1 - 1 © Chemeketa Community College: CH117 CH117 Chemistry in the Kitchen Unit 1: Measurements; Metric Units Phase Changes Water Solutions Polarity.

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Presentation transcript:

1 - 1 © Chemeketa Community College: CH117 CH117 Chemistry in the Kitchen Unit 1: Measurements; Metric Units Phase Changes Water Solutions Polarity

1 - 2 © Chemeketa Community College: CH117 MetricSICommonConversions Length Volume Mass Temperature Energy Units of Measurement meter (m) 1 m = 1.09 yd liter (L) 1 L = 1.06 qt gram (g) 1 kg = 2.2 lb Celsius ( o C) C = (F-32)/1.8 Kelvin (K) K = C + 273

1 - 3 © Chemeketa Community College: CH o 100 o Temperature

1 - 4 © Chemeketa Community College: CH117 MetricSICommonConversions Length Volume Mass Temperature Energy Units of Measurement meter (m) 1 m = 1.09 yd liter (L) 1 L = 1.06 qt gram (g) 1 kg = 2.2 lb Celsius ( o C) C = (F-32)/1.8 Kelvin (K) K = C calorie (cal) 1Kcal = 1000 cal = 1Cal Joule (J) 1 cal = 4.18 J

1 - 5 © Chemeketa Community College: CH117 Changes of State Melting Pt = Freezing Pt Boiling Pt Solid Liquid Vapor CondenseCondense FreezeFreeze MeltMelt VaporizeVaporize Slow, close, Fixed arrangement Moderate, close, Random arrangement Fast, far apart, Random Crystalline Amorphous

1 - 6 © Chemeketa Community College: CH117 Common Melting/Boiling Pts Freezing/ Melting Pt o C ( o F) Boiling Pt o C ( o F) Water100 (212)0 (32) Ethanol-114 (-173)78 (173) Salt801 (1474)1413 (2575) Sucrose Dec 186 (367) Canola Oil-10 (14) Smokes 204 (400) Olive Oil-6 (21) Smokes 190 (374) Peanut Oil3 (37) Smokes 232 (450) Coconut Oil25 (77) Smokes 177 (351) Lard41 (106) Smokes 188 (370)

1 - 7 © Chemeketa Community College: CH117 Common Melting/Boiling Pts Freezing/ Melting Pt o C ( o F) Boiling Pt o C ( o F) Water100 (212)0 (32) Ethanol-114 (-173)78 (173) Salt801 (1474)1413 (2575) Sucrose Dec 186 (367) Canola Oil-10 (14) Smokes 204 (400) Olive Oil-6 (21) Smokes 190 (374) Coconut Oil25 (77) Smokes 177 (351)

1 - 8 © Chemeketa Community College: CH117 Water Purification Desalination – remove salt Distillation – water boils at 100 o C; the impurity (salt) at 800 o C Water boils first – cools –condenses pure

1 - 9 © Chemeketa Community College: CH117 Water Purification Solar Still

© Chemeketa Community College: CH117 Solid Liquid Vapor Changes of State Frost DepositDeposit SublimeSublime Freeze Dry

© Chemeketa Community College: CH117 Temperature stays constant Temperature rises Heating Curve Temp constant Changes of State

© Chemeketa Community College: CH117 Temperature at Boiling Pt is Constant. Boiling Point Double Boiler: To melt chocolate or wax without burning.

© Chemeketa Community College: CH117 Temperature at Boiling Pt is Constant. Boiling Point Cooling for Nuclear Reactor: To generate energy without “meltdown”.

© Chemeketa Community College: CH117 We live at the bottom of an ocean of air Atmospheric Pressure Atmosphere: A sea of colorless, odorless gases surrounding the earth Boiling Point

© Chemeketa Community College: CH117 At higher elevations, there is less air so the P is less. Boiling Point Atmospheric Pressure

© Chemeketa Community College: CH117 Boiling Point = Boiling Point = Temp where molecule’s Vapor Pressure meets atmospheric Pressure Sea Level 760 torr Denver (5280’) 630 torr Mt. Evans,CO(14,000’) Mt. Everest(20,000’) 467 torr 270 torr H2OH2OH2OH2O = 100 o C = 95 o C = 87 o C = 73 o C If P goes down Boiling Pt goes down

© Chemeketa Community College: CH117 PT V If P goes up Boiling Pt goes up Boiling Point Pressure cookers Autoclaves

© Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Polarity (water vs ethanol) Solution Concentration Ethyl alcoholIsopropyl alcohol Mass = 46Mass = 60 Bp = 78 o CBp = 83 o C

© Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Polarity (water vs ethanol) Solution Concentration WaterEthyl alcohol Mass = 18Mass = 46 Bp = 100 o CBp = 78 o C

© Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Polarity (water vs ethanol) Solution Concentration

© Chemeketa Community College: CH117 Hydrogen Bonding of Water HH O ++++ ++++ ---- HH O ++++ ++++ ---- HH O ++++ ++++ ---- Hydrogen Bonds HH O ++++ ++++ ---- Polar Attraction Water beads, Water bends

© Chemeketa Community College: CH117 Hydrogen Bonding of Water Frozen H 2 O: Slow moving molecules H-Bond in patterns (Hexagonal Ring Crystals)

© Chemeketa Community College: CH117 Hydrogen Bonding of Water Hydrogen Bonds Causes Surface Tension Surfactants reduce Surface Tension by disrupting H-bonding (soaps, detergents etc.; make water “wetter”)

© Chemeketa Community College: CH117 Solutions Na + Cl - Na + Cl - Solvent Solvent : greater component in greater amount (The dissolver) Water Alcohol Solute Solute: lesser component in lesser amount (The dissolved) NaCl Sugar A solution A solution = A homogeneous mixture of components.

© Chemeketa Community College: CH117 Solutions Solid solutions Gelatin, Jelly 14K gold (58% Au ), Brass (Zn in Cu), Steel (C in Fe), Liquid solutions Gaseous solutions Air Air, Solid in Solid Liquid in SolidSoda, Vodka, Tea, Gas in Liquid Liquid in Liquid Solid in Liquid Gas in Gas

© Chemeketa Community College: CH117 Saturation Unsaturated: Can dissolve more. Saturated Have dissolved all possible Undissolved Solids in equilibrium w/ dissolved particles Undissolved Solids in equilibrium w/ dissolved particles

© Chemeketa Community College: CH117 Solutions Supersaturated: Temporarily dissolves more than normal at given Temp. Precipitate Excess solute that falls out of solution Ie. Rock Candy: On pipe cleaner: 7: Canadian guy: 14:35

© Chemeketa Community College: CH117 Solubility How much solute will dissolve in a solvent grams solute mls solution mls solution grams solute mls solution mls solution Factors affecting solubility PolarityPolarity TemperatureTemperature PressurePressure

© Chemeketa Community College: CH117 Polarity vs Solubility Like Dissolves Like NaClH 2 O NaCl dissolves in H 2 O C 6 H 14 But not in C 6 H 14 NaClH 2 O NaCl dissolves in H 2 O C 6 H 14 But not in C 6 H 14 OilC 6 H 14 Oil dissolves in C 6 H 14 H 2 O But not in H 2 O OilC 6 H 14 Oil dissolves in C 6 H 14 H 2 O But not in H 2 O Polar Attracts Polar Nonpolar Attracts Nonpolar

© Chemeketa Community College: CH117 Solubility “Like Dissolves Like” Polar water attracts to Polar particles Polar water attracts to Polar particles When polar solid dissolves in water, the polar solvent removes The particles from the crystal lattice.

© Chemeketa Community College: CH117 H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O -- ++ ++ H H O -- ++ ++ Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H - H O + H H O - + H - H O + H - H O + H - H O + H - H O + H - H O + H - H O + H - H O + H - H O + H - H O + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + Solubility

© Chemeketa Community College: CH117 H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + “Like Dissolves Like” Solubility

© Chemeketa Community College: CH117 Polarity vs Solubility Like Dissolves Like NaClH 2 O NaCl dissolves in H 2 O C 6 H 14 But not in C 6 H 14 NaClH 2 O NaCl dissolves in H 2 O C 6 H 14 But not in C 6 H 14 OilC 6 H 14 Oil dissolves in C 6 H 14 H 2 O But not in H 2 O OilC 6 H 14 Oil dissolves in C 6 H 14 H 2 O But not in H 2 O Polar Attracts Polar Nonpolar Attracts Nonpolar

© Chemeketa Community College: CH117 Temperature vs Solubility Solubility (g/100ml water) Temperature ( o C) GasGas NaCl

© Chemeketa Community College: CH117 Gases & most liquids less soluble when T increases Solids more soluble SolT T Sol Temperature vs Solubility

