Answered: We have a solution that contains 0.030…

We have a solution that contains 0.030 M Zn2+ ion and 0.10 M Mn2+ ion and you now add NaOH. Calculate the pH that would be required to remove 95% of the first precipitated metal.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 60E: A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly...

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We have a solution that contains 0.030 M Zn2+ ion and 0.10 M Mn2+ ion and you now add NaOH. Calculate the pH that would be required to remove 95% of the first precipitated metal.

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You find 425.0 mLof 0.350 M sodium oxalate in the lab, and you want to use it to make a buffer with a pH of 1.50. What mass of oxalic acid (MW = 90.03 g/mol, Ka= 5.9 × 10–2) is needed to make this buffer? (Neglect any volume changes due to the addition of solid oxalic acid.)
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