UNIT A: THE MIX AND FLOW OF MATTER

1. UNIT A: THE MIX AND FLOW OF MATTER

2. OVERVIEW OF THE UNIT SECTION 1 • 1.1: WHMIS Symbols and Lab Safety • 1.2: The Many Uses of Fluids SECTION 2 • 2.1: The Particle Model of Matter (Mixtures and Pure Substances) • 2.2: Concentration and Solubility (Solutes and Solvents) • 2.3: Factors Affecting Solubility • 2.4: Particle Model of Matter SECTION 3 • 3.1: Viscosity and Effects of Temperature • 3.2: Density of Fluids • 3.3: Density, Temperature and Buoyancy SECTION 4 • 4.1: Technologies Based on Solubility • 4.2: Technologies Based on Flow Rates and Moving Fluids (Pumps and Valves) • 4.3: Designing a Model of a Fluid-Using Device (Submarines)

3. SECTION 1.1LAB SAFETY RULES • READ all written instructions before doing an activity. • LISTEN to all instructions and follow them carefully. • WEAR all required safety equipment such as goggles, gloves, an apron.**Remember to tie back long hair. • NEVER TASTE OR SMELL unknown substances because they could be very harmful to you. • THINK! If you think you shouldn’t be doing something, chances are you’re not supposed to be. When in doubt, ask me! Here is a little tip to remember the rules: (Randy Loves Wicked New Treats)

4. WHMIS AND LAB SAFETY Some materials we work with in the lab are hazardous. All hazardous materials have a label called a hazard symbol. The hazard symbol uses color and shape to indicate how hazardous the material is. A yellow triangle means caution, an orange diamond means warning and a red octagon means danger.

5. WHMIS WHMIS stands for: W H M I S • WHMIS contains 8 symbols, each separated into classes of potentially harmful materials that must be memorized because you may come in contact with them at home, work or school.

7. SECTION 1.2THE MANY USES OF FLUIDS A Fluid is anything that has no fixed shape and can flow. Common examples include water, soft drinks and detergents. Can you think of some more? • Fluids are useful because they can mix with other materials (Ex: Juice), they can change to solids (Ex: Glass) and they can move materials, even if they are solid. (Ex: River)

8. FLUIDS • Flow is the movement of a fluid. A fluid is usually a liquid or a gas because liquids and gases can easily flow or move. A solid has a fixed shape, making it nearly impossible to flow. • Ex: Water. When you pour water into a jug, it flows out. When you heat the water up on the stove, the water is released as steam, which flows into the air. But if you take a block of ice and try to make it flow, you won’t succeed.

9. Disorder Some space Particles closer together Order Particles fixed in position Total disorder Lots of empty space Gas Liquid Solid http://www.harcourtschool.com/activity/states_of_matter/index.html

10. SECTION 2.1MIXTURES AND PURE SUBSTANCES ALL ONE SUBSTANCE MORE THAN ONE SUBSTANCE

11. A • A pure substance: - is always homogeneous - has the same properties no matter where in the world it is found.

12. MIXTURES AND PURE SUBSTANCES • PURE SUBSTANCES are made up of 1 type of matter and have a unique set of characteristics or properties. For example, Aluminum foil, baking soda and water are all pure substances because you cannot separate them into other substances. Pure substances cannot be broken down! • MIXTURES http://www.correspondence.school.nz/departments/science/chemistry/web/home/chemistry/substances/mixtures.html

13. CLASSIFICATION OF MATTER

15. HETEROGENEOUS MIXTURES Heterogeneous Mixtures • When a heterogeneous mixture contains 2 or more visible substances, it is also known as a Mechanical Mixture. Can you think of any more examples?

