1. Chapter 6 Notes: Solutions, Acids and Bases
Chapters 22: Solutions
Section 1: How Solutions Form
Mrs. Chilton

2. A. Solutions and Other Mixtures
All matter is either a pure substance or a mixture
Types of mixtures
Homogeneous = solution;
same composition throughout
Heterogeneous = not the same
composition throughout
Pure substances
Elements
Compounds

3. B. Solutions Solution is a homogeneous mixture
Made up of solute and solvent
Solute = what is dissolved
Solvent = substance doing the dissolving
Most common solvent?
Water! Why?

4. B. Solution Examples
KoolAid
Unsweet tea
Sweetened tea
Saltwater

5. C. Dissolving Molecules are constantly in motion according to…
Kinetic Theory of Motion
When particles collide, energy is transferred
When ionic compounds dissolve in water, ions separate in solution
Example: NaCl in water becomes Na+ and Cl-

6. D. Solvents Water is universal solvent b/c of its polarity
If something can dissolve in something else, it is said to be soluble
If it cannot dissolve, it is said to be insoluble
“Like dissolves like”

7. D. Solvents
“Like Dissolves Like”
NONPOLAR
POLAR

8. E. Solvation First... Then... Solvation – the process of dissolving
solute particles are surrounded by solvent particles
First...
solute particles are separated and pulled into solution
Then...

9. NaCl(s)  Na+(aq) + Cl–(aq)
E. Solvation
Dissociation
separation of an ionic solid into aqueous ions
NaCl(s)  Na+(aq) + Cl–(aq)

10. E. Solvation Non- Electrolyte Weak Electrolyte Strong Electrolyte+
sugar - +
acetic acid - +
salt
Non-
Electrolyte
Weak
Electrolyte
Strong
Electrolyte
solute exists as
molecules only
solute exists as
ions and
molecules
solute exists as
ions only

11. F. Factors Affecting Solubility
Solubility = amount of a substance that will dissolve in a liquid
Smaller pieces of a substance dissolve faster b/c of larger surface area
Stirring or shaking speeds dissolving b/c particles are moving faster and colliding more
Heating speeds dissolving (see above)
Not all substances dissolve

12. F. Solubility Solids are more soluble at...
high temperatures.
Gases are more soluble at...
low temperatures &
high pressures (Henry’s Law).
EX: nitrogen narcosis, the “bends,” soda

13. G. Solubility Solubility Curves
maximum grams of solute that will dissolve in 100 g of solvent at a given temperature
varies with temp
based on a saturated soln

14. G. Solubility Solubility Curve
shows the dependence of solubility on temperature

15. HNO3(aq) + H2O(l)  H3O+(aq) + NO3–(aq)
B. Solvation
Ionization
breaking apart of some polar molecules into aqueous ions
HNO3(aq) + H2O(l)  H3O+(aq) + NO3–(aq)

16. B. Solvation C6H12O6(s)  C6H12O6(aq) Molecular Solvation
molecules stay intact
C6H12O6(s)  C6H12O6(aq)

17. B. Solvation Soap/Detergent polar “head” with long nonpolar “tail”
dissolves nonpolar grease in polar water

18. H. Concentration
The more solute or less solvent in a solution, the more concentrated the solution becomes
The less solute or more solvent in a solution, the more dilute the solution becomes
A saturated solution is one in which no more solute can dissolve
A supersaturated solution is one in which the solvent is heated and can dissolve more solute

19. H. Concentration UNSATURATED SOLUTION more solute dissolves
no more solute dissolves
SUPERSATURATED SOLUTION
becomes unstable, crystals form
concentration

20. Chapter 23
Acids, Bases & Salts

21. Review – Acid Names
HCl
H2SO4
HNO3
H2SO3
HC2H3O2
Hydrochloric acid
Sulfuric acid
Nitric acid
Sulfurous acid
Acetic acid

22. What are acids? Compounds that donate H+ ions in water Taste sour
Concentrated acids can burn skin and eyes
On pH scale, found below 7
Stronger acids closer to 1
Examples: citric acid, stomach acid, soda, coffee

23. What are bases? Compounds that donate OH- ions in water
Taste bitter, are slippery
Can be dangerous as well
Often cleaning products
pH above 7
Stronger bases closer to 14
Examples: bleach, baking soda, antacids

24. Neutral All neutral solutions have a pH of 7
Water is a neutral solution

25. pH Scale

26. HCl + NaOH  H2O + NaCl Neutralization Example:
Reaction between an acid and a base to produce water and a salt
H+ + OH-  H2O
Example:
HCl + NaOH  H2O + NaCl
Do not always produce a neutral solution

27. Indicators
Chemical dyes whose color are affected by acidic and basic solutions are called acid-base indicators

28. Summary BASES ACIDS electrolytes  electrolytes sour taste
bitter taste
turn litmus red
turn litmus blue
Donate H+ (HCl)
Donate OH- (NaOH)
vinegar, milk, soda, apples, citrus fruits
ammonia, lye, antacid, baking soda