MHB HSO4^-1 as Arrhenius & Bronsted-Lowry Acid/Base

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HSO4^-1 acts as an Arrhenius acid by dissociating in water to produce hydrogen ions, represented by the equation HSO4^- + H2O → SO4^2- + H3O+. As a Brønsted-Lowry base, it accepts a proton, shown by the equation HSO4^- + H+ → H2SO4. Both behaviors illustrate the dual role of HSO4^-1 in acid-base chemistry. This demonstrates its versatility in different acid-base theories. Understanding these reactions is essential for grasping the properties of HSO4^-1 in aqueous solutions.
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write down 2 equations to show how the HSO4^-1 ion can behave as a arrhenius acid and bronsted lowry base

i know if its a arrhenius acid it dissociates in water to produce hydrogen ions

so HSO4^-1 +h20 goes to SO4^-2 and the hydronium ion. is this right? i don't know how to show if its a bronsted lowry base
 
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markosheehan said:
write down 2 equations to show how the HSO4^-1 ion can behave as a arrhenius acid and bronsted lowry base

i know if its a arrhenius acid it dissociates in water to produce hydrogen ions

so HSO4^-1 +h20 goes to SO4^-2 and the hydronium ion. is this right? i don't know how to show if its a bronsted lowry base

Hi markosheehan,

Behavior as an Arrhenius acid means it donates an $H^+$ ion to $H_2O$.
So indeed:
$$HSO_4^{-}(aq) \to SO_4^{2-}(aq) + H^+(aq)$$

Behavior as a Brønsted–Lowry base means it accepts an $H^+$ ion.
So:
$$HSO_4^{-} + H^+ \to H_2SO_4$$
 
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