Understanding Substances, Mixtures, and Separation Techniques
Classified in Chemistry
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Substances, Mixtures, and Separation Techniques
1. Pure Substances vs. Mixtures
- Distilled Water: Pure substance/compound
- Tap Water: Mixture/homogeneous
- Diamond: Pure substance/element
- Gasoline: Mixture/homogeneous
- Wine: Mixture/homogeneous
- Air: Mixture/homogeneous
2. Dalton's Theory
- Matter is made up of indivisible and indestructible atoms.
- All atoms of the same element are equal in mass and properties.
- Compounds are formed by the combination of different elements.
3. Separation Techniques
- Screening: Separates solid particles of different sizes. Instrument: sieve.
- Filtration: Separates solids from liquids. Instrument: filter.
- Evaporation: Separates solids from liquids when the liquid is not needed. Works best with homogeneous mixtures. The process is faster when heated.
- Settling: Separates immiscible mixtures based on density. Used for heterogeneous mixtures.
- Magnetic Separation: Separates ferromagnetic materials using a magnet.
- Distillation: Separates immiscible liquids or components of a solution by exploiting differences in boiling points.
4. Separating Sand, Gasoline, and Iron
- Use a magnet to separate iron filings from gasoline and sand. The iron filings will stick to the magnet.
- Pour the gasoline and sand mixture into a filter. The gasoline will pass through, leaving the sand on the filter paper.
5. Dissolution and Components
Physiological serum is a homogeneous mixture with distinguishable components. It is a liquid solution where the solvent (water) is in greater proportion and the solute (salt) is in lesser proportion.
6. Dissolution Based on Solute Quantity
- Dilute Solution: Little solute relative to the solvent.
- Concentrated Solution: Plenty of solute relative to the solvent.
- Saturated Solution: Maximum amount of solute dissolved in the solvent.
- Supersaturated Solution: More solute than normally possible, often achieved by heating.
7. Formulas
- % by mass of solute = (mass of solute / mass of solution) x 100
- % by volume of solute = (volume of solute / volume of solution) x 100
- Mass concentration of solute = mass of solute / volume of solution
- Solubility = g solute / 100 mL solvent = g solute / L solvent
1 g = 1000 mg
1 L = 1000 mL