Introduction to Solutions
### Introduction
A solution is a homogeneous mixture of two or more substances. The substance present in a larger
amount is called the solvent, while the substance present in a smaller amount is called the solute.
### Types of Solutions
Solutions can be classified based on the physical state of the solvent and solute:
1. **Gaseous Solutions**: Gas dissolved in gas (e.g., air).
2. **Liquid Solutions**:
- Gas in liquid (e.g., oxygen in water)
- Liquid in liquid (e.g., alcohol in water)
- Solid in liquid (e.g., salt in water)
3. **Solid Solutions**:
- Gas in solid (e.g., hydrogen in palladium)
- Liquid in solid (e.g., mercury in gold - amalgam)
- Solid in solid (e.g., alloys like brass).
### Concentration of Solutions
Concentration refers to the amount of solute present in a given quantity of solvent or solution.
Common terms include:
- **Mass Percentage**: (Mass of solute / Mass of solution) × 100
- **Volume Percentage**: (Volume of solute / Volume of solution) × 100
- **Molarity (M)**: Moles of solute per liter of solution
- **Molality (m)**: Moles of solute per kg of solvent
- **Mole Fraction**: Ratio of moles of one component to total moles in solution
This chapter further explores colligative properties, Raoult's law, and ideal and non-ideal solutions.
### Introduction
A solution is a homogeneous mixture of two or more substances. The substance present in a larger
amount is called the solvent, while the substance present in a smaller amount is called the solute.
### Types of Solutions
Solutions can be classified based on the physical state of the solvent and solute:
1. **Gaseous Solutions**: Gas dissolved in gas (e.g., air).
2. **Liquid Solutions**:
- Gas in liquid (e.g., oxygen in water)
- Liquid in liquid (e.g., alcohol in water)
- Solid in liquid (e.g., salt in water)
3. **Solid Solutions**:
- Gas in solid (e.g., hydrogen in palladium)
- Liquid in solid (e.g., mercury in gold - amalgam)
- Solid in solid (e.g., alloys like brass).
### Concentration of Solutions
Concentration refers to the amount of solute present in a given quantity of solvent or solution.
Common terms include:
- **Mass Percentage**: (Mass of solute / Mass of solution) × 100
- **Volume Percentage**: (Volume of solute / Volume of solution) × 100
- **Molarity (M)**: Moles of solute per liter of solution
- **Molality (m)**: Moles of solute per kg of solvent
- **Mole Fraction**: Ratio of moles of one component to total moles in solution
This chapter further explores colligative properties, Raoult's law, and ideal and non-ideal solutions.
