The following reactions are all similar to those of the industrial chemicals. Complete and balance the equations for these reactions: (a) reaction of a weak base and a strong acid \(\mathrm{NH}_{3}+\mathrm{HClO}_{4} \rightarrow\) (b) preparation of a soluble silver salt for silver plating \(\mathrm{Ag}_{2} \mathrm{CO}_{3}+\mathrm{HNO}_{3} \longrightarrow\) (c) preparation of strontium hydroxide by electrolysis of a solution of strontium chloride \(\operatorname{SrCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \stackrel{\text { electrolysis }}{\longrightarrow}\)

When mixing a weak base with a strong acid, the process is akin to a dance of chemical opposites. The weak base, which only partially ionizes in solution, meets the strong acid that fully dissociates, eagerly releasing its hydrogen ions. A classic example is the reaction between ammonia (NH₃), a typical weak base, and perchloric acid (HClO₄), a notoriously strong acid.

Imagine NH₃ as a hesitant participant, not entirely willing to accept protons, and HClO₄ as a prolific proton donor. When they react, they form ammonium perchlorate (NH₄ClO₄), a salt that is the end product of this neutralization. This reaction is crucial in numerous industrial and laboratory applications, as it allows the careful control of pH levels, a fundamental aspect in many chemical processes.

Key Steps in the Reaction:

• Ammonia accepts a proton (H⁺) from perchloric acid.
• This neutralization forms ammonium perchlorate, the salt.
• Such reactions are widely utilized in the production of fertilizers, cleaning agents, and other ammonium-based compounds.

Silver salts are compounds that play a pivotal role in various industrial processes, including photography, mirrors, and silver plating. Preparing a soluble silver salt like silver nitrate (AgNO₃) involves a reaction where a silver-containing compound, such as silver carbonate (Ag₂CO₃), interacts with a strong acid like nitric acid (HNO₃).

The reaction goes beyond just mixing: it's a transformation where the carbonate's affinity for silver is usurped by nitrate's stronger pull, creating silver nitrate along with carbon dioxide (CO₂) and water (H₂O). Efficiency is key - with precisely two moles of nitric acid needed for one mole of silver carbonate to ensure a complete reaction without any excess reactants. This process has immense significance in electroplating, where the produced silver nitrate is used to coat objects with a layer of silver for aesthetics and corrosion prevention.

Why Silver Nitrate Matters:

• Essential in creating a conductive layer for silver plating.
• Used in the preparation of anti-microbial agents and in photographic materials.
• Acts as a precursor in the synthesis of other silver compounds.

Electrolysis is the fascinating electrical artistry that allows the decomposition of substances using an electric current. When it comes to chemical synthesis, electrolysis is like a sculptor, carving out desired compounds from a block of reactants. Take, for instance, the preparation of strontium hydroxide (Sr(OH)₂) from strontium chloride (SrCl₂).

An electric current is passed through an aqueous solution of SrCl₂, compelling the water to part with its molecules to produce Sr(OH)₂, hydrogen gas (H₂), and chlorine gas (Cl₂). This process is essential in the production of many chemicals, where the precise control of electrical input results in the direct synthesis of target compounds.

The Essence of Electrolysis:

• Efficiently converts reactants into desired products using electric current.
• It is fundamental in the production of various hydroxides and gases.
• Enables the extraction of elements and synthesis of compounds that are difficult to obtain through other reactions.