Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a...
-
Upload
bryan-turner -
Category
Documents
-
view
221 -
download
0
Transcript of Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a...
![Page 1: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/1.jpg)
Chapter 13
Water and Its Solutions
![Page 2: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/2.jpg)
Objectives
• 13.1 Demonstrate the uniqueness of water as a chemical substance
• 13.1 Model the three dimensional geometry of a water molecule
• 13.1 Relate the physical properties of water to the molecular model
![Page 3: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/3.jpg)
Objectives
• 13.2 Compare and contrast the ability of water to dissolve ionic and covalent compounds
• 13.2 Distinguish solutions from colloids • 13.2 Compare and contrast colligative
properties• 13.2 Calculate concentrations
![Page 4: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/4.jpg)
Water
• What makes water unique– All three states of matter exist in large quantities
on earth– For its size, it has the highest melting point and
boiling point (all other molecules of similar size boil much sooner)
– It is one of few molecules which is more dense as a liquid than solid
• Most dense at 4 C
– Large specific heat
![Page 5: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/5.jpg)
Freezing and Boiling Explained
• Water is very polar – Oxygen 2nd most
electronegative• The hydrogen atom is
an exposed proton, very attracted to other oxygen lone pairs– Why water is an acid as
well (explained later)
![Page 6: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/6.jpg)
Hydrogen Bonding
• Occurs when Hydrogen is bound to an Oxygen or Flourine, and partially in Nitrogen
• These three (NOF) are able to expose the nucleus of the hydrogen, making it very positive and highly (electromagnetically) attractive towards other molecules
![Page 7: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/7.jpg)
![Page 8: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/8.jpg)
Surface Tension
• Results from imbalanced forces
• Interior molecules = Pulled in every direction
• Exterior molecules = Pulled down (but not up
![Page 9: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/9.jpg)
![Page 10: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/10.jpg)
Capillary
• The attraction of the molecule to the tube – Water (Blood)
likes glass more than itself, pulls itself up
– Mercury doesn’t, so it wouldn’t climb
![Page 11: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/11.jpg)
Universal Solvent
• Water dissolves almost anything (in tiny amounts)
• Very difficult to have “pure” water because it dissolves almost anything– Hard to get clean water to people, since water
dissolves in tiny quantities the pipes
![Page 12: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/12.jpg)
Rules of Solubility
• Likes dissolve likes– Polar dissolves Polar– Non-Polar dissolves Non-Polar
• Water = Polar, will dissolve anything with a charge – As long as charge isn’t too strong for water to pull
apart– Many salts and almost all sugars are soluble in
water
![Page 13: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/13.jpg)
Water (polar) dissolves other polars
![Page 14: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/14.jpg)
Sugar
![Page 15: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/15.jpg)
Quick Vocab
• Solution: Homogenous mixture • Solute: What is being dissolved• Solvent: What is doing the dissolving• Solubility: How much of a substance can
dissolve under said conditions• Saturated: A solution which can’t dissolve any
more (Has as much as possible): Opposite- un• Supersaturated: More than normally allowed
![Page 16: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/16.jpg)
Concentrated and Dilute
• Very vague terms• Concentrated: Associated with lots of solute• Dilute: Associated with minimal solute
![Page 17: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/17.jpg)
Solubility
• For most salts, as temperature goes up, solubility goes up
• Sugar changes solubility a lot as well
![Page 18: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/18.jpg)
Colligative Properties• When a pure solvent has another
element/substance dissolved into it (mixed in), the properties of the initial solvent changes.– This change is called colligative
properties
![Page 19: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/19.jpg)
Colligative Properties• Include
– Freezing Point Depression (lower Fp)– Boiling Point Elevation (higher Bp)– Lower Vapor Pressure above solvent– Change in Osmotic Pressure
![Page 20: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/20.jpg)
Colligative Properties• Does NOT depend on the type of
molecule dissolved• Depends on the quantity of
molecules dissolved
![Page 21: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/21.jpg)
Colligative Properties• In order of effect per mol in water
– 1 Mol of Na3PO4 4 Ions Largest – 1 Mol of Na2SO4 3 Ions – 1 Mol of NaCl 2 Ions– 1 Mol of Sugar 1 Molecule
• For roads, place salts which dissociate into many ions
![Page 22: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/22.jpg)
Vapor Pressure Explained
• There are less particles of solvent per Liter of solution, so the pressure from the solvent is decreased
• The amount of solute particles is directly proportional to the elevation and depression.
