1. Ch. 17 Water and Aqueous Systems
Water is a ___________ molecule and therefore __________.
Water forms _______________ ________ which strongly bonds the molecules together with each other. These intermolecular bonds give water some very unique properties:
1) High surface tension: acts like a thin “________” on the surface.
_______________ are used to reduce water’s surface tension so it can “wet down” a surface such as clothing.
bent
polar
hydrogen
bonds
skin
Detergents
“Water Strider”

2. Surface Tension of Water
metal paper clip on water
water forms “beads”

3. More Unique Properties of Water
2) Water forms 6-sided (hexagonal) ___________ of ice or snow and _____________ when it freezes. This makes ice ______ dense than water, so it ___________.
crystals
expands
less
floats
3) Water readily dissolves other _____________ substances and ionic solids/salts.
polar

4. Aqueous Solutions There are two parts to a solution:
1) ____________- the dissolving medium which is typically a liquid or the substance in greater amount when 2 similar phases are mixed
2) _____________ - the substance that dissolves
Solvent
Solute

5. Examples of common solutions:
Kool-aid = _________ in _______
Air = ____ in ____
sugar
water O2 N2
14K gold = _______ in _________
silver
gold

6. Examples of common solutions:
__________ = copper in zinc
Cola Drinks = sugar in water and ______ in ___________
Brass
CO2
water

7. “Like Dissolves Like”
This phrase means that polar solvents dissolve __________ solutes and nonpolar solvents dissolve ___________ solutes.
Example: Mix together water, oil, table salt, and iodine (I2).
What dissolves in what? ________________
____________________________________
polar
nonpolar
The nonpolar oil will dissolve the nonpolar I2
and the water dissolves the salt since they are
both polar.

8. nonpolar grease remover
“Like Dissolves Like”
nonpolar grease remover

9. “Unlike Polarity Cannot Dissolve Unlike”
Vinegar & oil dressing will separate. Shake well before using!

10. Solutions & Electricity
__________________- a solution that conducts electricity.
__________________- a solution that does not conduct electricity.
What Determines if a Solution will Conduct Electricity?
A solution will conduct if there are ____________ ______________ (or _________), in the solution.
Will a Solution be a Strong or Weak Electrolyte?
Using the Solubility Chart:
______ = many ions in the solution = __________________
______= few ions in the solution = ____________________
______= no ions in the solution = _____________________
Electrolyte
Nonelectrolyte
charged particles
ions S
Strong Electrolyte sS
Weak Electrolyte I
Nonelectrolyte
The Solubility Chart only lists ionic substances so if it isn’t in the chart it isn’t ionic and it isn’t an electrolyte!

11. The Light Bulb Demonstration
bright glow weak glow no glow
Strong Electrolyte Weak Electrolyte Nonelectrolyte
completely dissociate into ions
Examples: salt water, _______, drain cleaner
incompletely dissociate into ions
Examples: tap water, __________
no dissociation
Examples: sugar in water, _____, alcohol
oil
HCl
vinegar

12. air, brass, sugar water, salt water
Types of Mixtures
Type of Mixture Suspension Colloid True Solution
Relative Particle Size
Do the particles sink to
the bottom over time?
Can you filter out the particles?
Do the particles scatter a beam of light?
Examples
Large
Medium
Small
YES NO NO
YES NO NO
YES
YES NO
jello, paint, milk
air, brass, sugar water, salt water
muddy water
Tyndall Effect

13. vinegar and oil salad dressing
Suspensions
vinegar and oil salad dressing

14. Colloidal Gold and Colloidal Silver
Particle size ranges from 1 nm to 1000 nm.
Colloidal Silver

15. True Solutions

16. Water Vocabulary
hydrate- crystals that contain __________. (See Fig & Table 17.4)
Example: CuSO4·5H2O copper (II) sulfate pentahydrate
anhydrous- no _________ at all in the _______________.
Examples: ___________ ______________, CaCl2 beads.
water
water
crystal
Anhydrous ammonia

