Acids & Bases Properties Acid-Base Theories Acid-Base Reactions.
Acid-Base Reactions
description
Transcript of Acid-Base Reactions
![Page 1: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/1.jpg)
Strong and Weak Acids Titration Common Acid Names
Textbook section 4.3
![Page 2: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/2.jpg)
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)
![Page 3: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/3.jpg)
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.
![Page 4: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/4.jpg)
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.
![Page 5: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/5.jpg)
Strong Bases Ionize Completely
NaOH Na+ + OH-
Hydroxides are commonly strong bases. Including:
LiOHKOHCa(OH)2
Sr(OH)2
Ba(OH)2
![Page 6: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/6.jpg)
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
![Page 7: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/7.jpg)
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
![Page 8: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/8.jpg)
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.
![Page 9: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/9.jpg)
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
![Page 10: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/10.jpg)
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
+
![Page 11: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/11.jpg)
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.
![Page 12: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/12.jpg)
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.
![Page 13: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/13.jpg)
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
+
![Page 14: Acid-Base Reactions](https://reader035.fdocuments.us/reader035/viewer/2022062422/56813b32550346895da3fd89/html5/thumbnails/14.jpg)
Arrhenius: Acids put H+ into water Bases put OH- into water
Bronsted-Lowry Acids:“ADP”
Acids donate protons Bases accept protons