"Acid strength is the tendency of an acid... to dissociate into a proton... and an anion..." (Acid strength is the tendency of an acid to dissociate into a proton and an anion)
These are acids that do not dissociate completely in aqueous solutions, and have a lower tendency to donate protons. Examples include acetic acid (CH3COOH), carbonic acid (H2CO3), and formic acid (HCOOH).
Definition of Weak Acids: Understanding the basic concept of weak acids and comparing them with strong acids. Weak acids partially dissociate in water giving less H+ ions while strong acids dissociate completely to give many H+ ions.
pH Scale and Acid Strength: Introduction to the pH scale and understanding the relationship between pH and acid strength. The lower the pH, the stronger the acid.
Acid Dissociation Constant (Ka): Acid dissociation constant represents the extent to which an acid dissociates in water. A higher value of Ka represents a stronger acid.
Equilibrium Constant (Keq): Understanding the equilibrium constant and how to calculate it using the concentrations of the products and reactants.
Buffer Solutions: Understanding the concept of buffer solutions, their definition, and the importance of buffering capacity in regulating pH.
Acid-Base Equilibria: Understanding the relationship between weak acids and their conjugate bases and how they equilibrate in water.
Henderson-Hasselbalch equation: A formula to calculate the pH of a buffer solution.
Acid-Base Titration: A technique used to determine the concentration of an unknown acid or base by adding a known solution of the opposite reaction to reach the equivalence point.
Acid Strength Trends: Trends in the strengths of acids based on their molecular properties, such as electronegativity and bond polarity.
Polyprotic Acids: Weak acids with two or more dissociable protons, including their definitions, equations, and calculations.
Acid-Base Indicators: Compounds that change color in response to pH changes, used to determine the pH of a solution.
Common Weak Acids: A brief description of common weak acids, including acetic acid, formic acid, and hydrogen sulfide.
Lewis Acid-Base Theory: A theory that describes the bonding interactions between molecules, including those involving weak acids.
Acid-Base Reactions: Understanding the basic concepts behind acid-base reactions and equilibria, including Bronsted-Lowry acid-base theory.
Strong Bases: Comparing and contrasting strong bases with weak bases and weak acids with strong acids, including common examples such as NaOH and NH3.
Carboxylic acids: Organic acids that contain a carboxyl group (-COOH), which dissociates partially in water to form H+ ions. Examples include acetic acid, formic acid, and butyric acid.
Mineral acids: Inorganic acids that ionize in water to form H+ ions. Examples include hydrochloric acid, sulfuric acid, and nitric acid.
Phenols: Organic compounds that contain an -OH group attached to a benzene ring. They are weak acids that dissociate partially in water to form H+ ions. Examples include phenol, cresol, and thymol.
Hydrogen halides: Binary compounds of hydrogen and a halogen (fluorine, chlorine, bromine, or iodine) that are acidic in nature. They ionize in water to form H+ ions and a halide ion. Examples include hydrofluoric acid, hydrochloric acid, and hydrobromic acid.
Ammonia and amines: Ammonia (NH3) and amines (organic compounds with an -NH2 group) are weak bases that can act as weak acids in certain conditions. They can accept a proton (H+) to form ammonium ions. Examples include ammonia, methylamine, and ethylamine.
Boric acid: An inorganic acid that is weak and only partially ionizes in water. It is commonly used as an antiseptic and insecticide.
Hydrosulfuric acid: An inorganic acid that is a gas at room temperature and has a pungent smell. It ionizes in water to form H+ ions and sulfide ions.
Carbonic acid: An inorganic weak acid that is formed when carbon dioxide dissolves in water. It dissociates partially in water to form bicarbonate ions and hydrogen ions.
"The dissociation of a strong acid in solution is effectively complete..." (The dissociation of a strong acid in solution is effectively complete)
"Examples of strong acids are hydrochloric acid (HCl), perchloric acid (HClO4), nitric acid (HNO3), and sulfuric acid (H2SO4)." (Examples of strong acids are hydrochloric acid, perchloric acid, nitric acid, and sulfuric acid)
"A weak acid is only partially dissociated..." (A weak acid is only partially dissociated)
"Acetic acid (CH3COOH) is an example of a weak acid." (Acetic acid is an example of a weak acid)
"The strength of a weak acid is quantified by its acid dissociation constant, Ka value." (The strength of a weak acid is quantified by its acid dissociation constant, Ka value)
"The strength of a weak organic acid may depend on substituent effects." (The strength of a weak organic acid may depend on substituent effects)
"The strength of an inorganic acid is dependent on the oxidation state for the atom to which the proton may be attached." (The strength of an inorganic acid is dependent on the oxidation state for the atom)
"Acid strength is solvent-dependent." (Acid strength is solvent-dependent)
"For example, hydrogen chloride is a strong acid in aqueous solution, but is a weak acid when dissolved in glacial acetic acid." (Hydrogen chloride is a strong acid in aqueous solution, but is a weak acid when dissolved in glacial acetic acid)