1. Introduction to Acids and Bases
Chapter 15
Pages
A physicist, biologist and a chemist were going to the ocean for the first time. The physicist saw the ocean and was fascinated by the waves. He said he wanted to do some research on the fluid dynamics of the waves and walked into the ocean. Obviously he was drowned and never returned.
The biologist said he wanted to do research on the flora and fauna inside the ocean and walked inside the ocean. He too, never returned.
The chemist waited for a long time and afterwards, wrote the observation, "The physicist and the biologist are soluble in ocean water".

2. ACIDS
What is the first thing that comes to mind when you hear the term acids?

3. Watch a short clip about the properties of acids

4. Properties of Acids Acids have a sour taste
Acids change the color of acid-base indicators
Acids react with active metals
Acids react with bases to produce water and salts
Acids are electrolytes- conduct electric currents

5. Match the acid name with formulas
Sulfuric Acid
Nitric Acid
Phosphoric Acid
Hydrochloric Acid
Acetic Acid
CH3COOH(aq)
H3PO4(aq)
HCl(aq)
HNO3(aq)
H2SO4(aq)

6. Properties of Bases Bases have a bitter taste
Bases change the color of acid-base indicators
Bases feel slippery
Bases react with acids to produce water and salts
Bases are electrolytes- conduct electric currents
MOST BASES ARE HYDROXIDE COMPOUNDS

7. Types of Acids and Bases
There are several different types of acids and bases
Since different chemists discovered different properties of acids and bases, each was recognized by the “type”

8. Svante Arrhenius
Svante August Arrhenius (19 February 1859 – 2 October 1927) was a Swedish scientist, originally a physicist, but often referred to as a chemist, and one of the founders of the science of physical chemistry.

9. Arrhenius Acids and Bases
Arrhenius acid is a substance that increases the concentration of hydrogen ions, H+, when dissolved in water
HCl(aq) → H+(aq) + Cl-(aq)
Arrhenius base is a substance that increases the concentration of hydroxide ions, OH-, when dissolved in water
NaOH(s) → Na+(aq) + OH-(aq)

10. Strong Acids
A strong acid are characterized by ability to dissociate 100% to form H+ (H3O+)
7 strong acids (NEED TO KNOW)
H2SO4 (Sulfuric) H2SO4 → H+ +HSO4-
HClO4 (Perchloric) HClO4 → H+ +ClO4-
HClO3 (Chloric) HClO3 → H+ +ClO3-
HNO3 (Nitric) HNO3 → H+ +NO3-
HCl (Hydrochloric) HCl → H+ +Cl-
HBr (Hydrobromic) HBr → H+ +Br-
HI (Hydroiodic) HI → H+ +I-

11. HINT FOR STRONG ACIDS H2SO4 (Sulfuric) 2 HClO4 (Perchloric) 3
For ternary acids, as long as there is a difference of 2 or more hydrogens, then the acid is strong
H2SO4 (Sulfuric) 2
HClO4 (Perchloric) 3
HClO3 (Chloric) 2
HNO3 (Nitric) 2

12. Strong Bases
A strong base is characterized by ability to dissociate 100% to form OH- ions in solution
The hydroxides are the only strong bases.
LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

13. Acids-Base Reactions
If there is a strong acid and strong base when they react, they undergo a neutralization reaction
Acid + Base → Salt + Water
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

14. Brønsted-Lowry
Johannes Nicolaus Brønsted born in Varde (February 22, 1879 – December 17, 1947) was a Danish physical chemist.
Thomas Martin Lowry (October 26, November 2, 1936) was an English physical chemist

15. Brønsted-Lowry
Brønsted-Lowry acid is a molecule or ion that is a proton donor (H+)
HCl (aq) +NH3 (g) → Cl- (aq) + NH4+ (aq)
Brønsted-Lowry base is a molecule or ion that is a proton acceptor
H2O(l) + NH3 (g) → NH4+ (aq) + OH-(aq)

16. Acids Base Reactions
If there is a transfer of a proton, the remaining ion or molecule can re-accept that proton and can act as a base
Thus, the leftover ion is then a conjugate base of that acid

17. Conjugate base Lets see an example HF(aq) + H2O(l) → F-(aq) + H3O+(aq)
Acid conjugate base
The fluoride ion is the conjugate base of hydrofluoric acid

18. Acids Base Reactions
If there is a transfer of a proton, the new ion can act as a acid
Thus, the new ion formed is then a conjugate acid of that base

19. Conjugate acid Lets see an example HF(aq) + H2O(l) → F-(aq) + H3O+(aq)
Base conjugate acid
The water molecule is a Brønsted-Lowry base. It accepts the proton to form H3O+, which is an acid. The hydronium ion is the conjugate acid of water.

20. Gilbert Lewis
Gilbert Newton Lewis (October 23, March 23, 1946) was a famous American physical chemist known for the discovery of the covalent bond (see his Lewis dot structures and his 1916 paper "The Atom and the Molecule") and his theory of Lewis acids and bases

21. Lewis Acids and Bases
Lewis acid is an atom, ion or molecule that accepts an electron pair to form a covalent bonds
Lewis base is an atom, ion or molecule that donates an electron pair

22. IMPORTANT!! Overview of types of acids
Table 15-6 Acid-Base Systems
Type
Acid
Base
Arrhenius
H+ or H3O+ producer
OH- producer
Brønsted-Lowry
Proton (H+) donor
Proton (H+) acceptor
Lewis
Electron-pair acceptor
Electron-pair donor

23. Concentration
The concentration or strength of a solution is measured by molarity
Molarity is the number of moles in one liter of solution

24. Concentration
Convert to grams
Convert to mL

25. Practice
What is the molarity of sulfuric acid if there is 3.8 moles dissolved in 2.5 liter?

26. Try One!
You have 3.50 L of solution that contains 90.0 grams of sodium chloride. What is the molarity of the solution?
First find the moles and then find the molarity
90.0 g NaCl ÷ mole/g= 1.54 moles
1.54 moles NaCl ÷ 3.50 liters=0.440 M
Molarity is M