Predict how each molecule or ion would act, in the Brønsted-Lowry sense, in aqueous solution by writing "acid," "base," "both,"

Question

Allisa [31]

3 years ago

10

Predict how each molecule or ion would act, in the Brønsted-Lowry sense, in aqueous solution by writing "acid," "base," "both,"

or "neither" on the line provided.

Chemistry

2 answers:

Pavel [41] · Answer 1 · 2022-06-28T00:32:53+03:00

The question is incomplete. The molecules/ ions are:

Bicarbonate ion

N-methyl-3-phenyl-3-[4-(trifluoromethyl)phenoxy]propan-1-amine (Prozac)

Para aminobenzoic acid (PABA)

Trinitrotoluene

N-methylpyridinium ion

Answer:

Bicarbonate ion- base

N-methyl-3-phenyl-3-[4-(trifluoromethyl)phenoxy]propan-1-amine (Prozac)-acid

Para aminobenzoic acid (PABA)- both

Trinitrotoluene- acid

N-methylpyridinium ion- neither

Explanation:

In the Brønsted-Lowry sense, an acid is any substance that donates hydrogen ion while a base is any substance that accepts hydrogen ions. Looking at the compounds given above, acidity depends on the molecule's ability to accept or donate protons hence the classification given in the answer.

Fed [463] · Answer 2 · 2022-06-27T23:10:33+03:00

Answer:

Both

Explanation:

produce OH− (hydroxide) ions. According to this view, an acid–base reaction involves the reaction of a proton with a hydroxide ion to form water. Although Brønsted and Lowry defined an acid similarly to Arrhenius by describing an acid as any substance that can donate a proton, the Brønsted–Lowry definition of a base is much more general than the Arrhenius definition. In Brønsted–Lowry terms, a base is any substance that can accept a proton, so a base is not limited to just a hydroxide ion. This means that for every Brønsted–Lowry acid, there exists a corresponding conjugate base with one fewer proton, as we demonstrated in Chapter 4 "Reactions in Aqueous Solution". Consequently, all Brønsted–Lowry acid–base reactions actually involve two conjugate acid–base pairs and the transfer of a proton from one substance (the acid) to another (the base). In contrast, the Lewis definition of acids and bases, discussed in Chapter 8 "Ionic versus Covalent Bonding", focuses on accepting or donating pairs of electrons rather than protons. A Lewis base is an electron-pair donor, and a Lewis acid is an electron-pair acceptor.