17. Anhydrous Examples

18. Ch. 18-- Solutions Solution Vocabulary
Solubility tells us how much _________ can dissolve in a certain amount of _____________ at a particular temperature and pressure to make a “__________________” solution.
Solution Vocabulary
_________________ solutions: the solution cannot hold any more solute. (Some solute may be sitting on the bottom of the container.)
________________ solutions: the solution could dissolve more solute
____________________ solutions: the solution is holding more than it should at the given temperature, and if you messed with the solution by shaking it or throwing in one more crystal, the whole thing would _________________ rapidly!
solute
solvent
saturated
Saturated
Unsaturated
Supersaturated
crystallize

20. Supersaturated Sodium Acetate Solution

21. Factors that Affect Solubility
1) Temperature:
a) Gas dissolved in Liquid: As temperature_____ , solubility ______.
Examples: O2 in a fish tank…(________ water suffocates fish.)
CO2 in soda… (_________ soda loses fizz.)
inc.
dec.
Warm
Warm

22. Factors that Affect Solubility: Temperature
b) Solid dissolved in Liquid: As temperature ______ , solubility “generally” ________________.
Example: sugar in hot tea vs. sugar in iced tea
inc.
increases

23. Factors that Affect Solubility: Temperature
(abnormal behavior)

24. Factors that Affect Solubility
2) Pressure:
a) Gas dissolved in Liquid: As pressure _____ , solubility ______.
Examples: CO2 in soda: (made under _______ pressure)
inc.
inc.
high

25. Factors that Affect Solubility: Pressure
b) Solid dissolved in Liquid: As pressure ___________ , solubility ______ ______ _____________!!
Since you cannot compress either a solid or a liquid, pressure has ____ effect on the solubility!
inc.
does not change no

26. Measuring the Concentration of a Solution
___________________: how much solute is dissolved in a certain amount of solvent at some given temperature and pressure.
Qualitative Vocabulary
_______________ : contains a small amount of solute
_______________ : contains a large amount of solute
Concentration
Dilute
Concentrated
concentrated
dilute

27. concentrated
dilute

28. Quantitative Vocabulary:
____________: moles of solute per liter of solution
_______________ ( ) = moles of solute ÷ Liters of solution
Practice Problem: What is the molar concentration of an aqueous NaCl solution when 25.0 grams are dissolved in water to make 500 mL of solution?
Molarity
Molarity M
moles
Grams of solute = (M) x (L) x (Molar Mass)
Molarity X
Liters
25.0 g = (M) x (0.500 L) x (58.5 g/mole)
Molarity = M

30. Freezing Points and Boiling Points of Solutions
Any solute added to a liquid will _____________ the freezing point of the liquid.
In other words, if you put salt into water, instead of it freezing a 0˚C, it will freeze somewhere _________ zero depending on how concentrated the solution is.
Uses include making homemade ice cream and melting ice on a sidewalk.
lower
below

31. Freezing Point Depression

32. Freezing Points and Boiling Points of Solutions
Any solute added to a liquid will _____________ the boiling point of the liquid. In other words, if you put salt into water, instead of it boiling a 100˚C, it will boil somewhere ________ 100˚C depending on how concentrated the solution is. The solute decreases the solution’s vapor pressure. (See Fig )
Since ionic solids break up into multiple ions when dissolving, they actually change the F.P. & B.P. __________ than a molecule would.
That’s one reason why we use salts to melt ice instead of using sugar!
raise
above
more
lowest freezing point & highest boiling point

33. Boiling Point Elevation
Boiling Point (sea level):
219° F at 40 percent concentration 222° F at 50 percent 225° F at 60 percent

34. Ch. 20 Notes -- Acids and Bases
What makes something an acid?
Acid Properties:
(1) tastes _______-- _______________
(2) corrosive to _________
(3) contains [ ___ ] (or [ _____ ] = “_______________” ions)
(4) proton ([ ___ ]) __________-- Brønsted-Lowry Theory
Example: HCl + H2O  ______ + ______
sour
lemons
metals H+
H3O+
hydronium H+
donor
H3O+
Cl−

35. Examples of Common Acids:
Pepsi, _________ juices, ___________, stomach acid, battery acid, _____________, ______
citrus
aspirin
vinegar
DNA

36. Acid Vocabulary
strong acid - readily ___________ to produce ______ [H+] ions in water
Examples: _________, HNO3, _______
weak acid - produces a __________ amount of [H+] ions when in water
Examples: HC2H3O2 (vinegar) , _________, _________
dissociate
many
H2SO4
HCl
small
H2CO3
lemon juice

