Chapter 16: Problem 13
What are diprotic and triprotic acids? List an example of each.
Short Answer
Expert verified
Diprotic acids can donate two protons, like sulfuric acid (H_2SO_4), while triprotic acids can donate three protons, like phosphoric acid (H_3PO_4).
Step by step solution
01
Understanding Diprotic Acids
Diprotic acids are acids that can donate two protons (H+) per molecule during a reaction. They go through two steps of ionization.
02
Example of a Diprotic Acid
Sulfuric acid (H_2SO_4) is an example of a diprotic acid. In the first step of ionization, it loses one proton to form the bisulfate ion (HSO_4^-), and in the second step, it loses another proton to form the sulfate ion (SO_4^{2-}).
03
Understanding Triprotic Acids
Triprotic acids are acids capable of donating three protons (H+) per molecule during a reaction. They dissociate in three steps, each releasing one proton.
04
Example of a Triprotic Acid
Phosphoric acid (H_3PO_4) is an example of a triprotic acid. It releases protons stepwise to form dihydrogen phosphate (H_2PO_4^-), then hydrogen phosphate (HPO_4^{2-}), and finally the phosphate ion (PO_4^{3-}).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Proton Donation
The concept of proton donation is central to understanding the behavior of acids in chemistry. In simple terms, an acid is a substance that can donate hydrogen ions (H+), commonly referred to as protons, to another substance. Diprotic and triprotic acids, as the names imply, refer to acids that can donate two or three protons, respectively.
This donation of protons occurs through a process called ionization. For diprotic acids, this means that they can undergo two distinct ionization steps, each releasing a proton into solution. Similarly, triprotic acids undergo three ionization steps. In aqueous solutions, the ease of proton donation affects the acid's strength and its pH, which is a measure of acidity. For example, in the ionization of sulfuric acid (a diprotic acid), the first proton is released more readily than the second, indicating a difference in ionization steps and the relative strengths of the resulting ions.
This donation of protons occurs through a process called ionization. For diprotic acids, this means that they can undergo two distinct ionization steps, each releasing a proton into solution. Similarly, triprotic acids undergo three ionization steps. In aqueous solutions, the ease of proton donation affects the acid's strength and its pH, which is a measure of acidity. For example, in the ionization of sulfuric acid (a diprotic acid), the first proton is released more readily than the second, indicating a difference in ionization steps and the relative strengths of the resulting ions.
Ionization Steps
Understanding ionization steps is crucial to predicting the behavior and reactivity of diprotic and triprotic acids in solutions. Ionization is the process by which an acid molecule loses its hydrogen ions. In diprotic acids, this occurs in two stages: the first stage detaches one hydrogen ion, while the second stage removes the second.
For instance, with sulfuric acid (H2SO4), the first stage of ionization produces the bisulfate ion (HSO4-), and the second stage yields the sulfate ion (SO42-). Each step is distinct and has its equilibrium constant, indicating the strength of the acid at each stage. Triprotic acids go through a similar but extended process, involving three such stages of ionization, each releasing a hydrogen ion and producing successively less hydrogenated ions until reaching the fully deprotonated form.
For instance, with sulfuric acid (H2SO4), the first stage of ionization produces the bisulfate ion (HSO4-), and the second stage yields the sulfate ion (SO42-). Each step is distinct and has its equilibrium constant, indicating the strength of the acid at each stage. Triprotic acids go through a similar but extended process, involving three such stages of ionization, each releasing a hydrogen ion and producing successively less hydrogenated ions until reaching the fully deprotonated form.
Acid Examples
There are several well-known examples of diprotic and triprotic acids commonly found in educational materials, laboratories and various industrial processes. For diprotic acids, the quintessential example is sulfuric acid (H2SO4), which is used widely from car batteries to manufacturing fertilizers. Its ability to release two protons makes it a pivotal compound in countless chemical reactions. Another example is carbonic acid (H2CO3), which forms when carbon dioxide dissolves in water and is an important component in maintaining the pH of blood.
As for triprotic acids, phosphoric acid (H3PO4) is a central player in biochemistry, particularly within the energy cycle of living organisms through its role in ATP, and also used in food flavoring and as a rust converter. Citric acid is another triprotic acid, which you may recognize from citrus fruits, that plays an integral role in metabolism and is also employed in the food and beverage industry as a natural preservative and flavor enhancer.
As for triprotic acids, phosphoric acid (H3PO4) is a central player in biochemistry, particularly within the energy cycle of living organisms through its role in ATP, and also used in food flavoring and as a rust converter. Citric acid is another triprotic acid, which you may recognize from citrus fruits, that plays an integral role in metabolism and is also employed in the food and beverage industry as a natural preservative and flavor enhancer.