Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the diprotic acid H2SeO4.

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Identify the diprotic acid: \( \text{H}_2\text{SeO}_4 \) is a diprotic acid, meaning it can donate two protons (\( \text{H}^+ \)).

Write the first dissociation step: \( \text{H}_2\text{SeO}_4 \rightarrow \text{H}^+ + \text{HSeO}_4^- \).

Write the net ionic equation for the first dissociation: Since \( \text{H}_2\text{SeO}_4 \) is a strong acid, it dissociates completely in water, so the net ionic equation is the same as the molecular equation: \( \text{H}_2\text{SeO}_4 \rightarrow \text{H}^+ + \text{HSeO}_4^- \).

Write the second dissociation step: \( \text{HSeO}_4^- \rightarrow \text{H}^+ + \text{SeO}_4^{2-} \).

Write the net ionic equation for the second dissociation: \( \text{HSeO}_4^- \rightarrow \text{H}^+ + \text{SeO}_4^{2-} \).

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Diprotic Acids

Diprotic acids are acids that can donate two protons (H⁺ ions) per molecule in an aqueous solution. The dissociation occurs in two steps, where each step involves the release of one proton. Understanding the behavior of diprotic acids is crucial for writing balanced equations, as each dissociation step must be represented separately.

Net Ionic Equations

Net ionic equations represent the actual chemical species involved in a reaction, excluding spectator ions that do not participate in the reaction. To write a net ionic equation, one must first write the complete ionic equation and then eliminate the ions that appear on both sides. This concept is essential for accurately depicting the dissociation of acids in solution.

Equilibrium Constants

Equilibrium constants (K) quantify the ratio of products to reactants at equilibrium for a given reaction. For diprotic acids, there are two equilibrium constants corresponding to each dissociation step. Understanding how to write and interpret these constants is vital for analyzing the strength of the acid and the extent of dissociation in solution.