1. Acids/Bases/Salts
Properties

2. Properties BASES ACIDS electrolytes electrolytes bitter taste
sour taste
turn litmus red
turn litmus blue
Feel like burning
slippery feel
vinegar, soda, apples, citrus fruits
ammonia, lye, antacid, baking soda
pH more than 7
pH less than 7

3. Naming
Acids are composed of hydrogen (H+) followed by an anion (negative ion).
If the acid formula contains oxygen in the anion, such as in H2SO4, it is known as an oxyacid.

4. 3 Rules To Naming Acids
If H + anion ending in –ide: Acid name is “hydro_____ic acid”
Take the root from the anion name and fill in the blank.

5. Acid Naming Example Example: HCl Cl is the anion, its name is chloride
Name of acid is: hydrochloric acid
Example: HF
F is the anion, its name is fluoride
Name of acid is: hydrofluoric acid

6. 3 Rules To Naming Acids
H + anion ending in –ate: Acid name is “_____ic acid”
Take the root from the anion name and fill in the blank.
“What I ATE was ICky”

7. Acid Naming Example Example: HNO3
NO3 1- is the anion, its name is nitrate
Name of acid is: nitric acid
Example: H2CO3
CO3 2- is the anion, its name is carbonate
Name of acid is: carbonic acid

8. Exceptions Sulfate (SO4 2-) Phosphate (PO4 3-)
Root is not sulf, but sulfur
Sulfuric acid
Phosphate (PO4 3-)
Root is not phosph, but phosphor
Phosphoric acid

9. 3 Rules To Naming Acids
H + anion ending in –ite: Acid name is “_____ous acid”
Take the root from the anion name and fill in the blank.
“Don’t bITE; it’s infectiOUS”

10. Acid Naming Example Example: HNO2 Example: HClO2
NO2 1- is the anion, its name is nitrite
Name of acid is: nitrous acid
Example: HClO2
ClO2 1- is the anion, its name is chlorite
Name of acid is: chlorous acid

11. Writing Formulas Just work backwards, using the three rules.
You must criss-cross charges, just like with ionic compounds
H+ + anion-

12. Acid Writing Example Hydrobromic acid Acetic acid Phosphorous acid
anion is bromide (Br -)
formula is HBr
Acetic acid
anion is acetate (C2H3O2 -)
formula is HC2H3O2
Phosphorous acid
anion is phosphite (PO33-)
formula is H3PO3

13. Naming
Hydroxide bases are composed of a cation (positive ion) followed by hydroxide (OH-).
Naming bases is much simpler than naming acids. Name the cation and then add “hydroxide.”

14. Exception!!!!
Memorize: NH3 = ammonia

15. Base Naming Example NaOH Mg(OH)2 Fe(OH)2
name of base: sodium hydroxide
Mg(OH)2
name of base: magnesium hydroxide
Fe(OH)2
name of base: iron (II) hydroxide

16. Writing Formulas Writing base formulas is straightforward.
Find the formula for the cation and then add OH -.
Remember to criss-cross the formula so that the charges equal out to zero.

17. Base Writing Example potassium hydroxide calcium hydroxide
cation is potassium (K+)
formula is KOH
calcium hydroxide
cation is calcium (Ca 2+)
formula is Ca(OH)2
aluminum hydroxide
cation is aluminum (Al 3+)
formula is Al(OH)3

18. Electrolytes Solutions that have “free ions” in solution.
***Use solubility rules to determine if a compound will ionize in water***
Those “free ions” conduct electricity.
Found in sports drinks because body cells need ions to do work
Ex: Sodium/Potassium Pump

19. Strong Acids
Strong because there is a strong attraction between the acid and the water molecule.
Every acid molecule ionizes (dissolves)

20. Strong Acids Prechloric Acid: HClO4 Sulfuric Acid: H2SO4
NEED TO MEMORIZE!
Prechloric Acid: HClO4
Sulfuric Acid: H2SO4
Hydriodic Acid: HI
Hydrobromic Acid: HBr
Hydrochloric Acid: HCl
Nitric Acid: HNO3

21. Strong Acids If it is not listed. it is considered a weak acid.
Weak- they remain as molecules, they don’t ionize in water.

