Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq)-H2O(l) + LiCl(aq) b. MgS(aq) + CuCl2(aq)-CuS(s) + MgCl2(aq) c. NaOH(aq) + HNO3(aq)-H2O(l ) + NaNO3(aq) d. Na3PO4(aq) + NiCl2(aq)- Ni3(PO4)2(s) + NaCl(aq)

Understanding how to write a balanced molecular equation is crucial when studying chemical reactions. It involves representing the reactants and products of a reaction with their chemical formulas and ensuring that the amount of matter is conserved, following the Law of Conservation of Mass. To do this, one must balance the equation by adjusting coefficients—the numbers placed before compounds—to have the same number of atoms of each element on both sides of the reaction.

For instance, when we mix hydrochloric acid (HCl) with lithium hydroxide (LiOH), a balanced molecular equation would look like this: \( HCl(aq) + LiOH(aq) \rightarrow H_2O(l) + LiCl(aq) \). It shows that one molecule of HCl reacts with one molecule of LiOH to produce one molecule of water and one molecule of lithium chloride, with no atoms lost or gained in the process.

In contrast to the molecular form, a complete ionic equation breaks down aqueous ionic compounds into their constituent ions. Soluble substances dissolve in water and separate into cations and anions, which are surrounded by water molecules. This level of detail can provide a clearer picture of the reaction's underlying processes. For the reaction between HCl and LiOH, the complete ionic equation is:\( H^+(aq) + Cl^-(aq) + Li^+(aq) + OH^-(aq) \rightarrow H_2O(l) + Li^+(aq) + Cl^-(aq) \).

Note that the water produced remains in its molecular form because it is not an ionic compound in liquid state. By writing the reaction this way, we highlight the ion exchange that occurs in the solution. It's a valuable skill to interpret reactions at this ionic level, as it provides insights into the behavior of aqueous solutions.

Among the ions in a complete ionic equation, some do not participate actively in the chemical reaction. These are called spectator ions. Their presence in the solution is important, but they do not change in chemical form or composition during the reaction, thus named because they 'watch' the reaction rather than take part.

In our aforementioned example, the ions \( Li^+(aq) \) and \( Cl^-(aq) \) appear unchanged on both sides of the equation, making them spectator ions. Recognizing spectator ions is essential when simplifying to find the net ionic equation, as it involves canceling them out to focus solely on the ions and molecules that directly interact. Without understanding the role of spectator ions, completing ionic equations would be overly complicated and less informative.

A chemical reaction is a process where reactants convert to products through the breaking and making of chemical bonds. This can result in various changes such as the formation of a precipitate, the change in color or temperature, or the production of a gas. Understanding chemical reactions is central to the study of chemistry as they illustrate how different substances interact and transform.

Each type of chemical reaction has its own pattern. For example, in the reaction between sodium hydroxide (NaOH) and nitric acid (HNO3), we see a neutralization reaction, a type of double displacement reaction. In such reactions, acids and bases react to form water and a salt. The net result is an exchange of ions that yields entirely new compounds. Grasping the underlying principles of these reaction types deepens our comprehension of how substances interact on a molecular level and is indispensable to anyone studying chemistry.