In this example, which species acts as an acid and why? $H_2SO_4^- +H_2O -> SO_4^(2-) + H_3O^+$

Md Ariful Islam

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Md Ariful Islam

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An acid is a proton donor; a base is a proton acceptor. are substances that respectively increase concentrations of the characteristic cation and the characteristic anion of the , and here the solvent is water.

Now sulfuric acid is diprotic in water. We can separate out 2 successive acid base reactions:

$H_2SO_4 + H_2O rarr H_3O^+ + HSO_4^-$

$HSO_4^(-) + H_2O rarr H_3O^+ + SO_4^(2-)$

In each reaction, the base, the proton acceptor, is water.

You will note that acid/base reactions usually designate water as the solvent. Chemists can use other solvent systems, but at this level (?) stick to the water-based (hydroxide and hydronium) ion definition.

As far as anyone knows, the hydronium or acidium species, $H_3O^+$, is a cluster of water molecules, 3 or 4, with an extra $H^+$ to give $H_7O_3^+$ or $H_9O_4^+$; this cluster can easily exchange the $H^+$ with other water clusters; think of a rugby maul. We write $H_3O^+$ or even $H^+$ for convenience, and we can certainly do calculations on this basis.

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