Question

Identify the Brønsted-Lowry acid and Bronsted-Lowry base in this chemical equation. \(\mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{OH}^{-} \rightarrow \mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{H}_{2} \mathrm{O}\)

Short answer

\(\mathrm{H}_3\mathrm{PO}_4\) is the acid and \(\mathrm{OH}^-\) is the base.

Step-by-step solution

Identify Potential Acid and Base Components

In the given chemical equation \(\mathrm{H}_{3}\mathrm{PO}_{4}+\mathrm{OH}^{-} \rightarrow \mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O}\), we begin by identifying the components that can potentially act as acids and bases. \(\mathrm{H}_3\mathrm{PO}_4\) (phosphoric acid) contains hydrogen ions that can be donated, making it a candidate for an acid. \(\mathrm{OH}^-\) (hydroxide ion) is known to accept hydrogen ions, thus a potential base.

Determine the Brønsted-Lowry Acid

A Brønsted-Lowry acid is a substance that donates a proton (\(\mathrm{H}^+\)). In this reaction, \(\mathrm{H}_3\mathrm{PO}_4\) donates a hydrogen ion to \(\mathrm{OH}^-\), forming \(\mathrm{H}_2\mathrm{PO}_4^-\). Thus, \(\mathrm{H}_3\mathrm{PO}_4\) is the Brønsted-Lowry acid.

Determine the Brønsted-Lowry Base

A Brønsted-Lowry base is a substance that accepts a proton. Here, \(\mathrm{OH}^-\) accepts a hydrogen ion from \(\mathrm{H}_3\mathrm{PO}_4\), resulting in the formation of water (\(\mathrm{H}_2\mathrm{O}\)). Therefore, \(\mathrm{OH}^-\) acts as the Brønsted-Lowry base.

Key concepts

Proton Donation

In the realm of Brønsted-Lowry acid-base theory, proton donation is a cornerstone concept. It revolves around the ability of a chemical species to donate a hydrogen ion, commonly referred to as a proton. This process is essential in identifying acids in chemical reactions. For instance, when we consider the compound \[ \mathrm{H}_3\mathrm{PO}_4 \] it acts as a proton donor in reactions. As it loses a proton in the chemical process, it is transformed into \[ \mathrm{H}_2\mathrm{PO}_4^- \].
This transformation exemplifies the role of \[ \mathrm{H}_3\mathrm{PO}_4 \] as a Brønsted-Lowry acid because it participates in donating a proton.
Understanding proton donation involves recognizing the feature of substances that enable them to relinquish a hydrogen ion. With each proton release, these substances become lesser in hydrogen ions which often results in a new chemical species. Proton donation is not just about losing a hydrogen ion; it’s about participating in an interaction that restores balance in the chemical environment.

Proton Acceptance

Complementing the idea of proton donation in the Brønsted-Lowry theory is proton acceptance. This notion pertains to a chemical species that has the capability to accept a hydrogen ion. It is crucial in identifying bases in chemical reactions. For example, the hydroxide ion \( \mathrm{OH}^- \) in the equation acts as a proton acceptor.
Upon accepting a proton from \( \mathrm{H}_3\mathrm{PO}_4 \), the hydroxide ion transforms into water \( \mathrm{H}_2\mathrm{O} \).
The ability of a base to accept protons facilitates the transformation of acids and bases during a reaction. Recognizable by the hydroxide ion's attraction to protons, this acceptance signifies a base's role in the Brønsted-Lowry concept. This process of proton acceptance underscores the dynamic nature of chemical interactions, where substances constantly shift between accepting and donating protons, thus governing the acid-base balance in solutions.

Chemical Equation Analysis

Chemical equation analysis is invaluable in understanding the interactions within a reaction. It provides a visual representation of the substances before and after the chemical process, showing how reactants transform into products.
In our given equation:\[ \mathrm{H}_{3} \mathrm{PO}_{4} + \mathrm{OH}^{-} \rightarrow \mathrm{H}_{2} \mathrm{PO}_{4}^{-} + \mathrm{H}_{2} \mathrm{O} \]we observe the process of proton donation and acceptance effectively.
Analyzing such equations involves pinpointing each reactant's role, determining which component donates a proton, and which accepts it.

• First, look for the starting materials: \( \mathrm{H}_{3}\mathrm{PO}_{4} \) and \( \mathrm{OH}^- \).
• Note the transformation of \( \mathrm{H}_3\mathrm{PO}_4 \) to \( \mathrm{H}_2\mathrm{PO}_4^- \) (a proton loss).
• Recognize \( \mathrm{OH}^- \) turning into \( \mathrm{H}_2\mathrm{O} \) (a proton gain).

Each shift and transformation in the equation depicts the essence of the reaction, highlighting the exchange of protons between acids and bases. This understanding aids in grasping the mechanics of chemical interactions, essential for further exploration in chemistry.