1. SOLUTIONS Unit 3

2. Solution It is a homogeneous mixture that is formed when a substance is dissolved in another substance.

3. Homogeneous VS. Heterogeneous Mixture A homogeneous mixture is a mixture where the components that make up the mixture are uniformly distributed throughout the mixture. Homogeneous mixtures: air, blood, saturated sugar water A heterogeneous mixture is a mixture where the components of the mixture are not uniform or have localized regions with different properties. Heterogeneous mixtures: rocks, oil and water, soup, pizza

4. Solute and Solvent Solute - The dissolved substance Solvent - The substance that dissolves

5. Characteristics Transparent and clear Homogeneous Solute does not separate from solvent when left to stand on its own No residue when filtered

6. Examples

7. Dilute, Concentrated, Saturated

8. Serial Dilution Method

9. Uses of Solute and Solvent 1. Name at least 5 uses for solute and 5 uses for solvent 2. Describe the importance of water as a solvent. 3. Is water a universal solvent? 4. Write in your Science notebook

10. Solutions DiluteConcentratedSaturated Has very little solute Has a lot of solute Has the maximum amount of solute in it Can dissolve a lot more solute Can dissolve a little bit more solute Cannot dissolve any more solute

11. Concentration of a solution A volume of solution is usually measured in cm³ or dm³ 1 dm³ = 1000 cm³ A concentration of a solution is measured in grams per dm³ (g/dm³). Example: a concentration of 10 g/dm³ means there are 10 g of solute in every 1000 cm³ of solution To prepare 10 g/dm³ of sodium chloride, you need to weigh 10 g of sodium chloride and dissolve it in 1000 cm³ of distilled water.

12. Test Yourself 1. Which are the solvent and solute when salt is added into water to make a salt solution? 2. To prepare 20 g/dm³ of NaCl, how much cm³ of solvent distilled water do you need?

13. Suspension & Colloid Characteristics SUSPENSION Heterogeneous mixture Insoluble solids obtained at the filter paper when filtered Pushed down to the bottom/does not dissolve COLLOID Light can reflect - Particles are large enough to reflect light - Are not affected by gravity (they usually not settle at the bottom) - Heterogeneous (but looks homogeneous)

14. Which One Has Scattered Light? SolutionColloid

15. DISSOLUTION Solubility gives us a measure of how much solute can dissolve in a solvent Solubility is the maximum amount of solute in grams that will dissolve in 100 g of solvent at a given temperature

16. SOLUBILITY A solvent can only dissolve a certain amount of solute. Solubility gives us a measure of how much solute can dissolve in a solvent. For example, the solubility of sodium chloride in a water at a temperature of 20ºC is 38 g per 100 g of water. This means that a maximum of 38 g of sodium chloride can dissolved in 100 g of water at 20ºC. The solution produced is a saturated solution.

17. LAB CHEMICALS Chemical NameFormulaUses & Other names sodium chlorideNaClTable salt / common salt dihydrogen monoxide H ₂O Water glucoseC6H12O6Carbohydrate / simple sugar potassium nitrateKNO3Potash, Food preservatives, fertilizers, gun powder

18. Factors Affecting Solubility Nature of Solvent Nature of Solute Temperature Pressure

19. NATURE OF SOLVENT The solubility of a solute varies in different solvent

20. NATURE OF SOLUTE Different solutes have different solubility in a given solvent.

21. PRESSURE For solid and liquid solutes, changes in pressure have no effect on the solubility. For gaseous solutes, an INCREASE in pressure increases the solubility and a DECREASE in pressure decreases the solubility.

22. PRESSURE AFFECTS GAS SOLUBILITY For gaseous solutes, an INCREASE in pressure increases the solubility and a DECREASE in pressure decreases the solubility.

23. RATE OF DISSOLUTION Temperature of the Solvent Rate of Stirring Size of the Solute Particles

24. TEMPERATURE OF THE SOLVENT The higher the temperature of the solvent, the faster the solute dissolves.

25. RATE OF STIRRING The faster the stirring is, the faster the solute will dissolve in the solvent.

26. SIZE OF THE SOLUTE PARTICLES The smaller the size of the solute particle is, the faster it dissolves in a solvent.

27. Difference between solubility and dissolution Dissolution is a kinetic process and is quantified by its rate. Solubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a solid, liquid, or gaseous solvent to form a homogeneous solution of the solute in the solvent.