1. Unit 8: Acids, Bases, and Salts Topic 1: Properties of Arrhenius Acids and bases

2. I. What is an acid (Arrhenius acid?
H2O
To be an acid, it must be dissolved in __________
When acids are dissolved in ______________ , they ______________ and form ______________________
IMPORTANT: ACIDS ARE SUBSTANES THAT CONTAIN…
See Table ___ in Reference Tables for ________________
H2O
BREAK APART
FREELY MOVING IONS
H+ IONS THAT IONIZE WHEN DISSOLVED IN WATER
COMMON ACIDS K

3. I. What is an acid (Arrhenius acid?
Example: When an acid is dissolved in water, the H+ leaves the acid and bonds to the water molecule to form a ________________________
HCl (g) + H2O (l)  H3O + (aq) + Cl - (aq)
The acid HCl contains 1 H+ which combines with 1 H2O to form 1 H3O+
HYDRONIUM ION (H3O+)
Dissociation of acids in water animation

4. Ii. PROPERTIES OF ACIDS
A) Acids eat away (oxidize) active metals to produce _____________________ Example: 2 Li + 2 HCl  ________________ (__________________________________________) B) Acids have a __________________(we will discuss this more later on)
HYDROGEN GAS
2 LiCl + H2
METAL HAS TO BE ABOVE HYDROGEN ON TABLE J
pH LESS THAN 7

5. Ii. PROPERTIES OF ACIDS
C) Acids are ________________, meaning the _______________________________________
D) Acids taste ________(like _________, but DO NOT TASTE unknown substances)
ELECTROLYTES
CONDUCT ELECTRICITY WHEN DISSOLVED IN WATER
SOUR
LEMONS

6. Iii. Weak vs. strong acids
Acids always produce H3O+ (hydronium) ions when dissolved in water. The more H+ that dissociate when in water, the stronger the acid will be.
Examples of Strong Acids – ____________________
Example of Weak Acid – ______________
H Cl, H NO3, H Br, H I
CH3CH2COOH
(HC2H5O2)
(organic acids)
WEAK VS. STRONG ACID ANIMATION
Weak vs. Strong Acid Animation #2

7. IV. What is a Base? (Arrhenius Base)
IMPORTANT: BASES ARE SUBSTANES THAT CONTAIN…
See Table _________ in Reference Tables for
____________________
Example: When a base is dissolved in water, the OH - 1 leaves the base
NaOH (s) ______________________
OH- (Hydroxide) ions dissolved in aqueous solution. L
COMMON BASES
Na + 1 (aq) + OH - 1 (aq)

8. V. Properties of bases
A) Bases have a _______________ (we will discuss this more later on)
B) Bases are _______________, meaning _________________________________ 
C) Bases taste ______________ (like _________)
D) Bases hydrolyze fats (turns them into soap, also called “saponification”)
The manufacture of soap involves heating up animal fat or vegetable oil, (for example, glyceryl stearate) dissolving it in alcohol and adding NaOH or KOH to it slowly. This forms a soap (for example, sodium stearate), which can now be used for cleaning!
pH above 7
ELECTROLYTES
THEY CONDUCT ELECTRICITY WHEN DISSOLVED IN WATER
BITTER
SOAP/ MEDICINE

9. VI. Strong vs. weak bases
Like acids, the more ions that dissociate in water, the stronger the base is. Bases formed with group 1 and 2 metals are typically stronger.
Examples of Strong Bases – __________________
Example of Weak Bases – ___________________
LiOH, NaOH, Mg(OH)2
Al(OH)3, NH4OH

10. Check for understanding
Identify the following as acids or bases
Identify it as a strong or weak acid/base
1) NaOH __________ 4) H2SO4 ___________
2) H3BO3 __________ 5) HC2H3O2 ___________
3) KOH __________ 6) Ca(OH)2 _________
acid
(strong)
base
(strong)
acid
(strong)
acid
(weak)
base
(strong)
base
(strong)

