Redox Reactions: Why Doesn't 1 M NaOH Spontaneously Reduce Hydronium?

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1 M NaOH does not spontaneously reduce hydronium ions due to the oxidation state of sodium in the compound, which is Na+ and not metallic sodium (Na). While sodium is a strong reducing agent in its elemental form, in NaOH, it is already oxidized and cannot participate in reduction reactions. The discussion highlights confusion about the nature of reduction and the conditions under which certain substances can act as reducers. The distinction between metallic sodium and its ionic form is crucial for understanding redox reactions. Overall, the inability of 1 M NaOH to reduce hydronium ions stems from the oxidation state of sodium in the compound.
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Homework Statement



Which of the following does not spontaneously reduce 1 M hydronium ion?

Homework Equations



Spontaneous reduction: + E-zero value.

The Attempt at a Solution



The answer is 1 M NaOH. However, sodium is a very strong reducer. Why doesn't this reaction go spontaneously?
 
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And what are "the following", which you have not listed?

While sodium is a strong reducer, kitchen salt doesn't reduce my meals. Calcium is a strong reducer too, but despite being present in my bones, it doesn't reduce me to... something reduced. Can you think why?
 
I really have no clue. I've been looking at redox for the past twelve hours. An explanation would b highly appreciated!
 
But you do know the difference between metallic sodium (Na) and oxidized sodium (Na+) in a compound?
 
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Oh ... Ones not a good reducer
 
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