1.	Properties of Acids
a.	Acids have a sour taste
b.	Acids change the color of acid-base indicators
c.	Acids react with active metals
d.	Acids react with bases to produce water and salts 
e.	Acids are electrolytes- conduct electric currents
2.	Properties of Bases
a.	Bases have a bitter taste
b.	Bases change the color of acid-base indicators
c.	Bases feel slippery
d.	Bases react with acids to produce water and salts
e.	Bases are electrolytes- conduct electric currents
f.	MOST BASES ARE HYDROXIDE COMPOUNDS
3.	Types of Acids and Bases
a.	There are several different types of acids and bases
b.	Since different chemists discovered different properties of acids and bases, each was recognized by the “type”
i.	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.
1.	Arrhenius Acids and Bases
a.	Arrhenius acid is a substance that increases the concentration of hydrogen ions, H+, when dissolved in water
i.	HCl(aq) → H+(aq) + Cl-(aq)
b.	Arrhenius base is a substance that increases the concentration of hydroxide ions, OH-, when dissolved in water
i.	NaOH(s) → Na+(aq) + OH-(aq)
2.	A strong acid is characterized by ability to dissociate 100% to form H+ (H3O+)
a.	7 strong acids (NEED TO KNOW)
i.	H2SO4	 (Sulfuric) 	H2SO4 → H+ +HSO4-
ii.	HClO4	 (Perchloric)	HClO4 → H+ +ClO4-
iii.	HClO3 (Chloric) 		HClO3 → H+ +ClO3-
iv.	HNO3	 (Nitric) 	HNO3 → H+  +NO3-
v.	HCl (Hydrochloric) 	HCl  → H+  +Cl-
vi.	HBr (Hydrobromic) 	HBr  → H+  +Br-
vii.	HI (Hydroiodic) 		HI   → H+  +I-
b.	HINT FOR STRONG ACIDS
c.	For ternary acids, as long as there is a difference of 2 or more hydrogens, then the acid is strong
d.	H2SO4		(Sulfuric) 		2
e.	HClO4	 	(Perchloric)		3
f.	HClO3 		(Chloric)			2
g.	HNO3	 	(Nitric)			2
3.	A strong base is characterized by ability to dissociate 100% to form OH- ions in solution
a.	The hydroxides are the only strong bases.
i.	LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
4.	Acids-Base Reactions
a.	If there is a strong acid and strong base when they react, they undergo a neutralization reaction
i.	Acid + Base → Salt + Water
ii.	HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

ii.	Brønsted-Lowry
1.	Johannes Nicolaus Brønsted born in Varde (February 22, 1879 – December 17, 1947) was a Danish physical chemist.
2.	Brønsted-Lowry acid is a molecule or ion that is a proton donor (H+)
a.	HCl (aq) +NH3 (g) → Cl- (aq) + NH4+ (aq)
3.	Brønsted-Lowry base is a molecule or ion that is a proton acceptor
a.	H2O(l) + NH3 (g) → NH4+ (aq) + OH-(aq)
4.	Acids Base Reactions
a.	If there is a transfer of a proton, the remaining ion or molecule can re-accept that proton and can act as a base
b.	Thus, the leftover ion is then a conjugate base of that acid
c.	Let’s see an example
i.	HF(aq) +    H2O(l)   →   F-(aq) 	+ 	H3O+(aq)
ii.	Acid	            conjugate
			base
d.	The fluoride ion is the conjugate base of hydrofluoric acid
e.	If there is a transfer of a proton, the new ion can act as an acid
f.	Thus, the new ion formed is then a conjugate acid of that base
g.	Let’s see an example
i.	HF(aq) + H2O(l)   →    F-(aq)    +   H3O+(aq)
           					      Base 			conjugate 						            					  acid

h.	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.
iii.	Gilbert Lewis
1.	Gilbert Newton Lewis (October 23, 1875 - 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
2.	Lewis acid is an atom, ion or molecule that accepts an electron pair to form a covalent bond
3.	Lewis base is an atom, ion or molecule that donates an electron pair
4.	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	

5.	Concentration - The concentration or strength of a solution is measured by molarity
a.	Molarity is the number of moles in one liter of solution
b.	Practice - What is the molarity of sulfuric acid if there is 3.8 moles dissolved in 2.5 liter?

6.	The strength of an acid or base is determined by the concentration of H3O+ or OH-
a.	Before examining the pH scale, we need to look at the self-ionization of water, two water molecules produce a hydronium ion and a hydroxide ion
i.	Self-ionization of water: H2O(l) + H2O(l) → H3O+(aq) + OH-(aq) 
ii.	Experimental measurements show that the concentration of H3O+ and OH- are each 1.00x10-7 mol/L of water at 25 °C
iii.	To indicate concentration, the ion or molecule is enclosed in brackets
1.	[H3O+]= 1.00x10-7 mol/L →molar concentration of hydronium ion
2.	[OH-]= 1.00x10-7 mol/L →molar concentration of hydroxide ion
iv.	The product of [H3O+] and [OH-] remains constant in water at certain temperatures
v.	Thus, this constant is called the ionization constant of water
1.	Kw= [H3O+] [OH-] 
2.	The Kw of water at 25 °C is 1.0x10-14 M2
vi.	Although Kw does vary with temp, for our class, we will assume Kw=1.0x10-14 M2 unless stated otherwise
b.	Calculating [H3O+] and [OH-] 
i.	So initial concentration of acid or base will be the same concentration of H+ or OH-, respectively
ii.	What is the concentration of H3O+ and OH- if 1.0 x 10-2 M NaOH dissociates by the following equation? NaOH→ Na+ + OH-
1.	Since we know that NaOH is a strong base, the [OH-]= 1.0 x 10-2 
2.	Also, since Kw= [H3O+] [OH-], we can find [H3O+] 
3.	1.0x10-14 = [H3O+] [1.0 x 10-2]
4.	[H3O+] =1.0x10-12 M
7.	pH Scale
a.	Expressing acidity or basicity in terms of H3O+ or OH- can be cumbersome
b.	A more convenient quantity is called pH
c.	The letters pH stand for the French words, pouvior hydrogène, meaning “hydrogen power”
d.	The pH of a solution is defined as the negative log of the hydronium ion concentration [H3O+]
e.	pH= -log[H3O+]
i.	Since the [H3O+] of water is 1.0x10-7 M what is the pH
1.	pH= -log[H3O+]
2.	pH= -log[1.0x10-7]
3.	pH= 7.0
f.	Likewise, the pOH of a solution is defined as the negative log of the hydroxide ion concentration [OH-]
i.	pOH= -log[OH-]
1.	Since the [OH-] of water is 1.0x10-7 M what is the pOH 
a.	pOH= -log[OH-]
b.	pOH= -log[1.0x10-7]
c.	pOH= 7.0
g.	Let’s put them together
i.	Remember that the values of [H3O+] and [OH-] are related to Kw…
1.	The –log[Kw] = -log[1.0x10-14] =14.0
2.	Thus…. pH + pOH =14.0
8.	What is the pH and pOH of a solution that is 5.8x10-4 HCl?