An aqueous solution of hydrosulfuric acid, H2 S(a q), reacts with an aqueous solution of NaOH(a

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An aqueous solution of hydrosulfuric acid, H2 S(a q),...

An aqueous solution of hydrosulfuric acid, $\mathrm{H}_{2} \mathrm{~S}(a q)$, reacts with an aqueous solution of $\mathrm{NaOH}(a q)$. (a) Write the complete ionic equation for the acid-base neutralization that occurs. (Hint: $\mathrm{S}^{2-}(a q)$ ion is present in the neutralized solution.) (b) What salt would remain behind if you evaporated the water from the neutralized solution?

An aqueous solution of hydrosulfuric acid, $\mathrm{H}_{2} \mathrm{~S}(a q)$, reacts with an aqueous solution of $\mathrm{NaOH}(a q)$.
(a) Write the complete ionic equation for the acid-base neutralization that occurs. (Hint:
$\mathrm{S}^{2-}(a q)$ ion is present in the neutralized solution.)
(b) What salt would remain behind if you evaporated the water from the neutralized solution?

Key Concepts

Salt Formation via Evaporation

When the water is evaporated from an aqueous solution containing an ionic compound, the ions combine to form a solid salt. This process, known as salt formation, is based on the principle that the remaining ions will crystallize out once the solvent is removed. Understanding this concept is essential in contexts such as isolation and purification of ionic compounds from solution.

Acid-Base Neutralization

Acid-base neutralization is a fundamental reaction where an acid reacts with a base to produce a salt and water. In such reactions, hydrogen ions from the acid and hydroxide ions from the base combine to form water, while the remaining ions form an ionic compound (the salt). This concept is central to understanding reaction stoichiometry, reaction mechanisms, and the changes in solution composition following the reaction.

Ionic Equations in Aqueous Solutions

Ionic equations are used to represent reactions in aqueous solutions by breaking down strong electrolytes into their component ions. A complete ionic equation shows all of the species present in the solution, while a net ionic equation excludes spectator ions that do not participate directly in the chemical change. This type of equation is essential for visualizing the actual chemical processes and interactions occurring in aqueous reactions.

Polyprotic Acid Behavior

Polyprotic acids, which can donate more than one proton, exhibit sequential deprotonation steps. Each deprotonation step can have its own equilibrium, and under suitable conditions (especially with strong bases), the acid can be fully deprotonated. This concept is key when analyzing reactions involving polyprotic acids, as it helps predict the formation of various anionic species and their stoichiometric relationships in the reaction.

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