At what identical concentration of H⁺ and CH₃CO₂^- (?G°_f = -372.5 kJ) will the dissociation of 1 M acetic acid, below, ( $\Delta$ G°_f (CH₃CO₂H (aq)) = -399.6 kJ) become spontaneous at room temperature?
CH₃CO₂H (aq) $\rightarrow$ H⁺(aq) + CH₃CO₂^-(aq)

Question

At what identical concentration of H⁺ and CH₃CO₂^- (?G°_f = -372.5 kJ) will the dissociation of 1 M acetic acid, below, (

\Delta

G°_f (CH₃CO₂H (aq)) = -399.6 kJ) become spontaneous at room temperature?
CH₃CO₂H (aq)

\rightarrow

H⁺(aq) + CH₃CO₂^-(aq)

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The Answer of At what identical concentration of H⁺ and CH₃CO₂^- (?G°_f = -372.5 kJ) will the dissociation of 1 M acetic acid, below, ($\Delta$G°_f (CH₃CO₂H (aq)) = -399.6 kJ) become spontaneous at room temperature? CH₃CO₂H (aq) $\rightarrow$ H⁺(aq) + CH₃CO₂^-(aq)

At What Identical Concentration of H+ and CH3CO2- (?G°f = Δ\DeltaΔ

At What Identical Concentration of H⁺ and CH₃CO₂^- (?G°_f = $\Delta$