The hydrogen sulfite ion 1HSO3-2 is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water.

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Identify the amphiprotic nature of the hydrogen sulfite ion (HSO_3^-). It can donate a proton (H^+) acting as an acid, or accept a proton acting as a base.

To show HSO_3^- acting as an acid, write the chemical equation where it donates a proton to water (H_2O), forming bisulfite ion (SO_3^{2-}) and hydronium ion (H_3O^+).

The equation for HSO_3^- acting as an acid is: \[ \text{HSO}_3^- + \text{H}_2\text{O} \rightarrow \text{SO}_3^{2-} + \text{H}_3\text{O}^+ \]

To show HSO_3^- acting as a base, write the chemical equation where it accepts a proton from water, forming sulfurous acid (H_2SO_3) and hydroxide ion (OH^-).

The equation for HSO_3^- acting as a base is: \[ \text{HSO}_3^- + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_3 + \text{OH}^- \]

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Amphiprotic Species

An amphiprotic species is a substance that can both donate and accept protons (H+ ions). This dual capability allows it to act as an acid in some reactions and as a base in others. For example, the hydrogen sulfite ion (HSO3-) can donate a proton to water, forming bisulfite (SO3^2-) and hydronium (H3O+), or accept a proton from water, forming sulfuric acid (H2SO3) and hydroxide (OH-).

Acid-Base Reactions

Acid-base reactions involve the transfer of protons between reactants. In these reactions, acids are proton donors, while bases are proton acceptors. Understanding this concept is crucial for writing balanced chemical equations, as it helps identify the products formed when an amphiprotic species interacts with water, either donating or accepting a proton.

Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. Balancing ensures the law of conservation of mass is upheld. When writing equations for the amphiprotic behavior of HSO3-, it is essential to account for all reactants and products, ensuring that the total number of atoms for each element remains constant.