Download - Acid-Base Reactions
Strong and Weak Acids Titration Common Acid Names
Textbook section 4.3
Defined: ACID
Produces H+
ions in water solution
BASE Produces OH- ions in water solutionAcid Characteristics:
–Sour Taste (lemon)–Change Indicators Colors (litmus blue to red)
Strong Acids Ionize completely.
HCl (aq) H+ (aq) + Cl-
(aq)
The strong ACIDS are:1. HCl2. HBr3. HI4. HNO3
5. H2SO4
6. HClO4
What are the names of these acids?
Check the partner of the “H” for a hint.
These must be memorized.
Weak acids ionize partially.General formula:
HB H+ + B-
Double arrow means reversible or it does not go to completion.
The equilibrium includes both products AND reactants.
Compare # of HCl ions in solution to HF ions in solution. Each w/ 1.0 M concentration.
Strong Bases Ionize Completely
NaOH Na+ + OH-
Hydroxides are commonly strong bases. Including:
LiOHKOHCa(OH)2
Sr(OH)2
Ba(OH)2
Produce OH- ions by reacting with the water.
NH3 aq + H2O aq NH4+
aq + OH-
aq
Pulling an H+, and leaving OH- behind.
We often write water HOH, to easily keep track of this water reaction
Include: ammonia NH3
amides R-NH2Weak bases are weak electrolytes. The bulb will light up but it will be dim
Mix and acid and base what happens?
The results depend upon the strength of the reactants. 3 TYPES:
1 Strong ACID - Strong BASE
2 Weak ACID – Strong BASE 3 Strong ACID – Weak BASE
Neutralization Reaction occurs The products are water, and an
aqueous salt. (ions)Consider Nitric Acid and Sodium
HydroxideH+ + NO3
- + Na+ + OH- Since they are “strong”, they
fully ionize
Animation of Nitric acid and Sodium Hydroxide
Neutralization produces Water and a salt.
Write the complete equation for this reaction
Identify any spectator ions and then write a net ionic equation.
2 step reaction occurs, The acid HF partially
dissociates to H+ + F-
Then the Base NaOH, which has dissociated to produce OH- ions (plus the Na+ ions)
The H+ and OH- combine to from water
The weak base gets “protonated”The strong acid is already dissociated into H+ and B-.
Consider ammonia and Hydrochloric AcidNH3 + H+ + Cl- NH4
+ + Cl-
Methylamine and Nitric AcidCH3NH2 + H+ CH3NH3
+
Poem That Makes Sense After Studying Predicting Reactions:Johnny finding life a bore, drank some H2SO4.Johnny's father, an M.D., gave him CaCO3.Johnny's neutralized, it's true,But now he's full of CO2.
An standardized acid (known concentration) may be used to determine the unknown strength of a base. (or visa-versa)
Using an indicator (solution that changes color)
you can know when the added solution is exactly equal to the unknown.
this is known as the EQUILVALENCE POINT.
Objective: Determine the equivalence point.
Equivalence point nOH- = nH
+
If 25.00mL of 0.0800M NaOH is needed to react with 10.00 mL of HCl. What is the molarity of HCl?
1. Write the reaction2. Use M1V1=M2V2
In this case the formula could be written MOH- VOH
- = MH+VH
+
Arrhenius: Acids put H+ into water Bases put OH- into water
Bronsted-Lowry Acids:“ADP”
Acids donate protons Bases accept protons