1. Acids and Bases

2. Naming Acids Binary Acids- Contains H and one other element
Use the prefix hydro- and the root of the second element (change end to “ic”) + acid
Examples:
HCl- hydrochloric acid HF- hydrofluoric acid
HI- hydroiodic acid HBr- hydrobromic acid
*Special case- for acids w/ 3 elements (polyatomic ions), but no O:
Prefix hydro- and the root of the polyatomic ion (change end to “ic”) + acid
HCN hydrocyanic acid

3. Naming acids, cont.
Oxyacids- Contains an H and a polyatomic ion with an Oxygen
Use the root of the ion, add a suffix (ic or ous), then acid
**Do not use the prefix “hydro” for these!
When to use ic or ous:
If the ion ends in “ate” = change end to “ic”
Ex: HNO3 (anion = nitrate) = nitric acid
If the ion ends in “ite” = change end to “ous”
Ex: HNO2 (anion = nitrite) = nitrous acid

4. Naming Bases Name of element + hydroxide Mg(OH)2 magnesium hydroxide
KOH potassium hydroxide
**H must be at the beginning of the formula to be an acid**

5. What is an acid? - Sour taste - Turns blue litmus paper pink
-- Makes a conjugate base
-- Reacts with some metals to make H2 gas
-- pH less than 7
-- More H+ ions than OH-
-- Conducts electricity
-- Usually dissolved/diluted in H2O
-- H+ ion donor in reactions
-- Donates an H+ to base
-- Sometimes water acts as the acid in the reaction

7. What is an acid? Strong Acids Sulfuric Acid – H2SO4
Hydrobromic Acid – HBr
Hydrochloric Acid – HCl
Nitric Acid – HNO3
Ionize completely in reactions
Reaction goes to completion (cannot go in reverse)
Good conductors of electricity
Make weak conjugate bases
Weak Acids
Hydrofluoric Acid – HF
Acetic Acid – HC2H3O2
Hydrosulfuric Acid – H2S
Carbonic Acid – H2CO3
Ionize partially in reactions
Reaction in equilibrium (can go in reverse)
Does not conduct electricity well
Make strong conjugate bases

8. What is a base? -- Bitter taste -- Slippery to touch
-- Turns pink litmus paper blue
-- More OH- ions than H+ ions
-- pH greater than 7
-- Makes conjugate acid in reactions
-- Accepts H+ from acid
-- Conducts electricity
-- Usually dissolved/diluted in H2O
-- Sometimes water acts as a base in reactions

10. What is a base? Strong Bases Litihium hydroxide – LiOH
Sodium hydroxide – NaOH
Potassium hydroxide – KOH
Magnesium hydroxide – Mg(OH)2
Dissociate (dissolve) completely in water solutions to make metal ions and OH ions
NaOH  Na+ + OH-
Make weak conjugate acids
Weak Bases
Ammonia – NH3
Aluminum hydroxide – Al(OH)3
Iron (III) hydroxide – Fe(OH)3
Partially dissociates in water solutions to make conjugate base and OH ions
CH3NH2 + H2O ↔ CH3NH3+ + OH-
Make strong conjugate acids

11. What are conjugate acids and bases?
-- Conjugate acid -- created when a base accepts an H+
-- Conjugate base – created when an acid donates (gives away) an H+
-- Creates a conjugate acid-base pair – 2 substances related to each other by donating/accepting H+ ions in a reaction
-- General equation for a acid-base reaction is:
HX H2O  H3O X-
So, H2O and OH- are a conjugate acid-base pair and NH3 and NH4+ are a pair as well.
EXAMPLES: Identify the acid/base/c. acid/c. base
NH3 + H2O  NH OH-
NH3 + H2O ↔ NH OH-
HCN + H2O ↔ H3O+ + OH-
ACID
BASE
C. ACID
C. BASE

12. Other things to know…
-- Water is amphoteric, which means it can act as an acid or a base. It depends on what it reacts with that decides if it’s an acid or a base.
-- Monoprotic acids – only donate 1 H+ to the reaction
-- i.e. NH4 will become NH3 H2O will become OH-
-- Diprotic acids – donate 2 H+ to the reaction
-- i.e. H2SO4 will become SO42- H2CO3 will become CO32-
-- Polyprotic acids – donate 3 or more H+ to the reaction
-- i.e. H3PO4 will become PO43-
-- The process of giving off H+ ions is called ionization
-- The model we use to identify acids/bases/c. acids/c. bases is called the BrØnsted-Lowry model of acids and bases
-- Strength does not mean concentration. Just because an acid is strong does not mean it has a high molarity concentration.

13. What is the pH scale?
-- The pH scale measures how acidic or basic a substance is.
-- pH greater than 7 is basic
-- pH less than 7 is acidic
Stomach acid
Household ammonia
Battery acid
Soft drinks
Tomatoes
Coffee
Antacid
Hair remover
Milk
Pure water
Blood
Soap/Detergent
Milk of magnesia
Oven cleaner

14. pH (power of hydrogen)
Acids, Alkalis and Neutralization

15. How do you calculate pH? FORMULA: pH = -log [H+]
Example 1: What is the pH of a solution with a [H+] of 1x10-2?
pH = - log (1x10-2)
= - (log 1 + log 10-2)
= - [0 + (-2)]
= - [-2]
= 2
Example 2: What is the pH of a neutral solution?
pH = - log (1x10-7)
= - (log 1 + log 10-7)
= - [0 + (-7)]
= - [-7]
= 7

16. How do you calculate pOH?
-- pOH is the concentration of the OH- ions in a solution
-- pH + pOH = 14
FORMULA: pOH = -log [OH-]
Example 1: Ammonia has an [OH-] concentration of 4.0x Calculate pOH and pH.
pOH = - log (4x10-3)
= - (log 4 + log 10-3)
= -[ (-3)]
= - (-2.40)
= 2.40
pH = 14
pH =
= 11.60

17. Acid Base Indicators
-- Chemical dyes that change colors depending on their placement in an acidic or basic solution.
-- Some indicators may remain colorless in certain pH ranges.
-- Used in toys that change colors when water is added.

18. Indicators

19. Neutralization
Is a chemical reaction between and acid and a base in an aqueous solution
Usually a double replacement reaction
Makes water and a salt

20. Neutralization Reactions
-- Reaction where an acid and base react in an aqueous solution to produce a salt and water
EXAMPLE: Mg(OH) HCl  MgCl H2O
base acid salt water
MgCl2 made up by: Mg2+ from base and Cl- from acid
More Examples:
Write the salt and water formed from HCl reacting with NaOH.
HCl NaOH  NaCl H2O
salt water
Write the equation and identify the acid, base, salt, and water formed when nitric acid reacts with cesium hydroxide.
HNO CsOH  CsNO H2O
acid base salt water

21. More Practice….. 1) hydrobromic acid and calcium hydroxide
2) sulfuric acid and potassium hydroxide
3) acetic acid and ammonium hydroxide

22. Answers 1) 2HBr + Ca(OH)2  CaBr2 + H2O 2) H2SO4 + 2KOH  K2SO4 + H2O
3) HCH3COO + NH4OH  NH4CH3COO + H2O

23. Label as Acid, Base, or Salt
A) Na2SO4
B) Mg(OH)2
C) Ba3(PO)4
D) H3PO4
E) HI
F) Cu(OH)2
G) CsCl