Balance each of the following equations; then change them into balanced net ionic equations: (a) \(\mathrm{K}_{3} \mathrm{PO}_{4}(a q)+\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\mathrm{KNO}_{3}(a q)\) (b) \(\mathrm{Al}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)\) (c) \(\mathrm{Na}_{2} \mathrm{CO}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)\)

Net ionic equations focus on the particles that actually participate in the reaction. Begin with a balanced chemical equation. You'll dissociate the strong electrolytes into their respective ions. Then, identify and cancel out the spectator ions – ions that appear unchanged on both sides of the equation. This simplification isolates the ions and molecules directly involved in the reaction.
For example, in the reaction between potassium phosphate and calcium nitrate:
\[ 2 \mathrm{K}_{3} \mathrm{PO}_{4}(aq) + 3 \mathrm{Ca}(\mathrm{NO}_{3})_{2}(aq) \rightarrow \mathrm{Ca}_{3}(\mathrm{PO}_{4})_{2}(s) + 6 \mathrm{KNO}_{3}(aq) \]
The net ionic equation is:
\[ 2 \mathrm{PO}_{4}^{3-}(aq) + 3 \mathrm{Ca}^{2+}(aq) \rightarrow \mathrm{Ca}_{3}(\mathrm{PO}_4)_{2}(s) \]
Here, the potassium (\

Dissociation is when strong electrolytes dissolve in water and separate into ions. This process is crucial for understanding chemical reactions in aqueous solutions.
For instance, potassium phosphate dissociates as follows: \[ \mathrm{K}_{3} \mathrm{PO}_{4}(aq) \rightarrow 3 \mathrm{K}^{+}(aq) + \mathrm{PO}_{4}^{3-}(aq) \ \]. Similarly, calcium nitrate dissociates into: \[ \mathrm{Ca}(\mathrm{NO}_{3})_{2}(aq) \rightarrow \mathrm{Ca}^{2+}(aq) + 2 \mathrm{NO}_{3}^{-}(aq) \]
This dissociation helps to write the ionic equations, revealing the ions involved in the reaction. It's an essential step in deriving net ionic equations, leading to better insight into the reaction mechanisms.

Spectator ions are ions present in the solution that do not participate in the actual chemical reaction. These ions remain unchanged on both sides of the ionic equation.
Identifying and canceling them helps in simplifying the equation. For instance, in the balanced equation: \[ 6 \mathrm{K}^{+}(aq) + 2 \mathrm{PO}_{4}^{3-}(aq) + 3 \mathrm{Ca}^{2+}(aq) + 6 \mathrm{NO}_{3}^{-}(aq) \rightarrow \mathrm{Ca}_{3}(\mathrm{PO}_{4})_{2}(s) + 6 \mathrm{K}^{+}(aq) + 6 \mathrm{NO}_{3}^{-}(aq) \]
The potassium (\

Balancing chemical reactions ensures the conservation of mass and charge, meaning the same number of atoms for each element and the same total charge should be present on both sides of the equation.
Start by identifying the most complex molecule and balance the atoms within it, progressively moving to simpler molecules. Use coefficients to balance atoms for each element.
For example, to balance: \[ \mathrm{Al}(s) + \mathrm{H}_{2} \mathrm{SO}_{4}(aq) \rightarrow \mathrm{H}_{2}(g) + \mathrm{Al}_{2}(\mathrm{SO}_{4})_{3}(aq) \ \] , it's balanced as: \[ 2 \mathrm{Al}(s) + 6 \mathrm{H}_{2} \mathrm{SO}_{4}(aq) \rightarrow 3 \mathrm{H}_{2}(g) + \mathrm{Al}_{2}(\mathrm{SO}_{4})_{3}(aq) \ \]
Balancing reactions is a fundamental skill in chemistry, aiding in accurate calculations and predictions of reaction outcomes.