Explain why calmagite and eriochrome black T would not work well as indicators for EDTA titrations in acidic solution. Would the same apply to xylenol orange and pyrocatechol violet?
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Explain why calmagite and eriochrome black T would not work well as indicators for EDTA titrations in acidic solution. Would the same apply to xylenol orange and pyrocatechol violet?
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- Why is it necessary to buffer the solution to a pH between 10 and 12 during the complexometric determination of magnesium using EDTA?Elaborate the reason why EDTA is used in many complexometric titrations. How will you be able to improve its selectivity when it comes to analyzing specific metals?b. EDTA cannot be used as a primary standard always. When can EDTA be used as a primarystandard ? Give reason why EDTA is used in complexometric titrations.
- a) What is the equilibrium that influences the colour change of the Eriochrome Black T indicator? b) Consider how ETDA coordinates to metal ions and then consider this ligand below. Could this ligand be substituted for EDTA in a similar experiment? Why? Identify all possible donor atoms in the structure c) What is the function of the buffer solution for this experiment? Consider the form of EDTA (H4Y) compared to the form in the reaction equation below: The reaction of ETDA with metal cations, e.g. Mn+, may be written as: Mn+ + H2Y2– = MYn–4 + 2 H+(i) What type of non-stoichiometric point defect is responsible for the pink colour of LiCl?(ii) What type of stoichiometric defect is shown by NaCl?Explain the analogies between the titration of a metal with EDTA and the titration of a strong acid (H1) with a weak base (A2). Make comparisons in all three regions of the titration curve.
- 25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered to pH 5.0. Given that the formation constant for the Ni-EDTA (NiY2–) chelate is 4.2 x 1018 and the 4 value at pH 5.0 is 3.54 x 10–7. What is EDTA?Consider the titration of 100.0 mL of 0.010 0 M Ce41 in 1 M HClO4 by 0.040 0 M Cu1 to give Ce31 and Cu21, using Pt and saturated Ag | AgCl electrodes.(a) Write a balanced titration reaction. (b) Write two half-reactions for the indicator electrode. (c) Write two Nernst equations for the cell voltage. (d) Calculate E at the following volumes of Cu1: 1.00, 12.5, 24.5, 25.0, 25.5, 30.0, and 50.0 mL. Sketch the titration curve.25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered topH 5.0. Given that the formation constant for the Ni-EDTA (NiY2–) chelate is4.2 x 1018 and the 4 value at pH 5.0 is 3.54 x 10–7. Explain briefly why EDTA is an important reagent used in complexometrictitrations.
- Explain why ionic attractions are weaker in media with high dielectric constants, e. g.,water and aqueous buffers.a) Which ion, Pt(II) or Mn(II), is more likely to form a sulfide in the presence of H2S in water. b) Rationalize your answer with the trends in hard and soft character. c) Give a balance chemical equation from your reaction.An accurately weighed chelometric standard calcium carbonate of 200 mg was used to standardize Disodium Ethylenediaminetetraacetate, using the same procedures set by the monograph. If the molarity of the Disodium EDTA was found to be 0.054 M, what is the final volume of the titrant used?