If there only about 100 types of elements in the world, why are there so many different kinds of matter? matter of Types

Can it be physically separated? Matter Flowchart MATTER yes no Can it be physically separated? MIXTURE PURE SUBSTANCE Is the composition uniform? no yes Can it be chemically decomposed? no yes Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element Colloids Suspensions

Solutions I. The Nature of Solutions Make a list of as many different solutions as you can think of.

A. Definitions Solution - homogeneous mixture Solute - substance being dissolved Solvent - present in greater amount

A. Definitions Solute - KMnO4 Solvent - H2O

B. Solvation First... Then... Solvation – the process of dissolving solute particles are surrounded by solvent particles First... solute particles are separated and pulled into solution Then...

B. Solvation Non- Electrolyte Weak Electrolyte Strong Electrolyte + sugar - + acetic acid - + salt Non- Electrolyte Weak Electrolyte Strong Electrolyte solute exists as molecules only solute exists as ions and molecules solute exists as ions only DISSOCIATION IONIZATION View animation online.

NaCl(s)  Na+(aq) + Cl–(aq) B. Solvation Dissociation separation of an ionic solid into aqueous ions NaCl(s)  Na+(aq) + Cl–(aq)

HNO3(aq) + H2O(l)  H3O+(aq) + NO3–(aq) B. Solvation Ionization breaking apart of some polar molecules into aqueous ions HNO3(aq) + H2O(l)  H3O+(aq) + NO3–(aq)

B. Solvation “Like Dissolves Like” NONPOLAR POLAR

B. Solvation Soap/Detergent polar “head” with long nonpolar “tail” dissolves nonpolar grease in polar water

C. Solubility UNSATURATED SOLUTION more solute dissolves no more solute dissolves SUPERSATURATED SOLUTION becomes unstable, crystals form concentration

C. Solubility Solubility maximum grams of solute that will dissolve in 100 g of solvent at a given temperature varies with temp based on a saturated solution

C. Solubility Solubility Curve shows the dependence of solubility on temperature

C. Solubility Solids are more soluble at... high temperatures. Gases are more soluble at... low temperatures & high pressures (Henry’s Law). EX: nitrogen narcosis, the “bends,” soda

Quiz 1. In a solution the substance that is being dissolved is called the___ a) Solvent b) Emulsifier c) Solute d) Filtrate 2. An emulsion is always between___ a) Two solids b) A solid and liquid c) Two gases d) Two liquids 3. What is one property of a suspension that is different from that of a solution or a colloid? a) If left to rest, the particles of a suspension will settle out. b) The particles of a suspension reflect light. c) A suspension is always clear d) Suspensions are colorless

Quiz 4. A What is the size of particles in a solution? a) More than 10,000 Angstroms b) Between 10,000 and 100,000 Angstroms c) Between 10 and 10,000 Angstroms d) Molecule size 5. A solution that cannot hold any more solute at room temperature is ___ a) A weak solution b) A concentrated solution c) A saturated solution d) A supersaturated solution

Quiz 6. An example of a colloid which is an emulsion is ___ a) Whipped cream b) Mayonnaise c) Fog d) Gelatin 7. An example of a solution is ___ a) Sugar and water b) Sand and water c) Milk d) Whipped Cream 8. Oil floats on water. The most accurate reason for this is a) oil is less dense than water b) oil is immiscible (does not dissolve) in water c) oil is both less dense and immiscible with water d) water is heavier than oil

Quiz 9. The best method to separate the solute from the solvent in a solution would be ___ a) Distillation b) Filtration c) Sedimentation d) all of the above will work 10. What makes water such a good solvent? a) Water is a good solvent because it is a negatively charged ion. b) Water is such a good solvent because it repels most molecules b) Water is such a good solvent because it is such a small molecule d) Water is a good solvent due to its polarity and small molecular size