Question

What is the difference between (a) a monoprotic acid and a diprotic acid, (b) a weak acid and a strong acid, (c) an acid and a base?

Short answer

(a) A monoprotic acid donates one proton (H+) per molecule, like HCl, while a diprotic acid donates two protons (H+) per molecule, like H₂SO₄. (b) Weak acids partially dissociate in water (e.g., CH₃COOH), while strong acids fully dissociate (e.g., HCl). (c) Acids release H+ ions in water, have pH<7, and neutralize bases, while bases release OH- ions in water, have pH>7, and neutralize acids.

Step-by-step solution

(a) Monoprotic and Diprotic Acids

Monoprotic acids are the acids that can donate only one proton (H+) ion per molecule in a chemical reaction. Examples of monoprotic acids include hydrochloric acid (HCl), nitric acid (HNO₃), and acetic acid (CH₃COOH). Diprotic acids, on the other hand, can donate two protons (H+) ions per molecule in a chemical reaction. Examples of diprotic acids include sulfuric acid (H₂SO₄), carbonic acid (H₂CO₃), and oxalic acid (C₂O₄H₂).

(b) Weak and Strong Acids

Weak acids are the acids that do not completely dissociate into their ions when dissolved in water. In other words, only a small portion of its molecules will ionize, and the equilibrium lies towards the un-ionized form of the acid. Examples of weak acids include acetic acid (CH₃COOH) and phosphoric acid (H₃PO₄). Strong acids, on the other hand, completely dissociate into their ions when dissolved in water. This means that the equilibrium lies entirely toward the ionized forms of the acid. Examples of strong acids include hydrochloric acid (HCl), sulfuric acid (H₂SO₄), and nitric acid (HNO₃).

(c) Acids and Bases

Acids are the substances that release hydrogen ions (H+) when dissolved in water. They have a pH value lower than 7 and are capable of neutralizing bases. Properties of acids include their sour taste, reactivity with metals to produce hydrogen gas, and their ability to turn blue litmus paper red. Bases, on the other hand, are substances that release hydroxide ions (OH-) when dissolved in water. They have a pH value higher than 7 and are capable of neutralizing acids. Properties of bases include their bitter taste, slippery feel, and their ability to turn red litmus paper blue. Examples of bases include sodium hydroxide (NaOH), ammonia (NH₃), and calcium hydroxide (Ca(OH)₂).

Key concepts

Monoprotic and Diprotic Acids

In acid-base chemistry, understanding the differences between monoprotic and diprotic acids is essential. Monoprotic acids are those that can donate only one hydrogen ion (H⁺) per molecule in a chemical reaction. This characteristic makes them straightforward when it comes to reactions and calculations involving stoichiometry. Here are some common examples of monoprotic acids:

• Hydrochloric Acid (HCl)
• Nitric Acid (HNO₃)
• Acetic Acid (CH₃COOH)

Monoprotic acids often have simpler dissociation equations in water, turning into ions with one hydrogen lost.

On the other hand, diprotic acids are capable of donating two protons per molecule. They undergo a two-step dissociation process, meaning they lose hydrogen ions in separate stages. Examples of diprotic acids include:

• Sulfuric Acid (H₂SO₄)
• Carbonic Acid (H₂CO₃)
• Oxalic Acid (C₂O₄H₂)

Learners working with diprotic acids must consider both dissociation steps to fully understand the chemical behavior and calculate concentrations accurately.

Weak and Strong Acids

The strength of acids is another important aspect in the study of acids and bases. It determines how well an acid can donate protons in a solution. Weak acids are only partially ionized in water, meaning that not all of the acid molecules release their protons. As a result, a weak acid solution reaches an equilibrium between the non-ionized acid molecules and the ions produced. Some familiar examples of weak acids are:

• Acetic Acid (CH₃COOH)
• Phosphoric Acid (H₃PO₄)

This partial ionization impacts how these acids behave in solution, influencing their reactivity and pH levels.

Conversely, strong acids completely dissociate in water, meaning nearly every molecule releases its hydrogen ions. This results in a solution with a very high concentration of hydrogen ions and a much lower pH.
Examples include:

• Hydrochloric Acid (HCl)
• Sulfuric Acid (H₂SO₄)
• Nitric Acid (HNO₃)

Understanding whether an acid is weak or strong is crucial, as it directly affects its corrosiveness, reaction rates, and concentrations needed in various applications.

Properties of Acids and Bases

Acids and bases are key players in chemistry, each having distinct properties guiding their behavior and interactions. Acids are substances that release hydrogen ions (H⁺) when dissolved in water. This ion release leads them to have a pH lower than 7. Key properties of acids include their sour taste, similar to citrus fruits, and their reactivity with metals to produce hydrogen gas. Additionally, acids have the ability to turn blue litmus paper red, indicating their acidic nature.

Bases, in contrast, release hydroxide ions (OH⁻) in aqueous solutions, resulting in a pH value greater than 7. Bases are commonly known for their bitter taste and slippery feel, akin to soap. They can neutralize acids, forming water and a salt in the process. One of the distinguishing tests for bases is their ability to turn red litmus paper blue.
Some everyday examples include:

• Sodium Hydroxide (NaOH)
• Ammonia (NH₃)
• Calcium Hydroxide (Ca(OH)₂)

Grasping these properties aids in predicting the outcomes of acid-base interactions and their roles in various environmental and biological systems.