1. Solutions, Acids, and Bases
Chapter 8
Solutions, Acids, and Bases

2. 8.1 Formation of Solutions
DISSOLVING
Recall that a solution is a _____________ ________of two or more substances.
______- substance whose particles are dissolved in a substance.
______-The substance in which the solute dissolves.
These can be _____, ______, or _____. Most familiar is liquids.

3. 3 WAYS TO FORM SOLUTIONS
Substances can dissolve in liquids in three ways: __________, __________, and ___________
DISSOCIATION OF ______ COMPOUNDS
The particles that hold solutes to each other and solvents to each other must be overcome. Ex: NaCl is an ionic compound. Water is a polar molecule, and is attracted to the salt. The sodium and chlorine ions are pulled into solution one by one.
Dissociation-The process in which an ionic compound separates into ____ as it ______________.
When an ionic compound dissolves in water, the charged ends of water molecules surround the oppositely charged ions.

4. 3 WAYS TO FORM SOLUTIONS DISPERSION OF ___________ COMPOUNDS
Ex: Sugar and water are both polar molecules, so they attract one another. When the attractions between them are great enough to overcome the __________ holding the sugar molecule to the surface of the crystal, The sugar molecule breaks free, and is pulled into solution by the water molecules.
Dispersion-Breaking into small ________ that spread throughout the water.
Saliva dissolves the sugar in hard candy by dispersion. As water molecules collide with sugar crystals, attractions develop between the water molecules and sugar molecules at the ________ of the solid.

5. 3 WAYS TO FORM SOLUTIONS IONIZATION OF MOLECULAR COMPOUNDS
When HCl dissolves in water the hydrogen atom gets pulled away from chlorine and forms a hydronium ion. 
Ionization-_________molecules gain or lose electrons. This is different from the previous two because it is a _________ change. The solution that results contains ____substances.

6. Properties of Liquid Solutions
Only ______ physical properties of a solution will differ from those of its solute and solvent. They are ___________, ____________, and ________________.
CONDUCTIVITY
When NaCl is dissolved in water, the ion are free to ______. This will conduct an electric __________. NaCl ____ dissolved will not conduct a current.

7. Properties of Liquid Solutions
FREEZING POINT AND MELTING POINT
MgCl2 is used in winter to melt ice and snow. It ____________ into its ions. The structure of ice is __________ by the ions and cannot freeze.
Coolant is added to cars to _____ the boiling point and prevent the car from overheating.
The presence of solute particles affects how a solvent freezes. A Pure water freezes in a hexagonal pattern. B In water “salted” with MgCl2, the dissociated Mg2+ and Cl− ions ______ the formation of ice crystals.

8. HEAT OF SOLUTION
During the formation of a solution, energy is either _________ or _________. Like chemical reactions, this is described as endothermic or exothermic.
In order for a solution to form, bonds must be ________, and new attractions _______.
Breaking attractions ________ energy
The formation of attractions ________ energy
The difference in these energies is known as the ______________.

9. FACTORS AFFECTING RATES OF DISSOLVING
Like rates of chemical reactions, rates of dissolving depend on the __________and ________ of collisions that occur between very small particles.
Factors that affect the rate of dissolving include ___________, _________, and _________________.

10. Surface Area
When a sugar cube dissolves in water, the dissolving takes place at the _______ of the cube.
The _______ the surface area of a solid solute, the more _________ the collisions are between solute and solvent particles.
More collisions result in a_________rate of dissolving

11. Stirring
Stirring moves dissolved particles away from the _____ of the solid, and allows for ____ collisions between solute and solvent particles.
Stirring will make it dissolve _______.
The rate of dissolving can be increased by reducing the particle size of the solute, by stirring, and by heating the solvent.

12. Temperature
Increasing the temperature of a solvent causes its particles to move _______, on average.
As a result, both the number of _________ and the ________ of these collisions with solute particles increase.
The solute goes into solution more quickly.
Increase in temp. will _______________the rate of dissolving.

