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The book states: "The more negative the potential, the greater is the electron-donating power of the oxidation half-reaction and therefore the more strongly reducing the redox couple (that is, the stronger the tendency for the half-reaction to occur as an oxidation)".
So the standard potential in general states how likely a half reaction will become reduced. So, the higher the standard potential, the more likely the half reaction will reduce (and thus act as the oxidizing agent because it oxidizes the other half reaction). Therefore, the more negative the standard potential, the more likely it is the half reaction will become oxidized, which reduces the other half reaction (acting as the reducing agent, meaning it has increased reducing strength).
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