1. SOLUTIONS A homogeneous mixture in which the components are uniformly intermingled

2. Terms Solvent – The substance present in the largest amount in a solution. The substance that does the dissolving. Solute – The other substance or substances in a solution. The substance that is dissolved.

3. ELECTROLYTES Substances that break up in water to produce ions. These ions can conduct electric current Examples: Acids, Bases and Salts (ionic compounds)

4. SOLUBILITY Is the amount of a substance that dissolves in 100 g of water at a given temperature to produce a saturated solution “Like dissolves Like” – Polar molecules dissolve polar molecules – Nonpolar molecules dissolve nonpolar molecules

5. SOLUBILITY RULES All common salts of Group I elements and ammonium are soluble All common acetates and nitrates are soluble All binary compounds of Group 7 (other than F) with metals are soluble except those of silver, mercury I and lead All sulfates are soluble except those of barium, strontium, calcium, silver, mercury I and lead Except for those in Rule 1, carbonates, hydroxides, oxides, sulfides and phosphates are insoluble

6. Terms Saturated – When a solution contains the maximum amount of solute Unsaturated – When a solvent can dissolve more solute Supersaturated – When the solution contains more solute than a saturated solution will hold at that temperature Concentrated – When a relatively large amount of solute is dissolved Dilute – When a relatively small amount of solute is dissolved

7. Factors Affecting the Rate of Dissolution Surface Area Stirring Temperature

8. Temperature vs Solubility

9. MOLARITY Molarity-the number of moles of solute per liters of solution M = molarity = moles of solute liter of solution

10. Calculate the molarity of a solution prepared by dissolving 11.5 g of NaOH in enough water to make a 1.50 L solution.

11. Calculate the molarity of a solution prepared by dissolving 1.56 g of HCl into enough water to make 26.8 ml of solution.

12. DILUTIONS M 1 x V 1 = M 2 x V 2 What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H 2 SO 4 What volume of 12 M HCl must be used to prepare 0.75 L of a 0.25 M HCl?

13. MASS PERCENT A unit of concentration equal to the mass of solute per mass of solution partx 100 whole

14. A solution is prepared by mixing 1.00 g of ethanol with 100.0 g of water. Calculate the mass percent of ethanol in this solution. A 135 g sample of seawater is evaporated to dryness, leaving 4.73 g of salt. Calculate the mass percent of salt in the saltwater.