![Page 23: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/23.jpg)
![Page 24: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/24.jpg)
Colloid• A mixture, but with large particles
present suspended by charge– Note: In order to be a true solution, the
solute and solvent must have diameters of less than 1nm (1nanometer, or 1E-9m). Colloids have particles in the range of 1-1000nm
• One Å = 0.1 nanometer (Water has a diameter of 1.5 Å, so 0.15 nanometers).
• Examples include: Milk, Fog• Tyndall Effect: Scatter Light
![Page 25: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/25.jpg)
• Blue = Water
• Yellow = Milk
![Page 26: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/26.jpg)
SolutionsSolutions
Concentrations
![Page 27: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/27.jpg)
Major Ideas• Expressing Concentration in a
variety of ways, including:• Molarity (M)• PPM (Parts per million)• Mass %
– Mol Fraction – Molality (m)
![Page 28: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/28.jpg)
PPM• Often we hear the terms parts per
million and parts per billion in discussion of pollution and such.
• What does this mean? It is the number of grams of solute per million grams of solution (or billion if parts per billion)
![Page 29: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/29.jpg)
How Safe is your water?
• Some standards for your drinking water (from EPA) (Maximum allowable levels)
• Arsenic 10ppb• Perchlorate 4ppb• Flouride 4ppm• Lead/Copper 1.3ppm
![Page 30: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/30.jpg)
Calculating PPM• Advantage of using this method:
Useful for very small concentrations
ppXgSolution
gSolute#
![Page 31: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/31.jpg)
Quick Question• Working for the EPA, you find
0.002g of Lead dissolved into 500.0 g of water. Is the water meeting the EPA standards for safety?– EPA = 1.3 ppm is allowable
![Page 32: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/32.jpg)
Molarity• Describes how many mols of
solute are in each liter of solution.• Molarity = Mols / Liter of Solution
SolutionLiters
Solutemols
_
_
![Page 33: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/33.jpg)
Molarity• 3 mols of KBr dissolved into a 0.4
L solution is 0.75 Molar (molar = molarity)
• Usefulness: Stoichiometric Calc’s
MKBrLsolution
molsKBr75.0
4.0
3.0
![Page 34: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/34.jpg)
Review (and new)• Be careful when working with
solutions in which the solute dissociates (aqueous).
• A 1.0 Molar solution of CaCl2 is 1.0 Molar Calcium and 2.0 Molar Chloride
![Page 35: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/35.jpg)
Questions• Determine the molarity of the
following ions. • Li+ and NO3
- in a 0.0385 M LiNO3
• Ca+2 and Cl- in a 0.035 M CaCl2• Aluminum and Sulfate in a 0.0112
M solution of Al2(SO4)3
![Page 36: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/36.jpg)
Questions• A 3.2 Liter solution has 83grams of
Sodium Nitride (Na3N). What is the molarity of Sodium and Nitride in the solution?
![Page 37: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/37.jpg)
Mass %• Used for many solutions you
purchasemass of A in solutiontotal mass of solutionMass % of A
= 100
![Page 38: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/38.jpg)
Quick Question• 5 grams of acetic acid is dissolved
into 100 grams of Water. What is the mass percent of the solution?
• Your toothpaste is 0.15% flouride. If the tube has 80 grams of toothpaste, how much flouride are you buying?
![Page 39: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/39.jpg)
Mol Fraction (Don’t need to know)
• Way of describing what % by amount of mols instead of mass
moles of Atotal moles in solution
XA =
![Page 40: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/40.jpg)
Molality (Don’t need to know)
• Similar to Molarity, however, instead of Volume mass of solution (in kilograms)
• Useful for when temperature changes
mol of solutekg of solvent
m =
![Page 41: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/41.jpg)
Question Check• 2.0 mols of Hydrogen Peroxide
(HOOH) is dissolved into 480grams of water. The volume of the solution 500 mL. What is the concentration of the solution in
• A) Molarity B) Mass%• C) PPM
![Page 42: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/42.jpg)
Salinity (Don’t need to know)
• A common method for expressing the amount of salt dissolved into the ocean
• Salinity: Grams of Salt (all ions) per 1000 g of solution. The average salinity of ocean water is 35 (35 g of dissolved salt ions per 1000 g of solution).
