1. 1 Solutions One substance dissolved in another substance

2. TEKS 10 (A) describe the unique role of water in chemical and biological systems; 10 (B) develop and use general rules regarding solubility through investigations with aqueous solutions; 10 (C) calculate the concentration of solutions in units of molarity; 10 (D) use molarity to calculate the dilutions of solutions; 10 (E) distinguish between types of solutions such as electrolytes and nonelectrolytes and unsaturated, saturated, and supersaturated solutions; 10 (F) investigate factors that influence solubilities and rates of dissolution such as temperature, agitation, and surface area; 2

3. 3 Solution is... A Homogenous... Mixture of two or more substances (evenly mixed) NaCl H2OH2OH2OH2O NOT It is a physical change …NOT a chemical change + Salt Water

4. 4 Solution All solutions consist of two parts: Solute Solvent

5. 5 Solute The substance being dissolved. The substance present in the least amount.

6. 6 Solvent The substance doing the dissolving. The substance present in the highest amount.

7. 7 Must a solution be a liquid?

8. 8 No… Air is a solution Sterling silver is a solution It can be gas It can be solid

9. 9 Types of Liquid Solutions Aqueous A solution with water as the solvent Tincture A solution with alcohol as the solvent.

10. 10 Insoluble When a substance cannot be dissolved in a solvent... Oil Water + = Therefore, oil is INSOLUBLE in water.

11. 11 Solubility A measure of how much a solute can be dissolved in a solvent under certain conditions

12. 12 Limits of Solubility Supersaturated Supersaturated …more solute than the solvent can handle. Saturated Saturated … the point that no more solute can be added to the solvent or it will be --- Unsaturated Unsaturated … more solute can be added to the solvent

13. What affects the rate of Solubility? Temperature Agitation Surface Area Pressure (For Gases) 13

14. 14 Solubility Graphs saturated Hold all that it can possible hold (at a given temperature) - concentrated Contain less solute than it can hold (at a given temperature) - Diluted More solute then it can hold (at a given temperature)

15. 15 Ionization The formation of ions by the action of a solvent in solution. NaCl (salt) in to Na + + Cl - in water Ions are formed (+ or -)

16. 16 Dissociation Is the process of separating ions during the formation of a solution … the more it dissociates, the stronger it is... Na + OH - Na + OH - Na + OH - Na + OH - Strong Base OH - NH 4 + Weak Base NaOH Na + + OH - OH - NH 4 + NH 3 H2OH2O H2OH2O NH 3 + H 2 O NH 4 + + OH -

17. 17 Solution Concentration Refers to the amount of solute dissolved in a solvent. Diluted (less) Concentrated (more) 5 grams of salt in 100 grams of Water Dilute VS. 35 grams of salt in 100 grams of water Concentrated 100 g. 5 g 35 g

18. 18

19. 19 Electrolytes Because dissolved salts have positive and negative ions, they are electrolyte solutions, and conduct electricity Na + Cl - Na + Cl - Na + Cl - Na + Cl - Na + Cl - Na +

20. 20 Effervescence The escape of a gas from a liquid solution

21. 21 Water

22. 22 Common Solvent Water is the most common substance on earth 70% of the earth’s surface 65% of your body mass