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?
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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.
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- The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1Sketch a photometric titration curve for the titration of Sn2+ with MnO4 . What color radiation should be used for this titration? Explain.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.
- 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. Calculate the pNi at the equivalence point.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 Calculate the approximate transition range of this indicator when used in the titration of Ni2+ with EDTA at pH 5.0.25.00 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 An indicator (Ind) forms a metal-indicator complex with Ni2+ (NiInd), giving aconditional formation constant of 1.00 x 108 at pH 5.0. It is generally assumedthat human eyes can detect about 1 part of one color in 10 parts of another;therefore, the first discernible color change will occur when the [NiInd]:[Ind]ratio changes from 10 to about 0.1.
- Titration of a 25.00 mL sample of mineral water (containing both Ca2+ and Mg2+) at pH 10 required 19.18 mL of 0.01125M EDTA solution. Another 25.00 mL aliquot of the same mineral water was rendered strongly alkaline to precipitate the magnesium. Titration with a calcium-specific indicator required 14.92 mL of the EDTA solution. Calculate the mass of MgCO3 (FW= 84.314 g/mol) in the mineral water in mg (keep 2 decimals).A 0.9352g sample of ore containing Fe³+, Al³+ and Sr²+ was dissolved and made up to 500.00 mL. The analysis of metals was performed using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard 0.03145 mol/L EDTA solution, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Given the molar masses: Fe=55.845 g/mol; Al-26.982 g/mol and Sr-87.620 g/mol. a) Determine the percentage of each of the metals in the sample. b) Explain why the change in pH allows the determination of the three ions in this sample.An EDTA solution was allowed to react with Pb²⁺ to produce 0.25 M PbY²⁻, 2.67×10⁻⁸ M Pb²⁺ and an excess of 0.10 M at equilibrium (K = 1.1×10⁸). What will be the hydronium ion concentration of the resulting solution?
- Consider the titration of 25.0 mL of 0.020 0 M MnSO4 with 0.010 0 M EDTA in a solution buffered to pH 6.00. Calculate pMn21 at the following volumes of added EDTA and sketch the titration curve: 0, 20.0, 40.0, 49.0, 49.9, 50.0, 50.1, 55.0, and 60.0 mL.3. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation ofthe end point was equal to 13.03 mL. Based on this information,a) Outline the two steps involved, representing the related reactions./5b) Calculate the concentrations of CaCO3 and MgCO3 present in the initialsolution./6c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6d) Calculate the…Calculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 26.0 mL
