Identify each Bronsted acid and base in the following...

Identify each Bronsted acid and base in the following equations. Note that the reactions are assumed to be reversible. a. $\mathrm{HBr}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})$ b. $\mathrm{H}_2 \mathrm{O}(\ell)+\mathrm{N}_3^{-}(\mathrm{aq}) \Leftrightarrow \mathrm{HN}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$ c. $\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})$ d. $\mathrm{SO}_3{ }^{2-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \Rightarrow \mathrm{HSO}_3^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$ e. $\mathrm{HCN}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CN}^{-}(\mathrm{aq})$

Identify each Bronsted acid and base in the following equations. Note that the reactions are assumed to be reversible.
a. $\mathrm{HBr}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})$
b. $\mathrm{H}_2 \mathrm{O}(\ell)+\mathrm{N}_3^{-}(\mathrm{aq}) \Leftrightarrow \mathrm{HN}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
c. $\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})$
d. $\mathrm{SO}_3{ }^{2-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \Rightarrow \mathrm{HSO}_3^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
e. $\mathrm{HCN}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CN}^{-}(\mathrm{aq})$

Key Concepts

Bronsted-Lowry Acid

This concept defines an acid as a species that can donate a proton (H?) in a chemical reaction. It is foundational in understanding acid-base behavior, as it emphasizes the transfer of a proton rather than the formation of hydronium ions or the presence of protons in a molecule.

Bronsted-Lowry Base

According to the Bronsted-Lowry definition, a base is a substance that accepts a proton during a reaction. Recognizing bases involves identifying species that have the capacity to take up protons, which is essential in explaining the mechanism of many acid-base reactions.

Proton Transfer

Central to the Bronsted-Lowry theory is the concept of proton transfer, where a proton is moved from one molecule (the acid) to another (the base). This process defines the direction of reactivity in acid-base reactions and is key to identifying which species are acting as acids or bases.

Conjugate Acid-Base Pairs

Every acid-base reaction gives rise to a conjugate acid-base pair. When an acid donates a proton, it forms its conjugate base, and when a base accepts a proton, it forms its conjugate acid. This pairing helps in understanding reaction reversibility and equilibrium in acid-base chemistry.

Amphiprotic Species

Some substances, such as water, are amphiprotic, meaning they can either donate or accept a proton depending on the chemical context. This dual behavior is crucial when analyzing acid-base reactions, especially when water participates as either a solvent or a reactant.

Transcript

Please give Ace some feedback