Aqueous Solutions (When water is the solvent)

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1 Aqueous Solutions (When water is the solvent) Solvent= the dissolving medium (what the particles are put in ) Solute= dissolved portion (what we put in the solvent to make a solution) Because water is a polar molecule- the solute is most often: An ionic compound (NaCl) A polar covalent compound (NH 3, HCl) Like Dissolves Like

2 Water H 2 0 is foundation of ALL life on earth 75% of earth s surface comprised of water Water is often the reactant or product in bio-chemical reactions (metabolism)

3 Properties of Water O-H: Covalent Bond is highly polar Electronegativities give this molecule a slightly negative charge around the oxygen portion and positive charge around the hydrogen Hydrogen Bonding accounts for the characteristic properties we observe with water

4 Hydrogen Bonding Hydrogen covalently bonded to a highly electronegative atom such as oxygen, nitrogen or fluorine Hydrogen bonds are the strongest of the intermolecular forces

5 Properties of Water High Surface Tension Low Vapor Pressure High Specific Heat Capacity Many of these unique properties are a result of the hydrogen bonding in water High Heat of Vaporization High Boiling Point Solid phase is LESS dense than liquid phase

6 Surface Properties of H 2 0 High surface tension in water Surface tension= tendency of molecules to be drawn toward the interior of a liquid rather than the outer surfaces Surfactants reduce surface tension (detergents, grease etc.)

7 Low Vapor Pressure Hydrogen bonding holds these molecules so tight together, that water does NOT evaporate readily Vapor pressure is caused by increased kinetic energy that allows molecules to escape the surface of a liquid and enter gas phase

8 Specific Heat Capacity Specific heat of water- Q= 4.18 J (amount of energy needed to raise 1g of water 1 0 C) Compare to other substances such as: aluminum = 0.90 J iron = 0.44 J ethanol = 2.46 J Water absorbs large amounts of energy (heat/solar) Moderates weather

9 High Heat of Vaporization Hydrogen bonds must be broken before moving from liquid to vapor phase For water it takes 2.26 kj to convert 1g of liquid water (at C) to 1g of steam (at C) Same is true for condensation opposite of vaporization as 2.26 kj is released when 1g steam condenses to 1g of liquid Methane = 0.5 kj (Phase changes for water)

10 High Heat of Fusion (More phase changes for water- melting and freezing) Higher amounts of energy required to overcome strength of hydrogen bonds Energy is absorbed in melting, and released in freezing

11 Ice Yet another unique property of water- the fact that ice floats Ice has a hexagonal structure held in place by hydrogen bonds As ice melts the rigid framework collapses, water molecules are packed closer together in liquid form than solid form Water is most dense at 4 0 C. At 0 0 C, ice has a lower density. The resultice floats

12 Like dissolves Like What dissolves best in a given solvent Ions become surrounded by polar water molecules (hydrated) Polar molecules are attracted by polar portions of H 2 0 Nonpolar molecules associate with nonpolar solvents (not soluble in water) Water Column

13 Concentrations of Solutions Measure of the amount of solute dissolved in solution Dilute or concentrated: relative amounts of solute and solvent Percent- by mass or volume Molarity- used by chemists

14 Molarity= moles of solute per liter solution Moles of solute Liters of solution = molarity (M) When diluting a solution of known molarity- use the relationship: V 1 M 1 = V 2 M 2 Ex. You need to make a 3M solution of sulfuric acid that is 500mL from the concentrated 18M flask. How much of the 18M do you need to add to the water to make the 3M solution?

15 Solubility The amount of solute that will dissolve in a given amount of solvent (under specified conditions) Generally expressed as: grams of solute / 100g water Saturated Solution = Contains as much solute as will dissolve at that temperature Unsaturated Solution = Contains less solute than will dissolve at that temperature Supersaturated solution = Contains more solute than will dissolve at that temperature

16 The relationship between solubility and temperature can be expressed by a solubility curve. The solubility of most compounds increases as temperature increases, although exceptions do exist The solubility curves of several compounds are shown on the left. These curves reveal the maximum amount of solute that can be dissolved in 100 grams of water over a range of temperatures. Which salt is the most soluble at 20 O C? What is the solubility of K 2 Cr 2 O 7 at 70 O C?

17

18 Factors that affect Solubility: For Solids: Temperature- tend to more soluble at higher temperatures For Gases: Temperature- more soluble at lower temps Pressure- directly proportional to solubility

19 Solutions: Homogeneous Mixtures (Mixture that has the same composition and properties throughout) Solutions- particles can be separated only on the atomic or molecular level Suspensions- particles larger than atomic or molecular size (about 1000 times) Colloids- (colloidal suspensions) bridge the gap between solutions and suspensions Fog Hair spray Whipped cream Milk

20 Colloids & The Tyndall Effect: Colloids will scatter light. A beam of light or laser will be invisible in pure air or water, but once you have a colloid, the light is reflected off the many particles in the colloid suspension.

21 Electrolytes & Nonelectrolytes Electrolytes- compounds that will carry an electric current in aqueous solutions This occurs because some substances will dissociate into ions when dissolved in water solutions All ionic compounds are electrolytes as well as some very polar molecular compounds Most organic compounds are nonelectrolytes

22 Solutions: Liquids in Liquids Miscible= liquids which mix together in any proportion Immiscible= liquids which do not mix together (oil and water)

23 Rate of Solution: Rate at which the solute dissolves in the solution To increase the rate of solution- Increase the surface area of the solute Raise the temperature of the solvent Agitate the solution (stir)

24 Colligative Properties Use pgs to summarize what colligative properties are and some examples that illustrate how they work:

25 Colligative Properties Properties which depend only on the number of particles in solution (not on identity of the solute) Pure solvents have a specific vapor pressure at any given temperature A solution has a lower vapor pressure at the same temperature Colligative properties depend on vapor pressure The larger the number of particles in solution, the more the vapor pressure is lowered

26 Colligative Properties Boiling Point = the temperature at which the vapor pressure of the liquid is equal to the pressure above the liquid The vapor pressure of the solution is lower (at the same temp) than the vapor pressure of the pure solvent, so the solution will not boil at that temperature Boiling point elevation- the boiling point of the solution is higher than that of the pure solvent

27 Colligative Properties Freezing point = the temperature at which the vapor pressure of the liquid is equal to the vapor pressure of the solid Because the vapor pressure of the liquid solution is lower, it will be equal to the vapor pressure of the solid at a lower temperature Freezing point depression- the freezing point of the solution is lower than that of the pure solvent

28 Percent by Mass (usually for solid in liquid solutions) Mass of solute Mass of solution 100 = % mass For dilute solutions- the volume of solution is about the same as the mass of the solution (remember 1 ml water = 1g water

29 PPM= parts per million (used for reporting environmental conditions) Mass of solute Volume of solution 1,000,000 = ppm

30 Preparing a solution given the molarity: Ex) Prepare 175 ml of 0.25 M KCl 1.) Calculate the mass of the solute needed L 0.25 mol 74.6g = 3.3g KCl 1 L 1 mol KCl 2.) Describe how to prepare the solution- Mass 3.3 g KCl and dissolve in enough water to make 175 ml of solution

31 Molality (Use for calculations involving colligative properties) Molality = moles of solute per kg of solvent Moles of solute Kg solvent = molality (m)

32 Colligative Properties To find the actual amount of boiling point elevation or freezing point depression- t b = K b m t t f = K f m i t b and t f are the changes in boiling point and freezing point K b and K f are the molal boiling point constant and molal freezing point constant (they depend on the solvent) i = van t Hoff factor- it is the approximate number of moles of ions per mole of solute m = molality

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