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). α₄ value under these conditions is 0.85. What will be the hydronium ion concentration of the resulting solution? 1.0 × 10⁻⁶ M 1.0 × 10⁻⁸ M 1.0 × 10⁻¹⁰ M 1.0 × 10⁻¹² M None of the abov

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). α₄ value under these conditions is 0.85. What will be the hydronium ion concentration of the resulting solution? 1.0 × 10⁻⁶ M 1.0 × 10⁻⁸ M 1.0 × 10⁻¹⁰ M 1.0 × 10⁻¹² M None of the abov

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 92AE: The equilibrium constant for the following reaction is 1.0 1023:...

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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?
Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06. (pKa = 4.76) 0.3:1 1.99:1 0.50:1 1.51:1 What is the correct answer? 1,2,3 or 4?
Calamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?
Which member of each pair produces the more acidic aqueous solution: (a) ZnBr2 or CdCl2, (b) CuCl or Cu(NO3)2, (c)Ca(NO3)2 or NiBr2? Explain.
Compare the two quantities based on the given condition. Titration of the same sample solution of MgCl2 I. Volume at EP with 0.10 M EDTA as titrant II. Volume at EP with 0.10 M AgNO3 as titrant Are they equal? Or which one is greater? Or can it be determined?
What will be the molar Y⁴⁻ concentration in a 0.0200 M EDTA solution at a pH of 9.00? (α=0.054)
From the value Kf=1.2×10^9 for Ni(NH3)6^2+, calculate the concentration of NH3 required to just dissolve 0.026 mol of NiC2O4 (Ksp = 4×10^−10) in 1.00 L of solution. (Hint: You can neglect the hydrolysis of C2O4^2− because the solution will be quite basic.)
A 0.5745 g sample of an alloy containing principally bismuth and lead is dissolved in nitric acid and diluted to 250.0 mL in a volumetric flask. A 50.00 mL aliquot is withdrawn, the pH adjusted to 1.5, and the bismuth titrated with 30.26 mL of 0.01024 M EDTA. The pH of the solution is then increased to 5.0 and the lead titrated with 20.42 mL of the same EDTA solution. Calculate the percentages of lead and bismuth in the alloy.
Redox Titration Curve Consider the titration of 100.00 mL of 0.0100 M Ce4+ in 1.00 M HClO4 by 0.0400 M Cu+ to give Ce3+ and Cu2+. Cu2+ + e- ⇄ Cu+ E° = +0.161 V Ce4+ + e- ⇄ Cu3+ E° = +1.700 V (in 1.00 M HClO4) a) What is the overall standard potential for this titration (E°cell)? b) What is the Keq for this reaction?
An EDTA solution was prepared by dissolving approximately 3 grams of Na2H2Y•H2O in sufficient water to give 1 liter of solution. This solution was then standardized against 50.00 mL aliquots of 0.004517 molar Mg2+. An average titration volume of 32.22 mL was required. Determine the molar concentration of EDTA.
As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA.a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTAb. Calculate the percent brucite (Mg(OH)2) content of rock B if it was titrated with 76.5 mL EDTA
0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate the percentage of 38.5 mL of 0.161 M titrant consumed in the titration (Fe: 56 g/mol). 25.4150.82C.76,23D.32,45