11. VII. Naming acids and bases (SKIP)
Naming Binary Acids (hydrogen with nonmetal):
- Name the hydrogen in the acid hydro-
- Name the anion and change ending of the name to –ic acid
Examples:
1. HCl (aq) - _ ____________________________
2. HI (aq) - _____________________________
3. HBr(aq) - ____________________________
4. H2S(aq) - _____________________________
Hydrochloric acid
Hydroiodic acid
Hydrobromic acid
Hydrosulfuric acid

12. VII. Naming acids and bases (SKIP)
Naming Ternary Acids (hydrogen with PAI’s) 
Go to Table ______ and name the PAI (polyatomic ion)
DO NOT use the prefix hydro –
If the PAI ends in - ate, it changes to –ic acid
If the PAI ends in – ite, it changes to –ous acid
Examples:
1) H2CO3 (aq) - _ ____________________________
2) H3PO4 (aq) - _____________________________
3) H2SO4 (aq) - _____________________________
4) H2SO3(aq) - _____________________________ E
Carbonic acid
Phosphoric acid
Sulfuric acid
Sulfurous acid

13. VII. Naming acids and bases (SKIP)
Naming Bases:
- Bases are all ____________________, therefore, they are named just like ________________
Name 1st element
Use roman numeral if the metal has more than one charge listed
2nd half of the name will typically be _______________
Examples:
1. NaOH (aq) - ____________________
IONIC COMPOUNDS
IONIC COMPOUNDS
HYDROXIDE
Sodium hydroxide

14. VII. Naming acids and bases (SKIP)
Naming Bases (continued):
2. Ca(OH)2 (aq) - _____________________________
3. Fe(OH)3 (aq) - _____________________________
4. Co(OH)2 (aq) - _____________________________
Calcium hydroxide
Iron (III) hydroxide
Cobalt (II) hydroxide

15. VIII. How to know if a solution is acidic or basic
Indicator – 
Acid-Base Indicators (Found on Table ___________)
Acid-Base Indicators and narrowing down pH using multiple indicators (mixture of indicators gives great range of colors, pH paper)
Remember: An acid has a pH _________________ and a base has a pH
_________________
a substance that changes color if an acid or base is added M
less than 7
above 7

16. VIII. How to know if a solution is acidic or basic
Tips Using Table M:
If the indicator changes TO the listed color, pH is ___________ the pH range.
If the indicator does NOT change, pH is __________ the pH range.
The pH range does NOT indicate that the solution has pH within that range
above
below

17. Tips on using Table M
Tip 1- Notice "Common Acid Base Indicators," acid is on the left and base is on the right.
Low pH numbers are on the left and high pH numbers are on the right. They match up.
Tip 2 - Look at Methyl Orange, red is on the left, 3.2 is on the left. To the left (or below) a pH of 3.2 the color is red.
To the right (above) a pH of 4.4 the color is yellow.
Tip 3 - Between the 2 numbers will never be asked on a test. This is where the indicator changes color.

18. VIII. How to know if a solution is acidic or basic
Example: A solution has a pH of 5.5. What color changes will happen to following indicators.
1) Methyl orange __________ 3) Bromscresol green____________
2) Bromthylmol blue ________ 4) Thymol blue ______________
yellow
blue
yellow
yellow

19. VIII. How to know if a solution is acidic or basic
Example: A solution yields the following results when tested with various indicators:
Methyl Orange = yellow
Phenolphthalein = clear
Bromcresol Green = blue
Thymol Blue = yellow
- Can the pH be:
a) 2.8 b) c) d) 4.8
 pH above 4.4
 pH below 8.0
 pH above 5.4
 pH below 8

20. Unit 8: Acids, Bases, and Salts Topic 2: pH SCALE

21. IX. The Power of Hydronium (What ph really means)
The pH scale is easiest method to use for comparing the strengths of acids and bases. We test our fish tanks (fish pee out ammonia, which is a base, and brings the pH up), our lawns (acid rain brings the pH of the soil down) and even food is pH tested as it is being made to make sure that it falls within the right range. You wouldn’t want your super sour candy to have too little bite, would you? So just what is this pH, what does it mean, and how is it measured?
Water breaks up very slightly to form hydrogen ions and hydroxide ions:
H2O  H +1 + OH – 1
In neutral water, the concentration of H + = 1.0 x M, so the pH = _____ 7
↑ [H+]
↑ [OH-]

