sour taste electrolytes identified by the presence of h + ions (arrhenius). proton (h + ) donor...
TRANSCRIPT
Acids and Bases: an Introduction
Sour Taste Electrolytes Identified by the presence of H+
ions (Arrhenius). Proton (H+) donor (Bronsted-
Lowry). Common Acids: vinegar, citric
acid, sulfuric acid, hydrochloric acid.
Acids
An acid H+ in waterAn acid H+ in water
ACIDS
HNO3, nitric acidHNO3
HNO3 H+ + NO3-
Strong acids are strong electrolytes and completely dissociate in water.
An acid H+ in waterAn acid H+ in water
ACIDS
HCl hydrochloricHBr hydrobromicHI hydroiodicHNO3 nitric
H2SO4 sulfuric
HNO3
The following are examples of strong acids.
The Hydronium Ion
HCl
H2O H3O+
Cl-
hydronium ion
Free H+ is highly reactive and does not actually exist in nature. It reacts with water to form the hydronium ion, H3O+.
HCl (aq) H3O+ (aq) + Cl-
(aq)
Weak Acids
WEAK ACIDS are weak electrolytes and do not completely dissociate in water.
CH3CO2H acetic acid
H2CO3 carbonic acid
H3PO4 phosphoric acid
Dissociation of a Weak Electrolyte
Bitter taste Slippery Like acids, they are electrolytes Identified by the presence of OH-
ions (Arrhenius). Proton (H+) acceptor (Bronsted-
Lowry).
Bases
Base OH- in water Base OH- in water
BASES
NaOH(aq) Na+(aq) + OH-
(aq)
NaOH is a strong base
Strong bases are strong electrolytes and soluble in waterStrong bases are strong electrolytes and soluble in water
04m08an104m08an1
Based on the concentration of H+
or OH- ions in a solution. Strong Acids/Bases: completely
dissociate into ions in a solution. Weak Acids/Bases: do NOT
completely dissociate into ions in a solution.
Strength of Acids and Bases
Conjugate Acids/Bases
Acids and bases are related to each other through the addition/loss of hydrogen ions Conjugate acid-base pairs
Acids produce conjugate bases Bases produce conjugate acids
Conjugate Examples
HA + H2O H3O+ + A-
HNO3 + NH3 NH4+ + NO3
-
Conjugate Acid/Base Strength
Stronger the acid, the weaker the conjugate base
Stronger the base, the weaker the conjugate acid
Weak acids/bases have strong conjugate bases/acids
Strong Acid Example: HCl
Weak Acid Example: CH3CO2H
“BIG 6”---Strong Acids
(Know them!!) HClO4
HI HCl HNO3
HBr H2SO4
Strong Bases (Know them!!)
Group I metal hydroxides (NaOH, KOH, etc.)
Soluble/Slightly soluble Group II metal hydroxides ( Ca(OH)2, Sr(OH)2, Ba(OH)2 )
Binary acids– containing only 2 elements (one is
hydrogen) 1) Prefix “hydro—” with binary acid 2) root name for second element 3) End the name with “IC acid”
Oxyacids– acids containing hydrogen, oxygen, and a nonmetal 1) use the given polyatomic ion name from anion 2) add “IC acid”
Acid Nomenclature
Write name
Example 1: HBr
Write name.
Now you try, HCl
Write chemical formula
Example 2: Hydrofluoric acid
Now you try, hydriodic acid.
Write the name.
Example 3: H2SO4
Write the name.
Example 4: HClO2
HClO3
HClO HClO4
Try:
Name of cation, name of
anion/hydroxide
Ex. NaOH
Base Nomenclature
Briefly brainstorm how we
measure the amount of hydrogen ions in a solution? How can we quickly measure the acidity or basicity of a solution?
Brainstorm…