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 solution Acid 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. HCl 2. HBr 3. HI 4. HNO 3 5. H 2 SO 4 6. HClO 4 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: LiOH KOH Ca(OH) 2 Sr(OH) 2 Ba(OH) 2
Produce OH - ions by reacting with the water. NH 3 aq + H 2 O aq NH 4 + 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 NH 3 amides R-NH 2 Weak 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 Hydroxide H + + NO 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 Acid NH 3 + H + + Cl - NH Cl - Methylamine and Nitric Acid CH 3 NH 2 + H + CH 3 NH 3 +
Poem That Makes Sense After Studying Predicting Reactions: Johnny finding life a bore, drank some H 2 SO 4. Johnny's father, an M.D., gave him CaCO 3. Johnny's neutralized, it's true, But now he's full of CO 2.
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 n OH - = n H + If 25.00mL of M NaOH is needed to react with mL of HCl. What is the molarity of HCl? 1. Write the reaction 2. Use M 1 V 1 =M 2 V 2 In this case the formula could be written M OH - V OH - = M H + V H +
Arrhenius: Acids put H+ into water Bases put OH- into water Bronsted-Lowry Acids: “ADP” Acids donate protons Bases accept protons