific notation of 0.00012 = 1.2e-4
Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake. A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant. What is the concentration of hydroxide ions in the solution? Determine solubility s.
What is precipitation-titration? Then, briefly and consisely describe the methodology employed in the study (i.e define the titrant, the primary standards used, precipitants, etc that were essential in the process).
A student carried out an experiment trying to prepare tetra-methyl-ammonium tri-iodide.The student weighed 1.13 g tetra-methyl-ammonium iodide into a beaker containing 25 mL ethanol, and then added 1.57 g of iodine. The mixture was heated gently, whilst stirring, on a hotplate until tetra-methyl-ammonium iodide, a white powder, was completely dissolved. After the mixture was allowed to cool down to room temperature, the mixture was further cooled on ice. After filtration on a Buechner funnel, washing with diethyl ether and leaving it under vacuum suction for a couple of minutes, the student recovered the product and weighed it. The mass of the obtained tetra-methyl-ammonium triiodide was 1.62 g.What is the yield of the reaction in percent [%]? For the calculation, assume that the product is completely dry and pure, so there are no impurities like side-products, unreacted educts, or solvent residues.
When standardizing two liters of a potassium permanganate solution, approximately 0.0100 M, with a primary standard solution of sodium oxalate, it was planned to use between 30.00 and 45.00 ml of the titrated reagent. In which mass range (in grams) the primary standard should be weighed?
If the experiment started with solid KHP instead of a solution, why would it be acceptable to use a graduated cylinder to measure the water to make the KHP solution when a volumetric flask is used to mix the NaOHsolution?
A second analyst was attempting to determine the percent KHP in an unknown sample, similar to that in the CEM 262 laboratory experiment 1. The analyst found the molarity of the standardized NaOH solution to be 0.1016 mol/L. Three aliquots of the unknown sample having weights of 0.8181 g, 0.9393 g, and 0.8719 g were titrated with the NaOH solution requiring 20.00 mL, 22.39 mL, and 22.14 mL, respectively. From these data, determine the average percent KHP in the unknown sample.
A solid sample containing chloride ion is analyzed by argentimetric titration to find the percentage chloride by mass. The procedure involves the preparation of a solution made from primary standard sodium chloride (molar mass = 58.443 g mol-1). Aliquots of NaCl solution will be titrated with silver nitrate solution to accurately determine the AgNO3 concentration. The standardized silver nitrate will be used to titrate aliquots of unknown chloride solution, thus allowing for the determination of the percentage chloride in the original solid sample. To detect the endpoint of the titration the adsorption indicator dichlorofluorescein is used. Please solve for the highlighted portions.
f the mass of the KHP is 0.550 g and the average volume of the prepared NaOH solution consumed in the titration is 33.0mL, what is the standardized concentration of NaOH?
What is the titer (expressed in milligrams per milliliters) of a solution of oxalic acid dihydrate with respect to calcium oxide if 21.49 mL of it was needed to titrate 0.2203 g of calcium oxide?
After transfering the completely dissolved NaOH to the volumetric flask from the beaker, the beaker was washed with distilled water. What will happen to the apparent concentration of the solution if the beaker used to dissolve the NaOH was not covered with glass and the distilled water used to wash the beaker was disposed of in the sink? Select one: a. The concentration will decrease because the NaOH may evaporate b. The concentration will decrease because there may be NaOH present in the distilled water used to wash the beaker c. The concentration will not change because all NaOH was transferred to the volumetric flask d. The concentration will increase because the water may evaporate