1. Which is correct: a) The neutral EDTA is triprotic b) EDTA (Y-4) is tetradentate c) The blue EBT indicator is monoprotic d) At pH 3-5 EDTA is completely ionized 2. Which is not correct a) the final result in Volhard's titration is red solution b) the yellow color in redox experiment is iodine c) the Fajan's titration produces pink ppt e) the iodine molecule is oxidized in redox titration d) the thiosulfate is standardized in acidic medium

1. Which is correct: a) The neutral EDTA is triprotic b) EDTA (Y-4) is tetradentate c) The blue EBT indicator is monoprotic d) At pH 3-5 EDTA is completely ionized 2. Which is not correct a) the final result in Volhard's titration is red solution b) the yellow color in redox experiment is iodine c) the Fajan's titration produces pink ppt e) the iodine molecule is oxidized in redox titration d) the thiosulfate is standardized in acidic medium

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

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Which of the following statements CORRECTLY describes a EDTA titration? a. All statements are correct. b. Erichrome black T has the same endpoint with Calmagite indicators and its solution is more stable than the Calmagite. c. EDTA titration can be used only for direct titration methods. d. EDTA Titration can be used in determination of all cations. e. EDTA titration is usually used in the determination of water hardness.
Assuming a 0.010 M EDTA titrant solution, calculate the mass of pure dry CaCO3 standard to use suchthat the volume of titrant needed to reach the endpoint will be about 25 mL if one mole of calciumcarbonate reacts with one mole EDTA.
0.0322 M EDTA solution is used as the titrant in the titration of a 50.00 mL solution that is 0.0129 M in Cu2+. The solution is held at pH = 10.00 by a buffer that is 0.050 in ammonia (NH3). At what volume (in mL) of EDTA added will the equivalence point be reached?
In order to adjust the AgNO3 solution prepared as 0.1M, 25 ml of the standard NaCl solution with a concentration of 0.1025M is taken and necessary procedures are carried out. Since 24.3 ml AgNO3 solution is used for the titration, what is the concentration of AgNO3 solution?
A 24.0 mL sample of 0.113 MM sulfurous acid (H2SO3) is titrated with 0.1013 M KOH. At what added volume of base solution does the first equivalence point occur?
What species are present in a solution giving off a pure blue endpoint in a hard water sample containing an EBT indicator (In) with an EDTA titrant? a. HIn²⁻, CaY²⁻, MgY²⁻ b. HIn²⁻, MgIn⁻, CaY²⁻, MgY²⁻, CaIn⁻ c. HIn²⁻, MgIn⁻ d. HIn²⁻, MgIn⁻, CaY²⁻
Precipitation Titration (Argentimetry) All of the following is true regarding Argetometric titration method except: a) The method can be used for determination of Br and I b) AgNO, is the titrant and it is not a primary standard c) In Fajan's method excess amount of AgNO, is added then back titrated with Thiocyanate d) Different methods can be used for detecting the end point e) Fajan's method depends on using fluorescence indicators such as Dichlorofluorescine
Which of the following is false for potentiometric titration? A. With potentiometric titrations, a more accurate and sensitive reproducible titration end point can be determined than the presence of a chemical indicator. B. More accurate results are obtained in turbid and colored solutions. C. In potentiometric titrations, turning points are calculated from derivative curves. D. Visual acidity or basicity constants of weak acids or weak bases cannot be determined from potentiometric titration curves.
Advantages of potentiometric titrations over 'classical' visual indicator methods: (select the correct statement(s)). Can be used for colored, turbid or fluorescent analyte solution. Can be used if there is no suitable indicator or if the color change is difficult to visualize. Both answers 1 and 2 are correct
Which of the following can be used to determine the turning point in a complexometric titration?A. Redox markersAdsorption markersC. Eriochrome black TD. Fenolftaleyn
A 20.0 mL sample of 0.115 M sulfurous acid (H2SO3) solution is titrated with 0.1014 M KOH. At what added volume of base solution does each equivalence point occur?
A buffer was made by mixing 0.1404 moles of HN3 with 0.1025 moles of KN3 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2367 M HBr to 50.00 mL of the buffer? Ka(HN3) = 1.900e-5. Note: only a portion of the original buffer is used in the second part of the problem.