22. IX. The Power of Hydronium (What ph really means)
A pH of 0-7 is __________ When the concentration of H+ is...
A pH of 7 is ____________  M, pH = ____, , pH =___
A pH of 7-14 is _____________ , pH = _____
acidic 1 2
neutral
basic 3

23. X. The Power of Hydronium (What ph really means)
The pH scale is logarithmic. Each change of a single pH unit signifies a tenfold change in the concentration of the hydrogen ion. Therefore, the[H+] is ten times greater in a solution of pH of 5 as in a solution of pH of 6.
Examples:
A solution with pH of 3 is 10 times more acidic than solution with a pH of ____
B) A solution with pH of 3 is ___________ times more acidic than solution with a pH of 6.
C) A solution with a pH of 2.0 has a hydronium ion concentration 10,000 times greater than a solution with a pH of ___________
4 (for every power of 10, pH goes UP 1)
1,000 6

24. X. The Power of Hydronium (What ph really means)
The pH scale is logarithmic. Each change of a single pH unit signifies a tenfold change in the concentration of the hydrogen ion. Therefore, the[H+] is ten times greater in a solution of pH of 5 as in a solution of pH of 6.
Examples (continued):
D) A sample of base has pH of 9. What would the pH of a base 1,000 more basic be?
E) A sample of acid has a pH of 3. What would be the pH of an acid 100 times more acidic be?
12 (for every power of 10, the pH goes UP 1 to become more basic)
1 (for every power of 10, the pH goes DOWN 1 to become more acidic)

25. X. The Power of Hydronium (What ph really means)

26. X. The Power of Hydronium (What ph really means) 

27. Unit 8: Acids, Bases, and Salts Topic 3: acid and base neutralization

28. Think about this…
If you add a strong acid to a base, what would happen to the pH of the mixed solution?

29. XI. Acid and base neutralization
Neutralization: When an acid and base are mixed, the ____________________ and the  ______________________ combine to form _______________. The anion of the acid and the cation of the base come together to form a _________________.
Neutralization of Acid and Base Video Clip
Double Replacement Animation
Rainbow Connection Demo (Titration with pH indicators)
Salt – __________________________________________
H+ of the acid
OH --- of the base
Water (H2O)
salt
An ionic compound (metal with nonmetal/PAI) that can be formed by acid-base neutralization

30. XI. Acid and base neutralization
Examples:
1) HCl (aq) + NaOH (aq) 
_____ _____ ______ ___________
2) H2SO4(aq) + 2 __________  K2SO4 (aq) + 2 _________
_______ _______ ___________ ___________
3) 2 HNO3(aq) + __________  Ca(NO3)2 (aq) + 2 __________
_______ _______ _______ _________
DOUBLE REPLACEMENT REACTIONS!!!
NaCl(aq) +
HOH (l)
water
acid
base
salt
HOH(l)
KOH (aq)
acid
salt
base
water
Ca(OH)2 (aq)
HOH (l)
acid
base
salt
water

31. XI. Acid and base neutralization
Example: Write the equation for the neutralization reaction between dilute nitric acid (HNO3) and potassium hydroxide (KOH). (DON’T FORGET TO BALANCE) 1 1 1 1
___ HNO3( aq) + ___ KOH (aq) 
___ H(OH)(l) + ___ K(NO3)(aq)
Potassium nitrate
water

32. XI. Acid and base neutralization
Example: Write the equation for the neutralization reaction between dilute Mg(OH)2 and HCl. (DON’T FORGET TO BALANCE) 1 2 2 1
___ Mg(OH)2 ( aq) + ___ HCl (aq) 
___ H(OH)(l) + ___ MgCl2(aq)

33. Neutralization Worksheet
Complete problems 1, 3, and 5 with your assigned partner.
Write the general chemical equation for a neutralization reaction:
Example: lithium hydroxide is mixed with carbonic acid.