22. Strong Bases
Strong because there is a strong attraction between the base and the water molecule.
Every base molecule ionizes (dissolves)

23. Strong Bases NEED TO MEMORIZE! Lithium hydroxide: LiOH
Calcium hydroxide: Ca(OH)2
Sodium hydroxide: NaOH
Strontium hydroxide: Sr(OH)2
Potassium hydroxide: KOH
Barium hydroxide: Ba(OH)2
Magnesium hydroxide: Mg(OH)2

25. Strong Bases If it is not listed. it is considered a weak base.
Weak- they remain as molecules, they don’t ionize in water (And so, do not for electrolyte solutions)

26. Indicators Chemical dyes that change color as pH changes.
Different indicators change colors at different pH levels
choose an indicator that will show a color change at the pH that you are interested in.
Indicators can be on a strip of paper
called pH or litmus paper
Other indicators can be added to the solution directly.
Some indicators change color more than once and can be added to solutions so that we can see what is happening over time.

27. pH scale 14 7
INCREASING
ACIDITY
INCREASING
BASICITY
NEUTRAL

28. pH
Whether or not a solution is acidic, basic, or neutral depends on the balance of H+ and OH- ions:
Neutral: [H+] = [OH-]
Acid: [H+] > [OH-]
Base: [H+] < [OH-]

29. pH calculations (#1) pH + pOH = 14
The sum of the pH and the pOH always equals 14.
pH + pOH = 14

30. Example Find the pH, the pOH = 5.3 pH + pOH = 14 pH = 14 - 5.3

31. pH
pH is the negative base 10 logarithm of the hydrogen ion concentration:
pH = - log [H+]

33. pH calculations (#2)
pH is the expression of the acidity or alkalinity of a solution in terms of its hydronium ion concentration.
pH = - log [H+]

34. Example Calculate the pH, if the [H+] = 2.4 X 10-6 M pH = - log [H+]
= - log(2.4 X 10-6)
= -(-5.6)
= 5.6

35. pH calculations (#3) Use an identical equation to calculate pOH.
pOH = - log [OH-]

36. pH calculations (#4)
Use the reverse of the equation to calculate the [H+] when pH is known.
[H+] =10(-pH)

38. Example Calculate the [H+], if the pH is 4.71. [H+] = 10(-pH)
= 10 ^ (- 4.71)
= 1.95 X 10-5 M

39. pH calculations (#5)
Use identical process for [OH-] when pOH is known.
[OH-] = 10(-pOH)

40. Acid/Bases/Salts Neutralization/Titrations

41. A. Neutralization Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.

42. ACID + BASE  SALT + WATER
A. Neutralization
ACID + BASE  SALT + WATER
HCl + NaOH  NaCl + H2O
strong
strong
neutral
HC2H3O2 + NaOH  NaC2H3O2 + H2O
weak
strong
basic
Salts can be neutral, acidic, or basic.
Neutralization does not mean pH = 7.

43. Neutralization HCl + NaOH  NaCl + H2O H2SO4 + KOH  HNO3 + Ca(OH)2 +1 -1
HCl NaOH 
H2SO KOH 
HNO Ca(OH)2 
NaCl + H2O
Hydrocholoric acid
Sodium chloride
Water
Sodium hydroxide +1 -2 2
K2SO4 + H2O 2
Potassium hydroxide
Potassium sulfate
Sulfuric acid
Water +2 2 -1
Ca(NO3)2 + H2O 2
Nitric acid
Calcium hydroxide
Calcium nitrate
water

44. B. Titration
standard solution
unknown solution
Titration
Analytical method in which a standard solution is used to determine the concentration of an unknown solution.

45. B. Titration End Point – Equivalence point
point at which an indicator changes color during a titration
Equivalence point
Point at which equal amounts of H3O+ and OH- have been added.
when mole ratio exactly equals mole ratio required by reaction
Determined by…
indicator color change
dramatic change in pH

46. moles H3O+ = moles OH- MV n = MV n B. Titration M: Molarity
V: volume
n: # of H+ ions in the acid or OH- ions in the base

47. B. Titration
42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4.
H3O+
M = ?
V = 50.0 mL
n = 2
OH-
M = 1.3M
V = 42.5 mL
n = 1
MV# = MV#
M(50.0mL)(2)
=(1.3M)(42.5mL)(1)
M = 0.55M H2SO4