Which of the following causes the sharpest change in the equivalence point of a complexometric titration? a) Increasing the concentration of the EDTA solution b) Decreased concentration of the analyte c) increase the stability of the [metal-EDTA] complex
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Which of the following causes the sharpest change in the equivalence point of a complexometric titration?
a) Increasing the concentration of the EDTA solution
b) Decreased concentration of the analyte
c) increase the stability of the [metal-EDTA] complex
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Solved in 3 steps
- Which of the following causes the sharpest change in the equivalence point of a complexometric titration? A. Increasing the concentration of the EDTA solution B. Decreased concentration of the analyte C. Increasing the concentration of the EDTA solution D. Increasing the stability of the [metal-EDTA] complexWhich of the following statements about the indicators used in Edta titrations is false?A. The strength of the complex made with the metal ion should be less than the complex of the same metal with EDTA.B. Metal indicators are used to determine the turning point in complexometric titrations.C. They should form water-soluble colored chelate complexes with metals.D. The complex formation constant of the complex made with metal ions must be very low.The following statements are ways to mitigate EDTA titration's low sensitivity EXCEPT A. Buffer at specific pH to avoid other metal ions to complex with EDTA B. Use of masking agents to react with other cations C. Using higher concentration of EDTA titrant D. Use of optimal form of EDTA that will complex with the target metal ion/s E. None of the choices.
- What conditions must be followed to perform complexometric titration?A. presence of a catalystB. low temperatureC. [metal-EDTA] complex should be more stable than [metal-indicator] complexD. always add an EDTA solution to the analyzed solution and not vice versa11.Residual EDTA titrations are employed in the analysis of Bi and ________ containing compounds. 12.The equilibrium constant that drives complexation reactions to completion is known as?Which of the following statement regarding EDTA titration is incorrect In back titration, excess EDTA is titrated with another standard solution of a second metal ion In normal direct titration, the color of the endpoint is from the metal-indicator complex In indirect titration, the analyte can not be titrated against EDTA In masking titration, the sample or the interference can be isolated by "masking"
- In complexation volumetry, classify the statements below as true or false.Justify the one(s) that you judge to be “false”.a) When preparing an EDTA solution, to be used as a titrant of Ca2+ ions, it is necessary to add a small amount of Mg2+ in the solution.b) A metallochromic (Ind) indicator is a substance that forms colored complexes with metallic ions. The colors of these complexes are always the same as the colors of the free forms of these indicators.c) In order for the titration of a metal (Me) with EDTA to be carried out, it is necessary that the Me-EDTA complex has a stability constant greater than that of the Me-Ind complex.d) In determining the partial hardness of a hard water sample with EDTA solution, murexide is used as an indicator at pH 10.Which of the following can be used to determine the turning point in a complexometric titration? A. Redox markers b.Adsorption markers C. Eriochrome black T D. FenolftaleynWhich of the following is TRUE regarding the EDTA titration? a. The formation of complex favors the reaction with the lowest Kf value. b. In a solution with Mg and Ca ions, EDTA will favor complexation with Ca due to lower Kf value. c. Calcium ions would favor reaction with EDTA than EBT since this would result to higher Kf value. d. In the experiment, all Mg-complex are less stable than Ca-complex.
- For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL was taken from the prepared sample, diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The solution prepared was titrated with 27.4mL of 0.0097 M EDTA solution. Calculate the amount of calcium in the sample in terms of% CaCO3. (Ca = 40 g / mol, CaCO3 = 100g / mol) A. 4.47 B. 8.95 C. 3.58 D. 5.83For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g, necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The solution prepared was titrated with 27.4mL of 0.0097 M EDTA solution. Calculate the amount of calcium in the sample in terms of% CaCO3. (Ca = 40 g / mol, CaCO3 = 100g / mol)For complexometric titration of Ca (II) ions in the shell of an egg sample weighing 59,427 g, the necessary processes were applied to the egg shells and a sample of 100 mL was prepared. From the prepared sample, 1 mL was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dripped on it. The prepared solution was titrated with 27.4 mL of EDTA solution set at 0.0097 M. Calculate the amount of calcium in the sample in CaCO3%. (Ca = 40g / mol, CaCO3= 100g / mol)