13. 8.2 Solubility & Concentration
Solubility- The __________ amount of a solute that dissolves in a given amount of solvent at a constant ______________
Solubilities are usually expressed in grams of ______ per 100 grams of ________ at a specified temperature
At a given temperature, different solutes have different solubilities in water.

14. 3 Ways Solutions are Classified
Solutions are described as __________, ____________, or _____________, depending on the amount of solute in solution.
Saturated Solutions - contains as much solute as the solvent can _____ at a given temperature
The solvent is “_______” with solute. If you add more solute, it will ____ dissolve.

15. 3 Ways Solutions are Classified
Unsaturated Solution - A solution that has ____ than the maximum amount of solute that can be dissolved
Supersaturated Solution is one that contains _____ solute than it can normally hold at a given temperature.
Supersaturated solutions are very ______. If even a tiny crystal of the solute falls into a supersaturated solution, the extra solute can rapidly ____________of solution
If you heat a solvent up, more solute may dissolve. Then you then ______ cool the solvent back without jarring it, you may be able to keep the _________________in solution.
In the photo sequence, a single crystal of sodium acetate, NaC2H3O2, is added to a supersaturated solution of sodium acetate in water. The excess solute rapidly crystallizes out of the solution.

16. Factors Affecting Solubility
Three factors that affect the solubility of a solute are the _________ of the solvent, ______________, and ____________
Generally, a solute is more likely to dissolve in a “like” solvent than an “unlike” solvent.

17. Polar and Nonpolar Solvents
Oil does not dissolve in water because oil molecules are __________ and water molecules are _______.
guideline for predicting solubility is “____ dissolves _____.”
Soaps and detergents are used to remove grease and oil stains. Soap molecules form attractions to both polar water molecules and nonpolar oil molecules. As the water flows away, it carries the oil with it.

18. Temperature
In general, the solubility of solids increases as the solvent temperature ___________
When a glass of cold water warms up to room temperature, bubbles form on the inside of the glass. These bubbles are _______ that were dissolved in the water. They come out of the solution as the water temperature________.
Unlike most solids, gases usually become _____soluble as the temperature of the solvent ____________.

19. Pressure
Increasing the pressure on a gas ____________ its solubility in a liquid.
The pressure of CO2 in a sealed 12-ounce can of soda at room temperature can be two to three times ________________ pressure

20. Concentration of Solutions
Concentration of a solution-the amount of solute dissolved in a ___________ amount of solution
Concentration of solution is usually expressed as % by _______ or % by _______.
Percent by volume =
Useful when dealing with liquids
Percent by mass =
Useful when solute is a solid

21. 8.3 Properties of Acids and Bases
Identifying Acids
Acid- a compound that produces __________ ions (H3O+) when dissolved in water.

22. Properties of Acids Sour Taste
Lemons, grapefruits, limes, and oranges have ____ acid
Vinegar has _________ acid
Spoiled dairy products have _________ acid
NEVER TEST AN ACID BY TASTING IT

23. Properties of Acids Reactivity with Metals Color Changes in indicators
Acids and metals undergo a __________________ reaction
Color Changes in indicators
_________ – any substance that changes color in the presence of an acid or base.
Ex: Blue Litmus paper turns____

24. Identifying Bases
Base- a compound that produces __________ ions (OH-) when dissolved in water.

25. Properties of Bases Bitter Taste Slippery Feel
Unsweetened (baking) chocolate
Slippery Feel
Wet__________
Wet_________
Color Changes in Indicators
Red Litmus paper turns ____ in a base
Phenolphthalein turns red
Hydrangeas turn blue in acid soil, pink in basic soil

26. Neutralization and Salts
The reaction between an acid and a base is called ________________
Negative ions in an acid combine with the positive ions in a base to produce an ionic compound called a ______________

27. The pH Scale
pH scale – a number scale from __________used to describe the concentration of hydronium ions in a solution.
A ________tells you that the concentration of H+ ions is _____. (acid)
A _______tells you that the concentration of H+ ions is ____. (base)
pH lower than 7 = ________ (0-6)
pH higher than 7 = __________ (8-14)
pH of 7 = _______