Acids and Bases W - Lecture

Certainly! Here's a brief overview of acids and bases: Acids and bases are two fundamental categories of substances in chemistry, distinguished by their properties and behaviors in aqueous solutions. 1. **Acids**: - Acids are substances that can donate protons (H⁺ ions) to other substances. - Common examples of acids include hydrochloric acid (HCl), sulfuric acid (H₂SO₄), and citric acid (found in citrus fruits). - Acids typically have a sour taste and can cause a stinging sensation on the skin. - In aqueous solutions, acids increase the concentration of hydrogen ions (H⁺). 2. **Bases**: - Bases are substances that can accept protons or donate hydroxide ions (OH⁻) to other substances. - Common examples of bases include sodium hydroxide (NaOH), ammonia (NH₃), and calcium hydroxide (Ca(OH)₂). - Bases often have a bitter taste and feel slippery to the touch. - In aqueous solutions, bases increase the concentration of hydroxide ions (OH⁻). 3. **pH Scale**: - The pH scale is a measure of the acidity or basicity of a solution. It ranges from 0 to 14. - A pH of 7 is considered neutral, indicating an equal concentration of H⁺ and OH⁻ ions. - pH values below 7 indicate acidic solutions, with lower values corresponding to stronger acids. - pH values above 7 indicate basic (alkaline) solutions, with higher values corresponding to stronger bases. 4. **Neutralization Reactions**: - When an acid reacts with a base, they neutralize each other to form water and a salt. - This type of reaction is called a neutralization reaction. - The general equation for a neutralization reaction is: Acid + Base → Salt + Water. Understanding acids and bases is crucial in various fields, including chemistry, biology, and environmental science. They play essential roles in many chemical reactions and are involved in numerous industrial processes and biological functions.