Write a balanced net ionic equation for the reaction of each...

Write a balanced net ionic equation for the reaction of each of the following aqueous solutions with $\mathrm{H}^{+}$ ions.
(a) sodium fluoride
(b) barium hydroxide
(c) potassium dihydrogen phosphate $\left(\mathrm{KH}_{2} \mathrm{PO}_{4}\right)$

Key Concepts

Balancing Chemical Equations

Balancing chemical equations ensures that the law of conservation of mass and the conservation of charge are obeyed. This is essential when writing net ionic equations, as all atoms and charges must be the same on both sides of the equation.

Spectator Ions

Spectator ions are ions present in the solution that do not participate directly in the chemical reaction. They remain unchanged and are removed from the net ionic equation to simplify the representation of the reaction.

Acid–Base Reactions

Acid–base reactions involve the transfer of protons (H+ ions) between species. When an acid reacts with a base, the acid donates a proton to the base, forming a conjugate pair. Understanding this process is important for writing net ionic equations where H+ is a common reactant.

Ionic Dissociation in Aqueous Solutions

Ionic dissociation refers to the process by which ionic compounds separate into their individual ions when dissolved in water. This concept is critical for understanding reactions in aqueous media, as it explains how compounds exist as free ions that can interact with other ions, such as H+ in acid-base reactions.

Net Ionic Equations

Net ionic equations are representations that show only the chemical species that undergo a change during the reaction. They are used to simplify reactions by eliminating spectator ions, allowing one to focus on the actual chemical process occurring in the solution.

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