© Chemeketa Community College: CH117 solubility of a gas inversely temperature The solubility of a gas in a liquid is inversely related to the temperature. If T goes up Gas solubility goes down (gases escape) Temperature vs Solubility Gas Solubility TS T S T S

© Chemeketa Community College: CH117 Boiling Point Boiling points depend on Atmospheric Pressure Mass Polarity (water vs ethanol) Solution Concentration

© Chemeketa Community College: CH117 Boiling point elevation Adding solute raises the boiling point. 100 o C H 2 O Examples Cooking pasta or hard boiled eggs Making Fudge/Candy/Brittle Antifreeze More Solute  Higher Temp (Until solution is saturated) NaCl H 2 O More NaCl

© Chemeketa Community College: CH117 Adding solute lowers the freezing point. H2OH2O 0oC0oC NaCl H 2 O Freezing point depression Examples “Salting” roads in winter Making ice cream Frozen Juice concentrates More Solute  Lower Temp (Until solution is saturated)

© Chemeketa Community College: CH117 Liquid water: Held by Hydrogen bonds Solute particles interfere, causing the water molecules to slow down even more. This reduces the temperature.

© Chemeketa Community College: CH117 Hydrogen Bonding of Water Solute particles interfere, causing the hydrogen bonding To get disrupted and the ice to melt.

© Chemeketa Community College: CH117 Freezing Point Depression The more impurities the more unorganized so solution needs to be cooler to freeze solid. Mix of Sucrose, Glucose, Fructose resists stacking into crystals

© Chemeketa Community College: CH117 Crystals

© Chemeketa Community College: CH117

© Chemeketa Community College: CH117 Energy Energy Energy = The capacity to cause change Heat Light

© Chemeketa Community College: CH117 Temperature stays constant Temperature rises Heating Curve Temp constant Remember Changes of State Remember Changes of State Energy

© Chemeketa Community College: CH117 Potential Energy stored Energy Potential Energy = stored Energy (Has potential for motion) Kinetic Energy Energy in motion Kinetic Energy = Energy in motion (Fulfilling its potential) X Energy

© Chemeketa Community College: CH117 Energy calorie: E to raise 1 g H 2 0 by 1 o CE to raise 1 g H 2 0 by 1 o C H2OH2O 1 1 cal 1g 1 o C 1 1 cal 1g 1 o C Specific Heat 1oC1oC

© Chemeketa Community College: CH117 Energy Units of Energy = caloriecal kilocaloriekcal 1000 cal = 1 kcal CalorieCal Cal = kcal jouleJ 4.18 J = 1 cal British Thermal Unit BTU

© Chemeketa Community College: CH cal to melt ice g 1.00 cal to heat water g o C g o C 540 cal to vaporize g water g water Heat of Vaporization Specific Heat of H 2 O Heat of Fusion Heating Curve Energy

© Chemeketa Community College: CH117 E to raise Temp of 1g substance by 1 o C Fe0.11 Cu H 2 O 1.00 Ag Au Sand 0.19 Al 0.22 cal 1g 1 o C cal 1g 1 o C 0 o C = start Add 1 cal Specific Heat

© Chemeketa Community College: CH117 Specific Heat Fe0.11 Cu Ag Au Sand 0.19 Al o C = start H 2 O 1.00 E to raise Temp of 1g substance by 1 o C cal g o C cal g o C 1o1o 10 o 30 o 20 o Add 1 cal

© Chemeketa Community College: CH117 High SpHt; Resists change Specific Heat Fe0.11 Cu Ag Au Sand 0.19 Al 0.22 H 2 O o1o 10 o 30 o 20 o Low SpHt; Heats quickly

© Chemeketa Community College: CH117 Specific Heat 30 o C = start Energy gets given back with cooling 1o1o 10 o 30 o 20 oFe0.11 Cu H 2 O 1.00 Ag Au Sand 0.19 Al 0.22

© Chemeketa Community College: CH117 Specific Heat Fe0.11 Cu Ag Au Sand 0.19 Al 0.22 H 2 O 1.00 Energy gets given back with cooling cal g o C cal g o C 70 o 90 o 100 o 99 o 80 o 95 o High SpHt; Resists change Low SpHt; cools quickly

© Chemeketa Community College: CH117 Specific Heat Sand 0.19 H 2 O 1.00 Resists change Stays cold Heats quickly Gets hot Hydrated person Resists change in body temp Dehydrated person Body temp rises quickly & Lowers quickly