What is a solution? 22.1
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2 22.1 How Solutions Form What is a solution? Solution= homogeneous mixture- same composition throughout Can be: liquids, gases and even solids Worlds Largest= Ocean Solute: is dissolved Solvent: does dissolving Solid dissolving in a liquid: Solid = solute, liquid= solvent.
3 22.1 How Solutions Form Nonliquid Solutions All gas/gas mixtures are solutions. Ex: Air Alloy: Solid/solid solution; metals melted together. Ex: Sterling silver= Ag + Cu Brass= Cu + Zn Steel= Fe + C
4 22.1 How Solutions Form Nonliquid Solutions Solid/liquid- solid is the solvent Ex: dental amalgam Liquid Solvent + Gas = Soda Pop Carbon dioxide in water Liquid= vinegar Solid= salt water
5 22.1 How Solutions Form How It Happens (Solid in a Liquid) Step 1. Moving liquid particles surround and collide with surface of solid Step 2. Liquid particles pull the solid particles into solution.
6 22.1 How Solutions Form How It Happens Step 3. Liquid and solid particles spread out to form a homogeneous (even) mixture.
7 22.1 How Solutions Form Dissolving Liquids and Gases Particles of liquids and gases move much more than solids. In gas/gas or liquid/liquid solutions, particle movement spreads solutes evenly throughout the solvent.
8 22.1 To increase rate (how fast) of dissolving: Increase collisions btwn solute/solvent by: Stirring How Solutions Form Rate of Dissolving Increase surface area (smaller particles) Increase temperature
9 22.1 Rate of Dissolving To increase dissolving of gases: Increase Pressure How Solutions Form Decrease Temperature
10 22.1 Section Check Question 1 A mixture that has the same composition, color, and density throughout is a. A. solvent B. solute C. solution D. substance
11 22.1 Section Check Answer The answer is C. A mixture that has the same composition, color, and density throughout is a solution.
12 22.1 Section Check Question 2 The substance being dissolved in a solution is the. A. aqueous phase B. media C. solute D. solvent
13 22.1 Section Check Answer The answer is C. The substance doing the dissolving is the solvent; the substance being dissolved is the solute.
14 22.2 Solubility and Concentration How much can dissolve? Solubility: amount able to dissolve at specific temperature depends on the nature of the substances If temp. is the same, B is more soluble than A.
15 22.2 Solubility and Concentration How much can dissolve? Solubility is expressed as max # grams of substance dissolved at a certain temp. 20 o C: Li 2 CO g/ 100 ml H 2 O Sugar g/100 ml H 2 O
16 22.2 Solubility and Concentration Concentration Concentrated= large amount solute in solvent. Dilute: small amount of solute in solvent Precise way to describe concentration= % by volume of solute
17 22.2 Solubility and Concentration Types of Solutions Saturated: solution contains all the solute it can hold Unsaturated: solution that can dissolve more solute Supersaturated: solution contains more solute
18 22.2 Solubility and Concentration Supersaturated Solutions Supersaturated solutions are unstable. Created by slowing cooling a saturated soln.
19 22.2 Saturated Solutions Generally, as liquid solvent temp. increases, amount of solid solute that can dissolve increases. Solubility and Concentration
20 22.2 Solubility and Concentration Solubility Curves
21 22.2 Solubility and Concentration Solubility of Gases Shaking or pouring causes gas to come out of the solution. More gas molecules exposed to the surface, where they escape from the liquid.
22 22.2 Solubility and Concentration Pressure Effects Soft drinks are under increased pressure. Increased Pressure= increased gas solubility When pressure is released, the carbon dioxide bubbles out (solubility decreases)
23 22.2 Solubility and Concentration Temperature Effects Cooling a liquid solvent increases gas solubility. Particles slow down and can t escape as easily.
24 22.2 Section Check Question 1 What is solubility? Answer Solubility is the maximum amount of a solute that can be dissolved in a given amount of solvent at a given temperature.
25 22.2 Section Check Question 2 A(n) solution is any solution that can dissolve more solute at a given temperature. A. electrolyte B. saturated C. supersaturated D. unsaturated
26 22.2 Section Check Answer The answer is D. A saturated solution contains all the solute it can hold at that temperature, but an unsaturated solution can hold additional solute.
27 22.2 Section Check Question 3 Which is true of a supersaturated solution? A. conducts electricity in water B. can dissolve more solute at a given temperature C. cannot form crystals when additional solute is added D. unstable
28 22.2 Section Check Answer The answer is D. Supersaturated solutions are unstable; solute readily crystallizes from solution when seed crystals are added.
