Skip to main content
8: Acids and Bases, Equilibrium, and Buffers
-
-
Last updated
-
-
Save as PDF
-
-
-
8.1: Acid and Base Neutralization
-
When an acid and a base are combined, a double displacement reaction called neutralization reaction takes place and water and a salt are the products.
-
-
8.2: Acids-Properties and Examples
-
Acids are are all around us. Oranges and lemons contain citric acid and ascorbic acid (vitamin C). Carbonated sodas contain carbonic acid. Vinegar contains acetic acid. Stomach acid is hydrochloric acid required for the digestion of food.
-
-
8.3: Bases-Properties and Examples
-
A base is commonly referred to as any substance that can neutralize an acid, feel slippery to the touch when in solution, and taste bitter.
-
-
8.4: Brønsted-Lowry Theory of Acids and Bases
-
A Brønsted-Lowry acid is a proton donor, while a Brønsted-Lowry base is a proton acceptor.
-
-
8.5: Equilibrium
-
When the speed of the reverse reaction equals the speed of the forward reaction, the reaction has reached chemical equilibrium.
-
-
8.6: Acid and Base Strength
-
Acids and bases can be strong or weak depending on the extent of ionization in solution.
-
-
8.7: Ionization of Water and The pH Scale
-
A pH value is the negative of the logarithm of the hydronium ion concentration. The pH scale is used to communicate the acidity or basicity of a solution.
-
-
8.8: Le Châtelier’s Principle
-
Le Châtelier's principle explains changes to the position of equilibrium if you change the concentrations of reactants and products.
-
-
8.9: Blood Buffers
-
A buffer is a solution that resists sudden changes in pH. The pH of the blood is maintained between 7.35 and 7.45 by an important buffer system made of carbonic acid and the bicarbonate anion.
-
-
8.10: Compensation of pH via Organs
-
To maintain a constant serum pH the body relies on the control the hydronium ion concentrations by the involvement of the organs such as lungs and the kidneys.
-
-
8.11: End of Chapter Problems
-
This problem set is based on Chapter 8 topics.