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Chapter 4: Problem 31

Identify each of the following species as a Bronsted acid, base, or both: (a) HI, (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}\), (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (d) \(\mathrm{HSO}_{4}^{-}\)

Short Answer

Expert verified
HI is a Bronsted Acid, \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) is a Bronsted Base, and both \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) and \(\mathrm{HSO}_{4}^{-}\) are amphoteric (Bronsted Acid and Base).

Step by step solution

01

Classification of HI

Hydroiodic acid (HI) is a compound containing hydrogen. It can donate its single proton (H+) to a different compound, hence it acts as a Bronsted acid.
02

Classification of \(\mathrm{CH}_{3} \mathrm{COO}^{-}\)

The compound \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) (acetate ion) has a negative charge and can accept a proton. Hence, it is termed a Bronsted base.
03

Classification of \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

\(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (dihydrogen phosphate ion) can donate a proton considering its hydrogen content, hence acts as a Bronsted acid. Additionally, it also holds a negative charge that allows it to accept a proton, hence it acts as a Bronsted base as well. Thus, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) is a Bronsted acid and base, also termed amphoteric.
04

Classification of \(\mathrm{HSO}_{4}^{-}\)

Similarly, \(\mathrm{HSO}_{4}^{-}\) (hydrogen sulphate ion) has both characteristics. It can donate a proton due to the presence of hydrogen, making it a Bronsted acid. Its ability to accept a proton, due to its negative charge, makes it a Bronsted Base. Hence, \(\mathrm{HSO}_{4}^{-}\) is also amphoteric.

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