Question

Using the Bronsted theory, classify the following as either an acid or a base by placing the compound in the correct bin. acid

Answer 1

Concepts and reason

Bronsted-Lowry acid is a proton donor and Bronsted-Lowry base is a proton acceptor. The strength of the acidity and basicity of the Bronsted-Lowry acids and bases depends on the polarity of bond between hydrogen and central atom.

First compare the proton accepting or donating tendency of the compounds. Basing on proton donor and acceptor nature classify them into Bronsted acids and base.

Fundamentals

According to Bronsted–Lowry theory, a chemical compound that donates ${{\rm{H}}^ + }$ ion (proton) is known as Bronsted acid and a chemical compound that accepts ${{\rm{H}}^ + }$ ion is called as Bronsted-Lowry base.

The compound, ${\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{C}}{{\rm{H}}_{\rm{2}}}{{\rm{O}}^ - }$ has negative charge, it can accept a proton.

The compound, ${{\rm{C}}_6}{{\rm{H}}_5}{\rm{OH}}$ can donate a proton.

The compound, ${\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{N}}{{\rm{H}}_{\rm{3}}}^ +$ can donate a proton.

The compound, ${\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{C}}{{\rm{H}}_{\rm{2}}}{{\rm{O}}^ - }$ , is a proton acceptor, hence it is Bronsted base.

The compound, ${{\rm{C}}_6}{{\rm{H}}_5}{\rm{OH}}$ , is a proton donor; hence it is a Bronsted acid.

The compound, ${\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{N}}{{\rm{H}}_{\rm{3}}}^ +$ , is a proton donor; hence it is a Bronsted acid.

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