3.1 Exactly 1 litre of solution contains 0.018 mole of Ba?+ ions and 0.0018 mole of Pb2+ ions.You wish to separate these ions by selective precipitation using the drop-wise addition of asolution of K2SO4:Explain, by using a full calculation, which of the salts BaSO4 or PbSO, will precipitate first?Given: Kep (BaSO4) = 1.1 x 10-10 and Kep (PBSO4) = 1.6 × 10-83.2A voltaic cell is set up at 25 °C and delivers 0.060 V. One half cell contains an acidified solutionof permanganate and manganese(II) ions, and the other half-cell is based on the followingreaction:Br05 (aq) + 6H30*(aq) + 6e- → Br-(aq) + 9H20 (P), Eed = 1.44 V3.2.1 Write down the fully balanced cell-reaction equation.3.2.2[Mn2+]6What must the value of the ratio;be if [Br03] = 0.90 M, [Br¯] = 1.11 M, and the[MnOg]6pH = 0.60?

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3.1 Exactly 1 litre of solution contains 0.018 mole of Ba2+ ions and 0.0018 mole of Pb2+ ions. You wish to separate these ions by selective precipitation using the drop-wise addition of a solution of K2SO4. Explain, by using a full calculation, which of the salts BaSO, or PbSO4 will precipitate first? Given: Ksp (BaS04) = 1.1 × 10-10 and Ksp (PbS04) = 1.6 × 10-8

3.1 Exactly 1 litre of solution contains 0.018 mole of Ba2+ ions and 0.0018 mole of Pb2+ ions. You wish to separate these ions by selective precipitation using the drop-wise addition of a solution of K2SO4. Explain, by using a full calculation, which of the salts BaSO, or PbSO4 will precipitate first? Given: Ksp (BaS04) = 1.1 × 10-10 and Ksp (PbS04) = 1.6 × 10-8

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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