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