Acids and Bases | Chemical Equilibrium | CBSE | Class 11 Chemistry by Elearnin
Elearnin・2 minutes read
Arrhenius, Bronsted-Lowry, and Lewis concepts explain acids and bases behaviors in different ways. They detail how substances ionize in water, donate or accept hydrogen ions, and interact with electron pairs. Understanding the ionization of acids and bases, as well as their strengths, is crucial in determining their behavior and properties.
Insights
- The Arrhenius concept defines acids as substances that produce H+ ions in water and bases as those producing hydroxyl ions, but it is limited to water molecules.
- The Lewis concept expands the definition of acids and bases by focusing on electron pair donation and acceptance, illustrating that not all acids contain protons and emphasizing the importance of ionization in the process.
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Recent questions
What defines an acid and a base?
The Arrhenius concept states that substances producing H+ ions are acids, while those producing hydroxyl ions are bases when dissolved in water.
How do acids and bases interact?
According to the Bronsted-Lowry concept, acids donate hydrogen ions, and bases accept them, forming conjugate acid-base pairs that differ by a single proton.
What distinguishes the Lewis concept?
In the Lewis concept, acids accept electron pairs, and bases donate them, with examples like BF3 accepting electrons from NH3 to form BF3 and H3.
How do strong acids and bases behave?
Strong acids like HCl fully ionize in water to produce H3O+ and Cl-, while strong bases like LiOH fully ionize to yield OH- ions, indicating good proton donation/acceptance.
What determines the strength of weak acids?
The ionization constant Ka represents the strength of weak acids like HX, with a higher Ka indicating a stronger acid. Weak bases partially ionize, forming M+ and OH- ions, with the relationship between Ka and Kb determining net action equilibrium.
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Summary
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Acid-Base Concepts: Arrhenius, Bronsted-Lowry, Lewis
- Arrhenius concept of acids and bases: Substances that dissolve in water to produce H+ ions are acids, while those producing hydroxyl ions are bases. HX gives H+ and X- ions, forming hydronium ions. OH- ions also exist. However, this concept is limited to water molecules.
- Bronsted-Lowry concept: Acids donate hydrogen ions, bases accept them. HCl + H2O yields H3O+ + Cl-, NH3 + H2O yields NH4+ + OH-. Conjugate acid-base pairs differ by a single proton.
- Lewis concept: Acids accept electron pairs, bases donate them. BF3 + NH3 forms BF3 and H3. Not all acids contain protons, like BF3. Ionization is the process of gaining or losing atoms or electrons.
- Ionization of acids and bases: Strong acids fully ionize, weak acids partially. HA + H2O yields H3O+ + A-. Strong bases like LiOH and NaOH fully ionize, producing OH-. Strong acid/base indicates good proton donation/acceptance.
- Ionization constant of weak acids: Ka represents the ionization constant of a weak acid HX. Higher Ka means stronger acid. Weak bases like MOH partially ionize, forming M+ and OH-. Relationship between Ka and Kb determines net action equilibrium.
- Tri and polybasic acids/bases: Some acids like H2X are polybasic, with multiple ionizable protons. For example, H2X yields H+ + HX-. Multi-acidic bases like MOH2 have more than one ionizable proton. MOH2 forms M+ OH- + OH2-.
