Brønsted-Lowry Theory of Acids and Bases

The page discusses the Teoria Brønsteda (Brønsted-Lowry theory) of acids and bases, which is a fundamental concept in chemistry. This theory expands upon earlier models, such as the Teoria kwasów i zasad Arrheniusa (Arrhenius theory of acids and bases), by providing a more comprehensive explanation of acid-base reactions.

According to the Brønsted-Lowry theory, acids are defined as proton (H+) donors, while bases are proton acceptors. This definition allows for a broader understanding of acid-base reactions, including those that occur in non-aqueous solutions.

Definition: In the Brønsted-Lowry theory, an acid is a substance that donates a proton (H+), and a base is a substance that accepts a proton.

The page illustrates several examples of acid-base reactions, demonstrating how proton transfer occurs:

1. H₂O + NH₃ ⇌ H₃O+ + NH₄⁻ In this reaction, water acts as an acid by donating a proton to ammonia, which acts as a base.

2. HNO₃ + H₂O ⇌ H₃O+ + NO₃⁻ Nitric acid donates a proton to water, forming hydronium ions and nitrate ions.

3. H₂S + H₂O ⇌ H₃O+ + HS⁻ Hydrogen sulfide acts as an acid, donating a proton to water.

Example: The reaction between HCl (hydrochloric acid) and water demonstrates proton transfer: HCl + H₂O → H₃O+ + Cl⁻

The concept of conjugate acid-base pairs is also introduced. When an acid donates a proton, it becomes its conjugate base. Similarly, when a base accepts a proton, it becomes its conjugate acid.

Vocabulary: Conjugate acid-base pair - A pair of chemical species that differ by the presence or absence of a proton.

The page emphasizes the amphoteric nature of water, which can act as both an acid and a base depending on the reaction partner. This property is crucial in understanding many chemical processes in aqueous solutions.

Highlight: Water's ability to act as both an acid and a base (amphoteric) is a key concept in understanding reakcje w roztworach wodnych (reactions in aqueous solutions).

The strength of acids and bases is briefly mentioned, indicating that it relates to their ability to donate or accept protons. This concept is important for predicting the direction and extent of acid-base reactions.

Quote: "Moc kwasów i zasad zależy od ich zdolności do oddawania lub przyjmowania protonów." (The strength of acids and bases depends on their ability to donate or accept protons.)

Understanding the Brønsted-Lowry theory is essential for solving problems related to kwasy i zasady Brønsteda zadania (Brønsted acids and bases problems) and for analyzing reakcje w wodnych roztworach elektrolitów (reactions in aqueous solutions of electrolytes).