 A homogeneous mixture that contains a solvent and a solute(s).  PARTS OF A SOLUTION :  1) SOLVENT : The part of that is present in the largest amt; it dissolves the other substances.  2) SOLUTE : The part that is present in the smaller amt; it is dissolved by the solvent. Can have more than one solute!

 Solutions can be solid, liquid, or gaseous solid Brass and other alloys Dental fillings liquid Salt water coffee gas air gas in diving tanks

 Solutions that have water as their solvent are the most common solutions. They are said to be AQUEOUS solutions.  Because water can dissolve so many different solutes, it is called the universal solvent.

 COLLOID: mixture that contains small particles that DO NOT settle out but are large enough to scatter light TYNDALL EFFECT – the scattering of light –Pass light through mixture, if you see the light beam - it is a colloid. No light beam – it is a solution.

COLLOID SOLUTION

This is milk under a microscope. These are the fat particles in the milk.

The light from head lights is scattered by water particle in air.

SUSPENSION: a mixture in which the particles are easily seen and can be separated by settling or filtration.

SOLUTES : CO 2 gas flavoring coloring SOLVENT: water

 Solutes LOWER the freezing point and RAISE the boiling point of solvents

Concentration describes the amount of solute dissolved in a certain amount of solvent. Many times it is expressed as a percentage or a molarity (6 M or 1 M) Solutions can be described as being: 1) Dilute Or 2) Concentrated A 30% solution is more concentrated than a 10% solution. What does that mean?? Suppose the solute is sugar …. Explain!

 To make a solution MORE concentrated: 1) Add more solute 2) Remove some of the solvent To make a solution MORE DILUTE: Add more solvent

Properties of Acids:  Taste sour (lemons!)  React with metals & carbonates (corrosive)  Turns blue litmus paper to red (indicator) Common Acids: soda, vinegar, citrus juices

Properties of Bases:  Bitter taste  Feel slippery  Turn red litmus paper to blue Common bases: soap, shampoo, bleach, detergent

All acids begin with hydrogen! HNO 3 – nitric acid HCl – hydrochloric acid H 2 SO 4 – sulfuric acid HC 2 H 3 O 2 – acetic acid HF – hydrofluoric acid

Most bases end with hydroxide! NaOH KOH Ba(OH) 2 Al(OH) 3 Mg(OH) 2

Acids release H+ ions into the water when they dissolve. HCl  H+ + Cl- Bases release OH- ions into the water when they dissolve. NaOH  Na+ + OH-

The strength of acids & bases is measured using the pH scale. It describes the concentration of hydrogen ions in a solution This is why it is called pH! The more H+ ions in the water, the more acidic it is. The less H+ in the water the less acidic it is.

 The strength of an acid or base can be measured using the pH scale.  It ranges from 0 – 14  NEUTRAL = pH 7 = neither an acid nor a base  Below 7 = ACID Above 7 = BASE  The lower the pH the stronger the acid. The higher the pH the stronger the base.

 An reaction between and acid & base is called :  The products of a neutralization reaction are always water and a salt. HCl + NaOH  NaCl + H 2 O Since all acids begin with H and all bases end with OH they always form water!

H 2 CO 3 + KOH  K 2 CO 3 + H 2 O H 3 PO 4 + Ca(OH) 2  H 2 O + Ca 3 (PO 4 ) 2 Al(OH) 3 + H 2 S  Al 2 S 3 + H 2 O