16. A mechanical mixture • When materials are mixed together but we can still see the different parts we call it a mechanical mixture

17. Heterogeneous Mixtures Suspensions • A suspension is a heterogeneous mixture where droplets or pieces of one substance are held within another substance. Suspensions are usually cloudy (like muddy water or coffee) because you can actually see both substances, even though they are mixed. If you leave a suspension undisturbed, it will usually settle into separate parts. MUD + WATER = SUSPENSION

18. HETEROGENEOUS MIXTURES Colloids • A colloid is a heterogeneous mixture made up of tiny particles. Colloids are usually cloudy like suspensions, but because the particles are so small you cannot see the separate parts of the mixture and it cannot easily separated out. Some examples of colloids are hair gel, clouds and creamy milk.

19. HOMOGENEOUS MIXTURES Homogeneous Mixtures • Homogeneous mixtures are also known as Solutions because one substance is dissolved in the other. • Sometimes it is hard to tell the difference between solutions and pure substances so tests like boiling point and melting point are used.

20. Some examples of common solutions: Solid solution: Gas solution: Liquid solution: The Matter Bop

21. SECTION 2.2CONCENTRATION AND SOLUBILITY Forming a solution by mixing 2 or more materials together is called Dissolving Solute

22. Concentration and Solubility Solvent SOLUTE + SOLVENT =

23. Concentration and Solubility Depending on the solution, the amount of solvent and solute will be different. A concentrated solution has a larger amount of solute in a solvent. A diluted solution has a small amount of solute in a solvent. For example: if you’re making juice and put too much juice crystals in the juice will be too sweet (concentrated). But if you add more water to the juice, it will become less sweet (diluted).

24. Concentration and Solubility DILUTED (LESS SOLUTE, MORE SOLVENT) CONCENTRATED (MORE SOLUTE, LESS SOLVENT)

25. Measuring Concentration The Concentration of a solution is the actual amount of solute dissolved in a specific amount of solvent. • For example: 50g of solute dissolved in 100mL of water has a concentration of 50g/100mL of water. The amount of solute is measured in grams and it is always the first number. The amount of solvent is measured in milliliters and is always the last number. • Example: Solution ASolution B 10 g solute 25 g solute 50 mL solvent 100 mL solvent How do you write this in proper concentration format?

26. Comparing Concentrations • To compare concentrations, you need the same amount of solvent. • Example: Solution A 10 g solute/50 mL solvent Solution B 25 g solute/100mL solvent Which solution is more concentrated? • Step 1: Make the amount of solvent equal! change Solution A 50mL100mL  50ml x 2 = 100mL • Step 2: Whatever you do to the solvent, you must do to the solute! take 10g x 2 = 20g • Re-write concentrations per 100mL! Solution A 20g/100mL Solution B 25g/100mL

27. SATURATED VS. UNSATURATED SOLUTIONS • The limit to how much a solution can be concentrated is called solubility, which is the maximum amount of solute that can be dissolved in a fixed amount of solvent at a certain temperature. • If you take a frozen can of juice and mix it with a jug of water, the water would dissolve the frozen juice to make a solution. But if you put 2 cans of frozen juice in the same size of jug, what would happen?

28. SATURATED VS.UNSATURATED SOLUTIONS • If you have a solution where more solute can be dissolved, the solution is known as unsaturated. • If you have a solution where no more solute can be dissolved, the solution is known as saturated. Every solution has a saturation point—a point where the maximum amount of solute is dissolved at a given temperature. • Ex: When you put Kool-Aid in a jug of water, the Kool-Aid will dissolve, so the solution is unsaturated and you can add more Kool-Aid. If you put even more in to the point where no more Kool-Aid can be dissolved or added, the juice will be saturated.

29. SECTION 2.3FACTORS AFFECTING SOLUBILITY • Solubility depends on 3 main factors: • The most common solvent is water. Anytime you read the term aqueous solution on a product, it means water is the solvent. • But Remember: solutions do not have to always be made up of liquids

30. FACTORS AFFECTING SOLUBILITY Here are some examples:

31. Solubility Changes With Temperature • Solubility increases as the temperature of the solvent increases, because more space is provided between the particles for the solute particles to fit (dissolve) into. The reverse is true for a gas though - as the temperature increases, the solubility of a gas, in a liquid solvent decreases.

