Statement 1: Mohr titration is usually performed in an acidic medium. Statement 2: This is because under acidic conditions, the chromate ion is protonated to form chromic acid which leads to immediate precipitation at the end point. Statement 1 is incorrect and Statement 2 is correct Both statements are correct Both statements are incorrect Statement 1 is correct and Statement 2 is incorrect

Statement 1: Mohr titration is usually performed in an acidic medium. Statement 2: This is because under acidic conditions, the chromate ion is protonated to form chromic acid which leads to immediate precipitation at the end point. Statement 1 is incorrect and Statement 2 is correct Both statements are correct Both statements are incorrect Statement 1 is correct and Statement 2 is incorrect

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter10: Fuels, Organic Chemicals, And Polymers

Section: Chapter Questions

Problem 115QRT

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only SELECT correct respomses 1) Titrations of different forms are often employed to quantitate acids, bases, metal ions, and proteins. 2) To perform a titration, the experimenter must be familiar with the stoichiometry of the reaction taking place between the reagent and analyte. 3) Often in titrations, a visible color change will occur in the solution (due to an added indicator solution). 4) Gravimetric titrations directly measure the volume of reagent solution needed to react completely with an analyte. 5) For a monoprotic weak acid titration, the weak acid solution being titrated is the "sample" that is being quantitated. 6) For a monoprotic weak acid titration, the equivalence point is reached when the moles of added base equals the moles of weak acid originally present in the reaction vessel. 7) In a monoprotic weak acid titration, the weak acid is the analyte in solution, and a standardized base (for example, a solution of known concentration of NaOH) is the titrant. 8) A…
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.…
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.…
It is the process in which the concentration of a volumetric solution or titrant is determined by titrating it against a carefully measured quantity of primary standard. a. Digestion b. Back titration c. Gravimetry d. Standardization
TRUE OR FALSE 1. Sodium arsenite is formed due to the solubility property of arsenic trioxide in sodium hydroxide. 2. The permanganate method is always carried out in a highly acidic medium. 3. The color of permanganate solution renders impossible accurate readings at the lower meniscus. 4. Sodium bicarbonate in the standardization of iodine solution acts as a buffer. 5. Sulfuric acid in permanganate titration prevents the formation of reduction products.
Fill in the blanks by writing the name of the definition: __________ is a substance which is added to the reaction mixture and changes color at the equivalance point. a. titrant b. Primary standard c. İndicator d. analyte
Which of the statements given below is correct? A. Iodometry is a method in which I2 solution is used as a titrant and substances that can reduce iodine to iodine can be determined. B. Starch indicator is added to the medium at the beginning of the titration. A. All metal salts other than alkali salts dissolved in water cause hardness. D. 1 German hardness is the hardness of water containing cation equivalent to 1 mg CaCO3 in 100 mL.
Iodine can be in the form of I3 and I-2. Why are these forms used in the titration of vitamin C?
Compare and contrast the following general methods of argentometric titration. What are the strengths and limitations of each method? Explain. a. Mohr Methodb. Volhard Methodc. Fajans Method
If two water samples were collected as follows: Sample #1 with a pH = 8.8 and the concentration of [HCO3-] = 0.01 molar Sample #2 with a pH = 87.0 and the concentration of [HCO3-] = 0.00 molar Compare the alkalinity of the two samples Which of these two samples was taken from a well-buffered lake?
Which of the following statements is true? a.The equivalence point is the condition where the moles of analyte is equal to the moles of titrant b.The equivalence point is represented by the formation faint pink color c.The end point is always equal to the equivalence point d.None of the above
Which of the following statements is true? a. The equivalence point is the condition where the moles of analyte is equal to the moles of titrant b. The equivalence point is represented by the formation faint pink color c. The end point is always equal to the equivalence point d. None of the above

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		Statement 1 is incorrect and Statement 2 is correct
		Both statements are correct
		Both statements are incorrect
		Statement 1 is correct and Statement 2 is incorrect