Chemistry: Acids and Bases

Definition: Substances that donate protons (H⁺ ions) in a solution.
Properties:
- Sour taste (e.g., citric acid, acetic acid)
- Conduct electricity when dissolved in water (electrolytes)
- Change color of pH indicators (e.g., litmus turns red)
Strong Acids: Completely dissociate in water (e.g., hydrochloric acid, sulfuric acid).
Weak Acids: Slightly dissociate in water (e.g., acetic acid, citric acid).

Definition: Substances that accept protons or donate hydroxide ions (OH⁻) in a solution.
Properties:
- Bitter taste (e.g., sodium hydroxide, ammonia)
- Slippery feel (e.g., soap)
- Change color of pH indicators (e.g., litmus turns blue)
Strong Bases: Completely dissociate in water (e.g., sodium hydroxide, potassium hydroxide).
Weak Bases: Partially dissociate in water (e.g., ammonia).

Range: 0 to 14, measuring acidity and basicity.
- pH < 7: Acidic
- pH = 7: Neutral
- pH > 7: Basic
Importance: Indicates the concentration of H⁺ ions in a solution.

Definition: Reaction between an acid and a base to produce a salt and water.
General Equation:
- Acid + Base → Salt + Water
Example: HCl + NaOH → NaCl + H₂O

Definition: Ionic compounds formed from the neutralization of an acid by a base.
Properties:
- Generally crystalline at room temperature
- Can be soluble or insoluble in water
- Often have distinct tastes (e.g., table salt - sodium chloride)
Types:
- Acidic Salts: Formed from a strong acid and weak base (e.g., ammonium chloride).
- Basic Salts: Formed from a weak acid and strong base (e.g., sodium bicarbonate).
- Neutral Salts: Formed from strong acids and strong bases (e.g., potassium sulfate).

Acids: Used in food preservation, battery production, and cleaning agents.
Bases: Commonly found in cleaning products, antacids, and fertilizers.
Salts: Essential for human health (e.g., sodium, potassium) and used in various industrial processes.

Substances that release protons (H⁺ ions) in aqueous solutions, contributing to acidity.
Exhibit a sour taste, commonly seen in citric acid (found in citrus fruits) and acetic acid (vinegar).
Conduct electricity when dissolved, classifying them as electrolytes due to ionization.
Change the color of pH indicators; for instance, litmus paper turns red in acidic solutions.
Strong acids, like hydrochloric acid and sulfuric acid, fully dissociate in water, leading to a higher concentration of H⁺ ions.
Weak acids, such as acetic acid and citric acid, dissociate partially in solutions.

Substances that accept protons or release hydroxide ions (OH⁻) in a solution, contributing to basicity.
Characterized by a bitter taste; examples include sodium hydroxide and ammonia.
Feel slippery to the touch, often exemplified by soaps.
Change the color of pH indicators; litmus paper turns blue in basic solutions.
Strong bases, such as sodium hydroxide and potassium hydroxide, completely dissociate in water.
Weak bases, like ammonia, only partially dissociate in solutions.

Ranges from 0 to 14, providing a measure of acidity and basicity of a solution.
pH values below 7 indicate acidic solutions, while a pH of 7 signifies neutrality.
pH values above 7 denote basic solutions.
Critical for understanding the concentration of H⁺ ions in various solutions, influencing chemical reactivity and biological processes.

Defined as a chemical reaction where an acid reacts with a base to form a salt and water.
General reaction can be represented as: Acid + Base → Salt + Water.
Example: The neutralization of hydrochloric acid (HCl) with sodium hydroxide (NaOH) produces sodium chloride (NaCl) and water (H₂O).

Ionic compounds resulting from the neutralization of an acid with a base.
Typically crystalline at room temperature and may vary in solubility in water; some are soluble while others are not.
Exhibit distinctive tastes, such as sodium chloride (table salt).
Can be categorized into:
- Acidic salts: Made from strong acids and weak bases (e.g., ammonium chloride).
- Basic salts: Formed from weak acids and strong bases (e.g., sodium bicarbonate).
- Neutral salts: Result from the neutralization of strong acids and strong bases (e.g., potassium sulfate).

Acids play vital roles in food preservation, battery manufacturing, and as cleaning agents.
Bases are commonly used in household cleaning products, as antacids for digestive relief, and as fertilizers in agriculture.
Salts are essential for human health, contributing to key bodily functions (e.g., sodium and potassium) and are utilized in various industrial applications.