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Chapter 16: Problem 3

Classify each of these species as a Bronsted acid or base, or both: (a) \(\mathrm{H}_{2} \mathrm{O},\) (b) \(\mathrm{OH}^{-},\) (c) \(\mathrm{H}_{3} \mathrm{O}^{+}\), (d) \(\mathrm{NH}_{3}\) (e) \(\mathrm{NH}_{4}^{+},\) (f) \(\mathrm{NH}_{2}^{-},(\mathrm{g}) \mathrm{NO}_{3}^{-},\) (h) \(\mathrm{CO}_{3}^{2-}\) (i) HBr, (j) HCN.

Short Answer

Expert verified
H2O is both a Bronsted acid and base. OH- and NH3 are Bronsted acids. H3O+, NH4+, HBr and HCN are Bronsted bases. NO3- is neither a Bronsted acid nor base.

Step by step solution

01

Classify H2O as acid or base or both

H2O can donate a H+ ion to become OH- or accept a H+ ion to become H3O+. Therefore, it acts as both a Bronsted acid and base.
02

Classify OH- as acid or base or both

OH- can only accept a H+ ion to become H2O. Therefore, it acts as a Bronsted acid.
03

Classify H3O+ as acid or base or both

H3O+ can only donate a H+ ion to become H2O. Therefore, it acts as a Bronsted base.
04

Classify NH3 as acid or base or both

NH3 can only accept a H+ ion to become NH4+. Therefore, it acts as a Bronsted acid.
05

Classify NH4+ as acid or base or both

NH4+ can only donate a H+ to become NH3. Therefore, it acts as a Bronsted base.
06

Classify NH2- as acid or base or both

NH2- can only accept a H+ ion to become NH3. Therefore, it acts as a Bronsted acid.
07

Classify NO3- as acid or base or both

NO3- cannot donate or accept a H+ ion. Therefore, it is neither a Bronsted acid nor base.
08

Classify CO32- as acid or base or both

CO32- can only accept a H+ ion to become HCO3-. Therefore, it acts as a Bronsted acid.
09

Classify HBr as acid or base or both

HBr can only donate a H+ ion to become Br-. Therefore, it acts as a Bronsted base.
10

Classify HCN as acid or base or both

HCN can only donate a H+ ion to become CN-. Therefore, it acts as a Bronsted base.

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Most popular questions from this chapter

What are the strongest acid and strongest base that can exist in water?

In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid (use \(\mathrm{H}^{+}\) and \(\mathrm{BF}_{3}\) as examples)? What must be present for a molecule or ion to act as a Lewis base (use \(\mathrm{OH}^{-}\) and \(\mathrm{NH}_{3}\) as examples)?

Hemoglobin (Hb) is a blood protein that is responsible for transporting oxygen. It can exist in the protonated form of \(\mathrm{HbH}^{+}\). The binding of oxygen can be represented by the simplified equation $$\mathrm{HbH}^{+}+\mathrm{O}_{2} \rightleftharpoons \mathrm{HbO}_{2}+\mathrm{H}^{+}$$ (a) What form of hemoglobin is favored in the lungs where oxygen concentration is highest? (b) In body tissues, where carbon dioxide is released as a result of metabolism, the medium is more acidic because of the formation of carbonic acid. What form of hemoglobin is favored under this condition? (c) When a person hyperventilates, the concentration of \(\mathrm{CO}_{2}\) in his or her blood decreases. How does this action affect the above equilibrium? Frequently a person who is hyperventilating is advised to breathe into a paper bag. Why does this action help the individual?

Like water, ammonia undergoes autoionization in liquid ammonia: $$\mathrm{NH}_{3}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{NH}_{2}^{-}$$ (a) Identify the Bronsted acids and Brønsted bases in this reaction. (b) What species correspond to \(\mathrm{H}^{+}\) and \(\mathrm{OH}^{-},\) and what is the condition for a neutral solution?

Write all the species (except water) that are present in a phosphoric acid solution. Indicate which species can act as a Bronsted acid, which as a Bronsted base, and which as both a Bronsted acid and a Bronsted base.
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