Equilibria involving the transfer of protons between species in solution, characterized by the acid dissociation constant, Ka, and the base dissociation constant, Kb.
Properties of acids and bases: This topic covers the definitions, characteristics, and properties of acids and bases. It includes the Brønsted-Lowry and Lewis definitions.
pH and pOH: This topic covers the concept of pH (potential of hydrogen) and pOH (potential of hydroxide). It includes calculations for both and how to determine the concentration of hydrogen ions and hydroxide ions.
Acid-base reactions: This topic covers the different types of acid-base reactions, such as neutralization, proton transfer, and hydrolysis. It includes balancing chemical equations for acid-base reactions.
Acid-base equilibrium constants: This topic covers the equilibrium constants for acid-base reactions, such as Ka (acid dissociation constant) and Kb (base dissociation constant). It includes how to calculate these constants and their significance.
Common ion effect: This topic covers the effect of adding a common ion on an acid-base equilibrium. It includes how to calculate the new equilibrium constant after adding a common ion.
Buffers: This topic covers the concept of buffers, which are solutions that resist changes in pH. It includes how to prepare buffers and how they work.
Titration curves: This topic covers the graphical representation of an acid-base titration. It includes how to calculate the equivalence point and determine the pH at any point during the titration.
Acid-base indicators: This topic covers the use of acid-base indicators to determine the endpoint of a titration. It includes the different types of indicators and their pH ranges.
Acid-base theories: This topic covers the different acid-base theories, such as the Lewis theory and the solvent system theory. It includes their significance and applications.
Acid rain: This topic covers the phenomenon of acid rain, which is caused by air pollution. It includes the chemistry behind acid rain and its environmental impact.
Strong Acid-Strong Base Equilibrium: This is the most common acid-base equilibrium, in which a strong acid reacts with a strong base to produce a salt and water. The reaction completely goes to the right, and the pH of the solution is neutral.
Weak Acid-Strong Base Equilibrium: In this type of equilibrium, a weak acid reacts with a strong base to produce a salt and water. The reaction partially goes to the right, and the pH of the solution is slightly basic.
Strong Acid-Weak Base Equilibrium: Here, a strong acid reacts with a weak base to produce a salt and water. The reaction partially goes to the right, and the pH of the solution is slightly acidic.
Weak Acid-Weak Base Equilibrium: This type of equilibrium involves two weak substances reacting with each other to produce a salt and water. The reaction partially goes to the right or left, depending on the equilibrium constants of the acid and base. The pH of the solution depends on the relative strengths of the acid and base.
Amphiprotic Equilibrium: An amphiprotic substance can act as both an acid and a base when it is in solution. Examples include water (which can donate or accept hydrogen ions) and some amino acids. In this type of equilibrium, the amphiprotic substance reacts with itself to form a conjugate acid-base pair. The equilibrium can lie to the left or right, depending on the relative strengths of the acid and base forms.
Acid-Base Salt Hydrolysis Equilibrium: When an acid or base salt is dissolved in water, it can undergo hydrolysis, where the ions in the salt react with water to produce a weak acid or base. The equilibrium can lie to the left or right, depending on the equilibrium constants of the acid and base and the concentration of water.
Buffer Equilibrium: A buffer is a solution that resists changes in pH when small amounts of acid or base are added. It consists of a weak acid and its conjugate base (or a weak base and its conjugate acid). When an acid or base is added to a buffer, the buffer's equilibrium shifts to minimize the effect on the pH.
Lewis Acid-Base Equilibrium: A Lewis acid is an electron acceptor, while a Lewis base is an electron donor. In this type of equilibrium, a Lewis acid reacts with a Lewis base to form a complex ion. The equilibrium can lie to the left or right, depending on the strengths of the acid and base.