Unit A Mix and Flow of Matter PDF

UNIT A: MIX AND FLOW OF MATTER WHIMIS AND LAB SAFETY Workplace Hazardous Material = WHMIS Information Systems What does WHMIS mean at school? - All chemicals stored in the school have a workplace label, and have an SDS or MSDS available. - Household products (e.g antacids, baking soda) s...

UNIT A: MIX AND FLOW OF MATTER WHIMIS AND LAB SAFETY Workplace Hazardous Material = WHMIS Information Systems What does WHMIS mean at school? - All chemicals stored in the school have a workplace label, and have an SDS or MSDS available. - Household products (e.g antacids, baking soda) should be stopped in their original containers. - Chemicals placed in smaller containers for student use are labelled. - Chemicals placed temporarily in a container should be labeled by whoever placed it there. What are my responsibilities as a student? - Read and follow all safety precautions - Found in lab instructions - Given by teacher (verbally, written, posted, etc.) - Included on the label - Know the WHMIS label - Ask questions when things are unclear - Notify the teacher immediately of any accidents or safety issues WHMIS PICTOGRAPHS Top Safety Rules Rule 1: Always read the lab procedure carefully before starting any activity. Rule 2: Know the location of science safety equipment Rule 3: Wear safety goggles and other protective equipment as directed in the lab Rule 4: Report lab accidents, broken equipment, and injuries to the teacher immediately. Rule 5: Never taste, touch, or smell a chemical unless specifically instructed to do so by the teacher. Rule 6: Dress appropriately for safety. Tie back long hair and do not wear loose clothing in the lab. Rule 7: Never eat or drink in the laboratory Rule 8: Never fool around in the laboratory Rule 9: Dispose of lab waste per the teacher’s instructions. Do not leave a mess for somebody else to clean up. PROPERTIES AND USES OF FLUIDS What is a fluid? - Substances with no fixed shape that flow from one place to another Includes substance in two states of matter: - Liquid - Gasses Note: Solids sometimes seem to flow (ex. Pouring salt or sugar) but they are actually just lots of small particles. - Don’t take the flow of the shape of the container Fluids make it easier to transport, process, and use a variety of materials, even if these materials begin as solids. Fluids are easy to move and they take the shape of the container they are in. - Solids we use today started off as fluids (plastic and metals) Fluids can be used as lubricants - Oil/grease that helps minimize friction Some fluids can be compressed - Use force in order to compress fluids to move things like in air tools - Called pneumatic (air) or hydraulic (water or oil system) Slurries: mixture of water (or other fluids) with a solid - Helps transport solids - Examples: paint, asphalt, plastics, and gas PURE SUBSTANCES AND MIXTURES Matters Matter - anything with mass that takes up space - Includes solids, liquids, and gases Two Categories - Pure Substances - Mixtures Pure Substances - All matter is made of particles - Contains all of the same particle Two Categories of Pure Substances: 1. Elements are pure substances that cannot be broken down into simpler substances by chemical means. - Example: hydrogen, nitrogen, carbon 2. Compounds are pure substances made up of two or more elements chemically together. - Example: water, co2, NaC1 Mixtures - Two or more substances combined together - Different particles that aren’t together - Separated into their distinct components Two Categories of Mixtures 1. Homogenous = latin for same - Looks like one substances, but contains two or more substances - Can be called solutions - Example: coffee, cement, glue 2. Heterogenous = latin for different - Easily able to see there are two or more substances in the substance - Not evenly distributed particles Three Categories of Heterogeneous 1. Mechanical Mixtures - All parts of mixtures are visible 2. Suspension - Cloudy mixtures (hazy substance) where residues of one substance are floating in another substance. *Substance will separate if left still - Example: blood, orange juice with pulp 3. Colloids  - Cloudy mixture (hazy substance) but residues are so small, therefore they do not separate easily. How to tell pure substances from solutions? Pure substances and solutions look very similar. One tool used to tell them apart is chromatography. Some of the substance is placed on a piece of paper, which is placed in a solvent like water. - If the substance is pure, it will all move up the paper at once - If it is a solution, different parts of it will travel at different speeds CONCENTRATION AND SOLUBILITY Solutions Solution is made from dissolving two substances together - Solute: substance that is dissolved (found in a less quantity) - Solvent: substance that dissolves a solute to form a solution - Water is often called the universal solvent because it dissolved so many materials Concentration Concentration tells you the amount of solute dissolved in a specific amount of solvent at a certain temperature. - Concentrated solution: large amounts of solute in the solvent - Dilute solution: small amount of solute in the solvent. Volume of solvent must be the same for both solutions. - Use equivalent ratios to help convert concentrations - Find a common denominator Example: 34 g of salt dissolved in 100 ml of water Or 100 g of salt in 1500 ml of water 34 x 15 — 100 x 15 = 510 —-- 1500 100 x 1 —---- 1500 x 1 510/1500 = 0.34 100/1500 = 0.66 Soluble vs Insoluble Soluble: able to dissolve in a particular solvent Insoluble: not able to dissolve in particular solvent Saturation - If a solution is saturated, no more solute will dissolve in a specific amount of solvent at a specific temperature. - No more solute dissolves because all of the solvent is already attracted to as much solute as it can be. - An unsaturated solution is a solution that contains more solute than would normally dissolve at a certain temperature. Solubility - Solubility is how concentrated a solution can become - Useful tool to compare how different solutes dissolve in a certain solvent. FACTORS AFFECTING SOLUBILITY Three Factors: 1. Type of Solute 2. Type of Solvent 3. Temperature Aqueous solution = solvent is water Temperature - Most common liquids and solids increase in solubility when the solvent temperature increases - In gases, the reverse is true: as temperature increases, the solubility of a gas in a liquid solvent decreases - Which is why warm pop is less fizzy than cold pop Thermal Pollution: Environmental Effect of Solubility Factor - Warm water (industrial processes) is poured directly back into the lake or river from which it is taken - Warmer water = less oxygen PARTICLE MODEL OF MATTER Spaces Heat Attraction Moving Everything Particles in Solid - Tightly packed together - Cannot move around freely - Lowest amount of kinetic energy Particles in Liquids - Slide around each other - Fill a container and take the shape of that container Particles in Gases - Enormous amount of empty space between them - Most kinetic energy - Fill the entire container they are in The Particle Model of Matter and Mixing - Particles of different substances are different sizes - Mixing two substances together, smaller particles are able to fit in between the larger ones The Particle Model Of Matter and Mixing - The solute particles are attracted more to the solvent particles than to itself - Mechanical mixture = one substance strongly attracted to itself than to the other Factors that Affect the Rate of Dissolving - Temperature - Pressure - Amount of stirring (agitation) - Surface area of solute accessible Stirring = particles will interact more Surface Area = solute particles are more exposed to being pulled away by solvent particles Temperature: movement of the solute/solvent particles Pressure = helps dissolves faster