34. Neutralization Worksheet (answers)
1) Ba(OH)2(aq) + 2HCl(aq)  BaCl2 (aq) + 2H2O(l) barium barium hydroxide + hydrochloric acid  barium chloride + water
2) 2Al(OH)3(aq) + 3H2SO4(aq)  Al2(SO4)3(aq) + 6H2O(l)
aluminum hydroxide + sulfuric acid  aluminum sulfate + water
3) 3Fe(OH)2(aq) + 2H3PO4(aq)  Fe3(PO4)2(aq) + 6H2O(l)
iron (II) hydroxide + phosphoric acid  iron (II) phosphate + water

35. Neutralization Worksheet (answers)
4) Ca(OH)2(aq) + 2HNO3(aq)  Ca(NO3)2(aq) + 2H2O(l)
calcium hydroxide + nitric acid  calcium nitrate + water
5) 2NH4OH(aq) + H2S(aq)  (NH4)2S(aq) + 2H2O(l) ammonium hydroxide+ hydrosulfuric acid ammonium sulfide
+ water
6) KOH(aq) + HClO2(aq)  KClO2(aq) + H2O(l) potassium hydroxide + chlorous acid  potassium chlorite
+ water

36. XII. Titration (video demo)
Definition: process of adding a known amount of solution of known concentration to determine the concentration of another solution
moles of H+1 (aq) = moles of OH-1 (aq)
Molarity of Acid * Volume of Acid = Molarity of base * Volume of Base
Titration Equation (see Table T):
Titration Animation
Titration Animation #2
One mole of H + neutralizes one mole of OH --
MA(VA) = MB(VB) OR
(#H+)(MA)(VA) = (#OH---)(MB)(VB)

37. X. Titration
Example: What is the concentration of hydrochloric acid solution if 50.0 mL of a M KOH are needed to neutralize 20.0 mL of the HCl solution of unknown concentration?
(#H+)(MA)(VA) = (#OH---)(MB)(VB)
#H+= 1
MA = ?
MA = (#OH---)(MB)(VB)
(#H+)(VA)
VA = 20.0 mL
#OH--- = 1
MB = M
MA = (1)(0.250 M)(50.0 mL)
(1)(20.0 mL)
VB = 50.0 mL
= M

38. X. Titration
Example: What is the concentration for sulfuric acid solution if 50 mL of a M KOH are needed to neutralize 20 mL of the sulfuric solution of unknown concentration?
H2SO4
(#H+)(MA)(VA) = (#OH---)(MB)(VB)
#H+= 2
MA = ?
MA = (#OH---)(MB)(VB)
(#H+)(VA)
VA = 20.0 mL
#OH--- = 1
MB = M
MA = (1)(0.250 M)(50.0 mL)
(2)(20.0 mL)
= M
VB = 50.0 mL

39. X. Titration
Example: How many mL of 2.0 M H2SO4 are required to neutralize 30.0 mL of M NaOH?
(#H+)(MA)(VA) = (#OH---)(MB)(VB)
#H+= 2
MA = 2.0 M
VA = (#OH---)(MB)(VB)
(#H+)(MA)
VA = ?
#OH--- = 1
MB = 1.0 M
MA = (1)(1.0 M)(30.0 mL)
(2)(2.0 M)
VB = 30.0 mL
= 7.5 mL

40. X. Titration (complete in class)
Example: How many mL of 0.10 M Ca(OH)2 are required to neutralize 25.0 mL of M HNO3?
(#H+)(MA)(VA) = (#OH---)(MB)(VB)
#H+= 1
MA = 0.50 M
VB = (#H+)(MA)(VA)
(#OH---)(MB)
VA = 25.0 mL
#OH--- = 2
MB = 0.10 M
VB = (1)(0.50 M)(25.0 mL)
(2)(0.10 M)
= mL
VB = ??

41. TITRATION Partner Activity
With a partner and on a separate piece of paper answer question (evens only) on pages in the Unit 8 Work Packet.
Be sure to show ALL your work
I will collect one person’s paper from each group to grade.