32. Thermal Pollution • This decrease in the solubility of gases can have a serious effect on the environment. If the temperature of water increases (warm industrial waste water poured directly into lakes and rivers) then there is less oxygen that can be dissolved in the water – thus, affecting the living organisms in the water. This is called thermal pollution.

33. Changes of state – heating curve gas boiling  condensing liquid  gas liquid melting  freezing solid  liquid solid temperature time

34. Changes of state – cooling curve activity

35. Changes of state activity

36. The Particle Model of Matter TIME FOR A SONG

37. Factors Affecting The Rate Of Dissolving • The speed at which the solute dissolves in a solvent is called the rate of dissolvingand can be affected by:

38. SECTION 3VISCOSITY AND THE EFFECTS OF TEMPERATURE • One property that all fluids have is their ability to flow • How quickly fluids flow is called Viscosity. • Viscosity is determined by • Fluids with a high viscosity do not flow easily, but fluids with a low viscosity flow easy

39. SECTION 3.1TEMPERATURE AND VISCOSITY • A fluid’s viscosity depends on its amount of internal resistance or friction. • As the temperature of a liquid increases, its viscosity decreases. The opposite is also true. As the temperature of a liquid decreases, the viscosity increases. This can be explained using the Particle Model:

40. SECTION 3.1TEMPERATURE AND VISCOSITY • A liquid is made of particles that roll and slide over each other. When energy or heat is added, the particles move around more quickly ( less viscous; moves faster). But when the temperature drops, the particles slow down (more viscous; moves slower).

41. SECTION 3.2DENSITY • Density of Fluids • Densityis the amount of matter in a given volume. Every substance has a different density, because each substance is made up of different particles. The density of a substance depends on the particles it is made up of. When we talk about density, it's usually mass density we're referring to. The mass density of an object is simply its mass divided by its volume.

42. SECTION 3.2DENSITY • Density depends on whether the object is solid, filled with air pockets, or something in between. Substances that have a higher density than the density of the substance it is placed in will sink; substances that have a lower density than the density of the substance it is placed in will float.

43. SECTION 3.2CALCULATING DENSITY • Calculating Density • Density is the mass of a substance divided by its volume, which changes as temperature changes. • This is shown in the following equation form: • ** Density is measured in units of g/mL for liquids and g/cm cubed.

44. SECTION 3.3DENSITY, TEMPERATURE AND BUOYANCY • Changing Density • Can we can the density of a substance? The answer is yes. We can change the density of a substance by changing its concentration or by changing the temperature of a substance.

45. SECTION 3.3DENSITY, TEMPERATURE AND BUOYANCY • A fluids density may be changed by altering its concentration. A solution with a higher concentration will have greater density than one with a lower concentration. For example in a fresh water lake you would find it more difficult to float in than the Dead Sea, which has a high salt content. You can float more easily because the water has more particles per unit, thus is more dense.

46. SECTION 3.3DENSITY, TEMPERATURE AND BUOYANCY • By changing the temperature you can alter a substances density. When a substance is cooled the particles move closer together. This results in more particles in a given area, thus, an increased density. When particles are heated they move further apart. This results in fewer particles in a given area, thus, lower density.

47. BUOYANCY Buoyancy works on the principles of gravity and buoyant force.

48. SECTION 3.4COMPRESSION OF FLUIDS • Different fluids have different compressibility, which is the ability of a substance (solid, liquid or gas) to be compressed, or squeezed. For example you can compress air a lot more than you can compress water. This is because gases have greater room between the particles than fluids. Thus, by using force we can push gas particles closer together more easily than fluid particles.

49. SECTION 3.5 PRESSURE IN FLUIDS • Pressure is the amount of force applied on an area. • To calculate pressure we use the following formula: • The units are in kilopascals or N/cm

50. SECTION 3.5 PRESSURE IN FLUIDS • Depth and Pressure • The force of a fluid on a container is equal on all sides at equal depth. However, the pressure increases at greater depth. This is why hydroelectric damns water intake is from the bottom of the damn not the top. • When a container is enclosed, however, the pressure that is exerted is equal in all directions. This is known as Pascal’s Law.