Question

Consider the following net ionic equation: $$ \left.\mathrm{H}^{+}(a q)+\mathrm{OH}(a q)\right) \mathrm{H}_{2} \mathrm{O}(l) $$ Make a list of three different sets of two chemical compounds, each of which would result in this net ionic equation when they are mived.

Short answer

The appropriate three pairs of chemical compounds which would result in the given net ionic equation when mixed are: hydrochloric acid and sodium hydroxide, sulfuric acid and potassium hydroxide, and nitric acid with calcium hydroxide.

Step-by-step solution

Understanding Acid-Base Reactions

In acid-base reactions, protons (\( H^{+} \)) are transferred from one reactant (the acid) to another (the base). A compound containing \( H^{+} \) ions can act as an acid as it can donate a proton, while a compound with \( OH^{-} \) can act as a base because it can accept a proton. When an acid and a base react, they neutralize each other to form water.

Finding Pairs of Acids and Bases

Source for the \( H^{+}(aq) \) can be any strong acid such as hydrochloric acid (HCl), sulfuric acid (H_2SO_4), or nitric acid (HNO_3). The \( OH^{-}(aq) \) can come from any strong base such as sodium hydroxide (NaOH), potassium hydroxide (KOH), or calcium hydroxide (Ca(OH)_2).

Matching Acid-Base Pairs

Now it's time to combine the acids from step 2 with the bases. Possible matches are: 1) HCl and NaOH, 2) H_2SO_4 and KOH, 3) HNO_3 and Ca(OH)_2. It's important to note that these combinations will form water and their corresponding salts (NaCl, K_2SO_4, and Ca(NO_3)_2 respectively).

Key concepts

Net Ionic Equation

Understanding the net ionic equation is pivotal for students embarking on the study of chemical reactions, particularly in the realm of acid-base chemistry. Unlike a standard equation that shows all reactants and products, a net ionic equation boils down to the essentials, showcasing only the species that directly participate in the chemical change.

For example, in an acid-base reaction, many spectator ions may be present—ions that do not partake in the reaction and remain unchanged. The net ionic equation omits these spectators, revealing a clear view of the reaction's actual process. This simplification garners a deeper insight into the chemistry taking place. For instance, the equation \(\mathrm{H}^{+}(aq) + \mathrm{OH}^{-}(aq)\rightarrow \mathrm{H}_{2}\mathrm{O}(l)\) symbolizes the quintessential proton transfer that defines an acid-base reaction, culminating in the formation of water, regardless of the source compounds that furnished the \(\mathrm{H}^{+}\) or \(\mathrm{OH}^{-}\) ions.

Proton Transfer

Proton transfer is a key component of acid-base chemistry, and understanding this concept can significantly clarify a plethora of chemical processes. An acid, by definition, is a substance that donates protons (positive hydrogen ions, \(\mathrm{H}^{+}\)), while the base is one that accepts them.

During proton transfer, an exchange of this \(\mathrm{H}^{+}\) ion occurs from an acid to a base. This exchange can be visualized in an aqueous (water-based) medium where water molecules facilitate the movement of the proton.

Illustration of Proton Transfer

In this context, strong acids and bases, due to their complete dissociation in water, readily donate and accept protons, leading to a swift and virtually complete reaction. This exchange is the fundamental process that students can witness in the provided net ionic equation, capturing the essence of how acids and bases interact at a molecular level.

Neutralization Reaction

A neutralization reaction is a specific type of chemical reaction where an acid and a base react to form water and a salt. This process is foundational in acid-base chemistry, serving as a straightforward example of how two seemingly opposing substances can combine to yield completely new products.

In the context of the exercise, when the specified pairs of acids and bases are mixed, each undergoes a neutralization reaction as reflected in the net ionic equation.

Real-world Applications

Such reactions are not merely academic; they are practical and extensively utilized in fields ranging from industrial manufacturing to environmental management. In everyday life, antacids relieving heartburn demonstrate neutralization, where the acid in the stomach is neutralized by a basic compound in the medication.

Students should appreciate not just the stoichiometry but also the underlying concept of neutralization that dictates the transformation of strong, reactive substances into benign and stable compounds such as water and salts.