Interpretation Introduction Interpretation: The metal that could be used to reduce Mn 2+ ions but not Mg 2+ ions is to be listed. Explanation The substances having large positive reduction half-cell potentials show a strong tendency to gain electrons (reduce) and act as strong oxidizing agents. On the other hand, the substances with large negative reduction half-cell potentials show a strong tendency to lose electrons (oxidize) and act as strong reducing agents. The standard reduction potentials and reduction half-reactions for Mn and Mg are Mn 2 + ( aq ) + 2 e - → Mn ( s ) E º = - 1.18 V Mg 2 + ( aq ) + 2 e - → Mg ( s ) E º = - 2.37 V To reduce M n 2 + ions but not M g 2 + ions, a metal should have large negative reduction half-cell potential than Mn 2+ but small negative reduction half-cell potential than M g 2 +

3rd Edition

ISBN: 9780321809247

Author: Nivaldo J. Tro

Publisher: Prentice Hall

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Chapter 18, Problem 55E

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Interpretation: The metal that could be used to reduce Mn²⁺ ions but not Mg²⁺ ions is to be listed.

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Chapter 18, Problem 54E

Chapter 18, Problem 56E

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Chapter 18 Solutions

Chemistry: A Molecular Approach

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The metal that could be used to reduce Mn 2+ ions but not Mg 2+ ions is to be listed.

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Interpretation: The metal that could be used to reduce Mn2+ ions but not Mg2+ ions is to be listed.

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Chapter 18 Solutions

Interpretation: The metal that could be used to reduce Mn²⁺ ions but not Mg²⁺ ions is to be listed.