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Chapter 7: Problem 39

The species: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{HCO}_{3}^{-}, \mathrm{HSO}_{4}^{-}\) and \(\mathrm{NH}_{3}\) can act both as Br枚nsted acids and bases. For each case give the corresponding conjugate acid and base.

Short Answer

Expert verified
The conjugate acid and base pairs are: \(\mathrm{H}_{2}\mathrm{O}/\mathrm{H}_{3}\mathrm{O}^{+}/\mathrm{OH}^{-}\), \(\mathrm{HCO}_{3}^{-}/\mathrm{H}_{2}\mathrm{CO}_{3}/\mathrm{CO}_{3}^{2-}\), \(\mathrm{HSO}_{4}^{-}/\mathrm{H}_{2}\mathrm{SO}_{4}/\mathrm{SO}_{4}^{2-}\), \(\mathrm{NH}_{3}/\mathrm{NH}_{4}^{+}/\mathrm{NH}_{2}^{-}\).

Step by step solution

01

Identify the Substances

We need to analyze each of the four species provided: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{HCO}_{3}^{-}, \mathrm{HSO}_{4}^{-}, \mathrm{NH}_{3}\) to determine their conjugate acids and bases.
02

Consider \(\mathrm{H}_{2} \mathrm{O}\) as an Acid

As an acid, \(\mathrm{H}_{2} \mathrm{O}\) donates a proton (\(\mathrm{H}^{+}\)) to form its conjugate base, \(\mathrm{OH}^{-}\).
03

Consider \(\mathrm{H}_{2} \mathrm{O}\) as a Base

As a base, \(\mathrm{H}_{2} \mathrm{O}\) accepts a proton to form its conjugate acid, \(\mathrm{H}_{3} \mathrm{O}^{+}\).
04

Consider \(\mathrm{HCO}_{3}^{-}\) as an Acid

As an acid, \(\mathrm{HCO}_{3}^{-}\) donates a proton to form its conjugate base, \(\mathrm{CO}_{3}^{2-}\).
05

Consider \(\mathrm{HCO}_{3}^{-}\) as a Base

As a base, \(\mathrm{HCO}_{3}^{-}\) accepts a proton to form its conjugate acid, \(\mathrm{H}_{2}\mathrm{CO}_{3}\).
06

Consider \(\mathrm{HSO}_{4}^{-}\) as an Acid

As an acid, \(\mathrm{HSO}_{4}^{-}\) donates a proton to form its conjugate base, \(\mathrm{SO}_{4}^{2-}\).
07

Consider \(\mathrm{HSO}_{4}^{-}\) as a Base

As a base, \(\mathrm{HSO}_{4}^{-}\) accepts a proton to form its conjugate acid, \(\mathrm{H}_{2}\mathrm{SO}_{4}\).
08

Consider \(\mathrm{NH}_{3}\) as an Acid

As an acid, \(\mathrm{NH}_{3}\) donates a proton to form its conjugate base, \(\mathrm{NH}_{2}^{-}\).
09

Consider \(\mathrm{NH}_{3}\) as a Base

As a base, \(\mathrm{NH}_{3}\) accepts a proton to form its conjugate acid, \(\mathrm{NH}_{4}^{+}\).

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Key Concepts

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

Conjugate Acid
In Br枚nsted-Lowry theory, the conjugate acid is formed when a base accepts a proton. Consider how substances like
  • Water ( \( \text{H}_2\text{O} \) ) acts as a base and accepts a proton, transforming into its conjugate acid, hydronium ( \( \text{H}_3\text{O}^+ \) ).
  • Bicarbonate ( \( \text{HCO}_3^- \) ) acts as a base as well, accepting a proton and becoming carbonic acid ( \( \text{H}_2\text{CO}_3 \) ).
  • Bisulfate ( \( \text{HSO}_4^- \) ) similarly acts as a base in some situations, accepting a proton to form sulfuric acid ( \( \text{H}_2\text{SO}_4 \) ).
  • Ammonia ( \( \text{NH}_3 \) ) is also capable of proton acceptance to form the conjugate acid ammonium ( \( \text{NH}_4^+ \) ).
Conjugate acids are always paired with their corresponding conjugate bases in a chemical reaction. This interconversion highlights how equilibrium is maintained in acid-base reactions.
Conjugate Base
When an acid donates a proton, the resulting species is known as the conjugate base. This process can be seen through
  • Water ( \( \text{H}_2\text{O} \) ) acting as an acid, which after losing a proton, forms hydroxide ( \( \text{OH}^- \) ), its conjugate base.
  • Bicarbonate ( \( \text{HCO}_3^- \) ) functions as an acid when it donates a proton, yielding carbonate ( \( \text{CO}_3^{2-} \) ) as the conjugate base.
  • Bisulfate ( \( \text{HSO}_4^- \) ) can give up a proton, thus transforming into sulfate ( \( \text{SO}_4^{2-} \) ), which is its conjugate base.
  • Ammonia ( \( \text{NH}_3 \) ), while less common, can also act as an acid, resulting in amide ( \( \text{NH}_2^- \) ) as the conjugate base.
Understanding the formation of conjugate bases helps in predicting the behavior of substances in various chemical equilibria.
Proton Donation
Proton donation is a core aspect of the Br枚nsted acid-base theory. In this context, an acid is defined by its ability to donate a proton (\(\text{H}^+\)), which consequently influences its interactions and reactions. When substances like
  • Water ( \( \text{H}_2\text{O} \) ) donates a proton to become hydroxide,
  • Bicarbonate ( \( \text{HCO}_3^- \) ) loses a proton to become carbonate, and
  • Bisulfate ( \( \text{HSO}_4^- \) ) gives up a proton to form sulfate,
  • Ammonia ( \( \text{NH}_3 \) ) donates a proton creating the amide ion.
Each of these transformations shows how acids operate by donating their protons, leading to significant changes in pH and ion concentration in solutions.
Proton Acceptance
Opposite to donation, proton acceptance is a key component of base behavior in acid-base chemistry. A base accepts a proton from an acid, which is essential for neutralization and many other reactions. Instances of proton acceptance include when:
  • Water ( \( \text{H}_2\text{O} \) ) accepts a proton to become hydronium.
  • Bicarbonate ( \( \text{HCO}_3^- \) ) captures a proton resulting in carbonic acid.
  • Bisulfate ( \( \text{HSO}_4^- \) ) gains a proton forming sulfuric acid.
  • Ammonia ( \( \text{NH}_3 \) ) accepts a proton, forming ammonium.
The patterns in proton acceptance show how solutions can become more acidic by absorbing protons, affecting equilibrium and pH levels.

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