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Chapter 4: Problem 31

Identify each of the following species as a Br贸nsted 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
(a) Acid, (b) Base, (c) Both, (d) Both.

Step by step solution

01

Define Br酶nsted Acids and Bases

A Br酶nsted acid is a substance that can donate a proton (H鈦�) to another substance. A Br酶nsted base is a substance that can accept a proton from another substance.
02

Analyze HI

HI is a molecule that can donate a proton to a base, forming I鈦� after losing one H鈦�. Therefore, HI is a Br酶nsted acid.
03

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

The acetate ion \((\mathrm{CH}_{3} \mathrm{COO}^{-})\) can accept a proton to form acetic acid \((\mathrm{CH}_{3} \mathrm{COOH})\). Thus, \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) is a Br酶nsted base.
04

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

\(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\), the dihydrogen phosphate ion, can either donate a proton to become \(\mathrm{HPO}_{4}^{2-}\), or it can accept a proton to become \(\mathrm{H}_{3} \mathrm{PO}_{4}\). Thus, it acts as both a Br酶nsted acid and base (amphiprotic).
05

Analyze \(\mathrm{HSO}_{4}^{-}\)

\(\mathrm{HSO}_{4}^{-}\), the bisulfate ion, can donate a proton to become \(\mathrm{SO}_{4}^{2-}\), or it can accept a proton to reform \(\mathrm{H}_{2} \mathrm{SO}_{4}\). Hence, it acts as both a Br酶nsted acid and base (amphiprotic).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Br酶nsted acid
In the Br酶nsted-Lowry theory, a Br酶nsted acid is characterized by its ability to donate a proton, which is symbolized as (H鈦�), to another molecule or ion. This transfer of the proton is fundamental in acid-base interactions. A common example of a Br酶nsted acid discussed is the molecule HI. HI can release a proton to form the iodide ion (I鈦�), demonstrating its role as a proton donor.

To identify a Br酶nsted acid in chemical reactions, look for substances that lose a hydrogen ion.
  • The strength of an acid can vary; some fully donate their protons in water like strong acids, while weak acids partially dissociate.
  • HI is an example of a strong acid, as it completely dissociates in water, making it a classic example of a Br酶nsted acid.
Br酶nsted base
Conversely, a Br酶nsted base is defined by its ability to accept a proton (H鈦�) from another substance. This acceptance of a proton allows Br酶nsted bases to perform essential roles in chemical equilibria and reactions. A typical illustration of a Br酶nsted base is the acetate ion ( CH鈧僀OO鈦�), which can accept a proton to transform into acetic acid ( CH鈧僀OOH).

When identifying a Br酶nsted base, observe for substances that gain hydrogen ions in reactions.
  • Bases can range from strong to weak, depending on their ability to accept protons.
  • The acetate ion is a weaker base compared to others like OH鈦�.
The transformation of the acetate ion exemplifies its role in buffering systems and its capability to maintain pH levels in various solutions by accepting protons.
Amphiprotic species
An amphiprotic species is quite versatile in the realm of acids and bases because it can act as both a Br酶nsted acid and a Br酶nsted base. This dual functionality allows them to either donate or accept a proton (H鈦�), making them vital in various chemical processes. The dihydrogen phosphate ion ( H鈧侾O鈧勨伝) serves as an excellent example of an amphiprotic species. It can lose a proton to become HPO鈧劼测伝 or gain a proton to transform into H鈧働O鈧�.

Another amphiprotic species is the bisulfate ion ( HSO鈧勨伝), which can act similarly by donating a hydrogen ion to become (SO鈧劼测伝) or accepting a proton to revert back to (H鈧係O鈧�).
  • This capability is significant in buffer solutions, which regulate pH by reacting with any excess acids or bases.
  • Being able to both accept and donate protons makes amphiprotic species extremely useful in maintaining the balance in various reaction environments.

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Most popular questions from this chapter

Lithium fluoride (LiF) is a strong electrolyte. What species are present in \(\mathrm{LiF}(a q) ?\)

You have \(505 \mathrm{~mL}\) of a \(0.125 \mathrm{M} \mathrm{HCl}\) solution and you want to dilute it to exactly \(0.100 M\). How much water should you add? Assume volumes are additive.

Calculate the volume in \(\mathrm{mL}\) of a solution required to provide the following: (a) \(2.14 \mathrm{~g}\) of sodium chloride from a \(0.270 \mathrm{M}\) solution, (b) \(4.30 \mathrm{~g}\) of ethanol from a \(1.50 M\) solution, (c) \(0.85 \mathrm{~g}\) of acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) from a \(0.30 \mathrm{M}\) solution.

A sample of \(0.6760 \mathrm{~g}\) of an unknown compound containing barium ions \(\left(\mathrm{Ba}^{2+}\right)\) is dissolved in water and treated with an excess of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\). If the mass of the \(\mathrm{BaSO}_{4}\) precipitate formed is \(0.4105 \mathrm{~g},\) what is the percent by mass of \(\mathrm{Ba}\) in the original unknown compound?

A \(5.00 \times 10^{2}\) -mL sample of \(2.00 M\) HCl solution is treated with \(4.47 \mathrm{~g}\) of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.
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