37. Strong Acids vs. Weak Acids

38. Indicator Colors For Acids
Indicators
An indicator is a chemical that will change ___________ when placed in an acidic, basic or neutral environment.
Indicator Colors For Acids
litmus paper = _______
phenolphthalein = ___________
methyl orange = _______
colors
red
clear
red

39. pH Paper : Indicator Colors
Neutral
Acidic
Basic

40. Properties of Bases What make something a base?
Base Properties: (…the opposite of acid properties)
(1) tastes ________ -- ___________ peel , parsley, dark chocolate
(2) feels _____________ -- ________
(3) contains [ _____ ] ions
(4) proton ([H+]) ______________-- Brønsted-Lowry Theory
Example: NH H2O  ______ + _______
bitter
banana
slippery
soap
OH−
acceptor
NH4+
OH−

41. Indicator Colors for Bases
litmus paper = _______
methyl orange = ____________
phenolphthalein = ______
blue
yellow
pink
phenolphthalein
Acid
Base

42. Common Bases
Examples of Common Bases: milk of magnesia, ___________, drain cleaner, soap, blood, ____________ tablets, ___________ ________.
ammonia
antacid
baking
soda

43. Strong Bases vs. Weak Bases
strong base- readily __________ to produce ______ [OH−] ions in water
Examples: NaOH , ________
weak base- produces a __________ amount of [OH−] ions when in water
Examples: _____ (ammonia); Mg(OH)2 (milk of magnesia)
dissociate
many
KOH
small
NH3

44. Conjugate Acid-Base Pairs
Conjugate Acid- substance formed when a _______ gains a [H+] ion.
Conjugate Base- substance formed when an ______ loses a [H+] ion.
Practice Problems: Label the acid & base on the left side of the reaction and the conjugate acid & conjugate base on the right side.
a) HCl H2O  H3O Cl−
______ ______ ______ ______
b) NH H2O  NH OH−
_____ ______ ______ ______
base
acid
acid
base
C.A.
C.B.
base
acid
C.A.
C.B.

45. Measuring the Amount of H+ Ions in a SolutionpH
concentration
_____ Scale- measures the _____________ of [H+] ions in a solution
Formulas
pH = − (log [H+])
[H+] = 10−pH
With the pH scale, we have another way to define acids and bases:
Acids have a pH _________7.0
Bases have a pH _________7.0
Neutral pH ___7.0
below
above =

47. Practice Problems: 1) a) Calculate the pH of a 0.001 M HCl solution.
2) a) Calculate the pH of a 1 x M HCl solution.
3) What is the [H+] of a solution with a pH of 8.0?
[H+] = M
So…pH = − (log M)
pH = 3
[H+] = 1 x 10–5 M
So…pH = − (log 1 x 10–5 )
pH = 5
[H+] = 10−pH
[H+] = 10−8 Molar or 1.0 x 10−8 M

48. Ch. 21 Notes -- Neutralization
Neutralization Reactions
When an acid and base are mixed, the reaction produces _______ and ___________.
If the initial concentrations and volumes of the reactants are equal, the products will be ____________... (pH= 7.0)
These reactions are _________ ___________ reactions!
salt
water
neutral
double replacement

49. Titration
Mixing an acid with a base to determine a __________________ is called “titration.”
An ____________ is used to determine when neutralization has occurred.
________________ Solution - the solution of known concentration
The ______________ point is where the moles of [H+] ions equals the moles of [OH−] ions.
concentration
indicator
Standard
equivalence

50. Determining the Concentration of an Acid (or Base) by Titration
(Macid)x(Vacid) = (Mbase)x(Vbase)
Practice Problems:
A 25 mL solution of HNO3 is neutralized by 18 mL of 1.0 M NaOH standard solution using phenolphthalein as an indicator. What is the concentration of the HNO3 solution?
(2) How many mL of 2.0 M KOH will it take to neutralize 55 mL of a M HCl standard solution?
( ) x ( ) = ( ) x ( )
Macid
25 mL
1.0 M
18 mL
Macid = Molar
( ) x ( ) = ( ) x ( )
0.76 M
55 mL
2.0 M
Vbase
Vbase = mL