Diluted acid is an acid solution containing a relatively low concentration of acid in a solvent, most commonly water. In essence, it's an acid that has been weakened by adding a substantial amount of water.
Understanding Diluted Acids
The process of diluting an acid involves increasing the proportion of the solvent (usually water) relative to the acid. This reduces the concentration of hydronium ions (H3O+) in the solution, which directly impacts the acid's pH and reactivity.
Key Characteristics:
- Lower Concentration: Diluted acids have a lower concentration of acid molecules per unit volume compared to concentrated acids.
- Higher pH: Dilution increases the pH of the acid solution, moving it closer to neutral (pH 7). The pH is still below 7, but higher than the pH of the concentrated acid.
- Reduced Reactivity: Dilution generally decreases the reactivity of the acid. While still capable of undergoing typical acid reactions, the rate of reaction will be slower.
- Higher Water Content: The primary difference between a concentrated and diluted acid is the significantly higher proportion of water in the diluted form.
How to Dilute Acids Safely:
Always add acid to water, and not water to acid. This is because the dilution process is exothermic (releases heat). Adding water to concentrated acid can cause the water to boil rapidly, potentially splashing concentrated acid out of the container, leading to serious burns. Adding acid to water allows the heat to dissipate more safely.
Examples of Diluted Acids:
- Diluted Hydrochloric Acid (HCl): Used in various cleaning and laboratory applications.
- Diluted Sulfuric Acid (H2SO4): Found in car batteries and used in various industrial processes.
- Diluted Acetic Acid (CH3COOH): Vinegar is a common example (typically 5% acetic acid).
Importance of Concentration
The concentration of an acid greatly impacts its properties and uses. Concentrated acids are highly corrosive and dangerous, requiring careful handling. Diluted acids are often safer to use for general purposes.
