Baking soda is (a) \(\mathrm{NaHCO}_{3}\) (b) \(\mathrm{NaHCO}_{3}-6 \mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (d) \(\mathrm{Na}_{2} \mathrm{CO}_{3}{ }^{-1} \mathrm{OH}_{2} \mathrm{O}\)

Sodium bicarbonate is a compound with the formula \(\mathrm{NaHCO}_3\). Commonly known as baking soda, it is widely used in baking as a leavening agent due to its ability to release carbon dioxide when it reacts with an acid and heat. Beyond the kitchen, sodium bicarbonate serves diverse roles, from neutralizing odors to acting as a mild cleaning agent.

Chemically speaking, sodium bicarbonate is a salt composed of a sodium cation \(\mathrm{Na}^+\) and a bicarbonate anion \(\mathrm{HCO}_3^-\). When dissolved in water, it slightly dissociates to form sodium and bicarbonate ions, rebalancing pH levels, making it useful for neutralizing acids in both culinary and medical applications.

Chemical nomenclature refers to the systematic naming of chemical compounds based on the rules set by the International Union of Pure and Applied Chemistry (IUPAC). Understanding nomenclature is crucial for communication in the scientific community. For instance, the IUPAC name of baking soda is sodium hydrogen carbonate, correlating to its chemical composition and indicating the presence of hydrogen (\(\mathrm{H}\)), which differentiates it from sodium carbonate (\(\mathrm{Na}_2\mathrm{CO}_3\)).

The IUPAC nomenclature also guides on how to distinguish between ionic compounds, molecular compounds, and acids, ensuring clarity when identifying and working with chemicals. Writing the formula of a compound like sodium bicarbonate correctly is key in recognizing the substance and understanding its properties and interactions.

Ionic compounds are formed from the electrostatic attraction between positively charged cations and negatively charged anions. The nomenclature and properties of ionic compounds come from the ions that make them up. For example, in the case of sodium bicarbonate \(\mathrm{NaHCO}_3\), the sodium ion \(\mathrm{Na}^+\) is the cation, while the bicarbonate ion \(\mathrm{HCO}_3^-\) acts as the anion.

These compounds commonly form a crystalline lattice structure, which gives them high melting and boiling points. Ionic compounds also tend to dissolve well in water due to the polar nature of water molecules, which disrupt the ionic bonds, allowing the ions to disperse in solution. Recognizing an ionic compound is key in predicting its behavior in reactions, such as its ability to conduct electricity when dissolved or molten, a property not typically found in covalent compounds.