29 22.2 Section Check Question 4 Which of these factors does not affect solubility? A. container size B. crystal size C. surface area D. temperature
30 22.2 Section Check Answer The answer is A. Speeding up movement of the particles by stirring and increasing the temperature, and decreasing the crystal size all increase the dissolving rate of a solute.
31 22.3 Particles in Solution Particles in Solution Like Dissolves Like Polar solvents dissolve polar solutes Nonpolar dissolves nonpolar Water (polar) and oil (nonpolar) don t mix
32 Particles in Solution 22.3 Particles with a Charge Electrolytes: Compounds that produce solutions of ions that conduct electricity To form ions, molecules must be broken apart Ionization: process of forming ions Ex: HCl in H 2 O
33 22.3 Ionization Particles in Solution Water pulls polar molecules apart and forms ions.
34 22.3 Dissociation Particles in Solution Dissociation: ionic solid separates into ions Ex: NaCl in H 2 O Water s polar ends attract oppositely charge ionic solid ends and separates them
35 22.3 Particles in Solution Particles with a Charge Nonelectrolytes: form no ions in water and cannot conduct electricity Ex: Sugar (sucrose)
36 22.3 Particles in Solution Effects of Solute Particles All solute particles affect properties of the solvent- freezing point and boiling point. Depends on # solute particles in soln.
37 22.3 Particles in Solution Lowering Freezing Point Adding a solute lowers the freezing point of the solvent. Ex: antifreeze
38 22.3 Particles in Solution Lowering Freezing Point Solute particles interfere with solid pattern formation, making it harder for the solvent to freeze.
39 22.3 Car Radiators Particles in Solution Adding solute particles raises boiling point. Particles of solute take up space on the surface Fewer water molecules can reach the surface and evaporate
40 22.3 Section Check Question 1 Compounds that produce solutions of charged particles that can conduct electricity in water are known as. A. electrolytes B. ions C. nonelectrolytes D. solvents
41 22.3 Section Check Answer The answer is A. Some electrolytes conduct a strong current. Ions are charged particles.
42 22.3 Section Check Question 2 What effect does the addition of solute particles have on the boiling point of a solution?
43 22.3 Section Check Answer Adding solute particles raises the boiling point of a solution, because the solute particles interfere with the evaporation of solvent particles.
44 22.3 Section Check Question 3 is the process in which an ionic solid separates into its positive and negative ions. A. decomposition B. dissociation C. electrolysis D. ionization
45 22.3 Section Check Answer The answer is B. Ions already exist in the solid compound and are attracted into solution by surrounding polar water molecules.
46 22.4 Dissolving Without Water When Water Won t Work Water is polar- can dissolve polar substances However, nonpolar materials have no separated positive and negative areas. Nonpolar materials do not dissolve in water except to a small extent, if at all. Water and oil don t mix
47 22.4 Dissolving Without Water Versatile Alcohol Alcohols- both polar and nonpolar ends Can dissolve both types of solvents Ex: ethanol
48 22.4 Dissolving Without Water Useful Nonpolar Solvents Mineral oil removes: candle wax, bubble gum, oil-based paint Turpentine removes: oil- based paint Dry Cleaners
49 22.4 Toxic Dissolving Without Water Nonpolar Solvent Drawbacks Flammable Need good ventilation due to high evaporation- can lead to dangerous vapor levels in air
50 22.4 Dissolving Without Water How Soap Works Soaps: salts of fatty acids hydrocarbon molecules w/ carboxylic acid group COOH Acid group= polar Dissolves in water Hydrocarbon= nonpolar Dissolves oily dirt
51 22.4 Dissolving Without Water Polarity and Vitamins Vitamins B and C= polar Dissolve in water of body cells Must replace by: Foods Vitamin supplement Vitamin C
52 22.4 Dissolving Without Water Polarity and Vitamins Vitamin A, D, E & K= nonpolar- dissolve in fat of body Do not get washed away Toxic in high concentration large doses dangerous
53 22.4 Section Check Question 1 Which of the following cannot dissolve oily dirt? A. ethanol B. mineral oil C. turpentine D. water
54 22.4 Section Check Answer The answer is D. Oily dirt is nonpolar and water alone cannot dissolve it.
55 22.4 Section Check Question 3 What are some characteristics of nonpolar solvents?
56 22.4 Section Check Answer Nonpolar solvents can dissolve nonpolar substances that water cannot, they are fat soluble, they are often flammable and some are toxic.
57 End of Chapter Summary File
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