Understanding Substances, Mixtures, and Separation Techniques

Classified in Chemistry

Written at on English with a size of 2.62 KB.

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

  1. Use a magnet to separate iron filings from gasoline and sand. The iron filings will stick to the magnet.
  2. 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

Entradas relacionadas: