Question

What is the conjugate base of \(\mathrm{H}_{3} \mathrm{O}^{+}\) ? of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) ?

Short answer

Conjugate base of \( \mathrm{H}_{3} \mathrm{O}^{+} \) is \( \mathrm{H}_{2} \mathrm{O} \); conjugate base of \( \mathrm{H}_{2} \mathrm{SO}_{4} \) is \( \mathrm{HSO}_4^{-} \).

Step-by-step solution

Understand the concept of a conjugate base

The conjugate base of an acid is formed when the acid donates a proton (H⁺). An acid loses a hydrogen ion to its conjugate base.

Determine the conjugate base of \( \mathrm{H}_{3} \mathrm{O}^{+} \)

Remove one proton (H⁺) from \( \mathrm{H}_{3} \mathrm{O}^{+} \) to get its conjugate base. When \( \mathrm{H}_{3} \mathrm{O}^{+} \) loses a hydrogen ion, we get \( \mathrm{H}_{2} \mathrm{O} \) as the conjugate base.

Determine the conjugate base of \( \mathrm{H}_{2} \mathrm{SO}_{4} \)

Remove one proton (H⁺) from \( \mathrm{H}_{2} \mathrm{SO}_{4} \) to identify its conjugate base. After donation of a hydrogen ion, the conjugate base of \( \mathrm{H}_{2} \mathrm{SO}_{4} \) is \( \mathrm{HSO}_{4}^{-} \).

Key concepts

Acid-Base Reactions

In chemistry, acid-base reactions are essential for understanding many chemical processes. These reactions involve an acid and a base, where the acid donates a proton (H⁺) to the base. This transfer of a proton is what characterizes the reaction.
During the process, the acid becomes its conjugate base after losing the proton, and the base becomes its conjugate acid after gaining a proton.
Here are some key points to remember:

• An acid donates a proton (H⁺) in the reaction.
• A base accepts a proton during the reaction.
• The conjugate acid-base pairs are formed as a result of proton transfer.
• Understanding these reactions helps explain many natural and industrial processes.

Proton Donation

Proton donation is a fundamental concept in acid-base chemistry. It refers to the process by which an acid gives up a proton (H⁺) to a base. When this occurs, the original acid is transformed into what is known as its conjugate base.
This proton donation is central to how acids and bases interact in chemical reactions.
Let's see how this plays out:

• When an acid donates a proton, it reduces its positive charge.
• The acid becomes its conjugate base once it has donated the proton.
• This concept helps in predicting the products of acid-base reactions.

Hydronium Ion

The hydronium ion, represented as \( \mathrm{H}_{3} \mathrm{O}^{+} \), is a common result of acid dissolution in water. When an acid breaks down in water, it donates a proton to a water molecule, forming the hydronium ion. This ion is essentially a water molecule with an added proton.
Understanding hydronium ions is important for grasping the behavior of acids in aqueous solutions:

• Hydronium ions are a key indicator of acidity in a solution.
• They are formed when an acid donates a proton to water.
• The concentration of hydronium ions determines the pH of a solution.

Sulfuric Acid

Sulfuric acid \( \mathrm{H}_{2}\mathrm{SO}_{4} \) is one of the most widely used acids in industry and research. It's a strong acid, meaning it dissociates completely in water, releasing protons readily. When sulfuric acid donates a proton, it forms its conjugate base, the hydrogen sulfate ion (\( \mathrm{HSO}_{4}^{-} \)).
Here are some important aspects of sulfuric acid:

• It poses as a strong acid capable of donating more than one proton.
• Its conjugate base, \( \mathrm{HSO}_{4}^{-} \), can further participate in reactions.
• Widely employed in chemical manufacturing, such as fertilizers and explosives.