![Page 43: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/43.jpg)
Salinity (Don’t need to know)
• The salinity of Sodium in the ocean is 10.8 and Chlorine is 19.4. – For every 1000 grams of ocean
water, 10.8 grams of that is Sodium in its cation form
![Page 44: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/44.jpg)
SolutionsSolutions
Dilutions
![Page 45: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/45.jpg)
Question• 200 grams of Potassium Oxide is
dissolved into 870 grams of water and has a volume of 1.0 Liters.
• What is the • A) Molarity B) Mass % C) PPM
![Page 46: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/46.jpg)
Diluting Solutions• Often times you will need to dilute
a more concentrated solution to a less concentrated solution. This can be done by using the equation:
• M1V1=M2V2 • Where M is Molarity and V is
Volume
![Page 47: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/47.jpg)
Question• Example: A chemist has 2.0 L of
6.0 Molar (M) HCl (aq). • How much water will be needed to
dilute the solution to 1.0 M HCl (aq)?
![Page 48: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/48.jpg)
Follow Up• Analysis• M1 = 6.0 M, V1 = 2.0 L, M2 = 1.0 M
(6)(2)= (1)(x)• The final volume is 12 L. However
you need to add 10 L of water (otherwise you will have a new volume of 14 L).
![Page 49: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/49.jpg)
Which way do you go?• Always Add Acid to water. • If you add the water to the acid,
the water will be in a very small concentration, and the heat of the reaction can cause the water to boil and splatter. This splattering might have the acid with it.
![Page 50: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/50.jpg)
Which Way Then• The proper way to dilute the
solution is by adding the 2.0 L of 6.0 M to 10.0 L of water.
![Page 51: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/51.jpg)
Questions• Question: A chemist has 40 mL of
12.0 M HCl (aq). How much water will be needed to dilute the solution to 0.5 M HCl (aq)?
![Page 52: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/52.jpg)
Questions• Question: A teacher needs to
make 500 mL of 2.0 M HCl for his class. The teacher has 12.0 M HCl (aq) and water. How much of each should the teacher put together to make a 500 mL 2.0 M HCl solution?
![Page 53: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/53.jpg)
Solubility Rules• In General, what dissolves and
what doesn’t in large quantities in a water solution
![Page 54: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/54.jpg)
Rules of Solubility• Likes dissolve likes Polar
Compounds dissolve other polar compounds
• Non-polar compounds dissolve other non-polar compounds
![Page 55: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/55.jpg)
Solubility Rules• Vitamin B,C = Polar molecules,
dissolve into water
• Vitamin C
![Page 56: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/56.jpg)
Solubility Rules• Vitamin C deficiency happens
quickly. Our body doesn’t store Vitamin C in an appreciable amount because it is water soluble.
• It is very hard to overdose on Vitamin C because our Kidney’s can regulate it out.
![Page 57: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/57.jpg)
Solubility Rules• Vitamin A, D, E = Non-polar
molecules, dissolved into fat (non-polar hydrocarbon chains)
![Page 58: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/58.jpg)
![Page 59: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/59.jpg)
Gases and Solubility
– There is very little attraction between gases and liquid solvents. Temperature and Pressure will dictate how much gas will be dissolved.
• Temperature Increasing temperature decreases solubility
![Page 60: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/60.jpg)
Gases: Temperature• This is because the liquid
molecules move more and the gas can sneak its way to the top.
• When Pop gets warm, it doesn’t taste as sharp, carbon dioxide escapes.
![Page 61: Chapter 13 Water and Its Solutions. Objectives 13.1 Demonstrate the uniqueness of water as a chemical substance 13.1 Model the three dimensional geometry.](https://reader036.fdocuments.us/reader036/viewer/2022062308/56649e755503460f94b763f8/html5/thumbnails/61.jpg)
Gases: Pressure• Pressure Increasing pressure
increases solubility of gases– The gas is forced into the water
under high pressure.– When you open a can of pop, the
pressure decreases and the gas molecules can escape