Ionic equilibrium is a subtopic of physical chemistry which deals with the dynamic balance between the ionised and unionised molecules of an electrolyte solution. It is the equilibrium between the cations and anions in a solution.
What is meant by the term 'strong electrolyte' in Ionic Equilibrium?
A strong electrolyte is a solution that is completely ionized or dissociated in water, meaning that all of the solute is present as separated ions. Examples include HCl, NaOH, and HNO3.
What is the relationship between pH, pOH and the product of the concentration of H+ and OH- ions for a neutral solution?
pH + pOH = 14 and [H+] x [OH-] = 1 x 10^-14 for a neutral solution.
What is the Henderson-Hasselbalch equation?
The Henderson-Hasselbalch equation is an equation that relates the pH or pOH of a buffer solution to the dissociation constant and the ratio of the concentration of the conjugate base to the concentration of the weak acid or vice versa. It is commonly used in buffer calculations.
What is the definition of a buffer solution in Ionic Equilibrium?
Buffer solutions are solutions that resist changes in pH upon addition of small amounts of acid or base. They are usually a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid.
What is the significance of the Kw value in Ionic Equilibrium?
The Kw value is the ion product constant for water and it is used to describe the equilibrium between hydrogen ions (H+) and hydroxide ions (OH-) in aqueous solutions. It is used to calculate the pH or pOH of a solution.
What is the difference between a strong acid and a weak acid in Ionic Equilibrium?
A strong acid is an acid that is completely ionised in water, meaning that all of the acid molecules dissociate into ions. A weak acid is an acid that only partially dissociates into ions in an aqueous solution.
What is the common-ion effect in Ionic Equilibrium?
The common-ion effect is the effect on the equilibrium of a solution caused by the addition of an ion that already exists in the solution. It causes the equilibrium to shift towards the opposite side of the ion that was added.
What is the Bronsted-Lowry acid and base theory in Ionic Equilibrium?
The Bronsted-Lowry acid and base theory is a theory of acids and bases that defines an acid as a proton (H+) donor and a base as a proton acceptor. It is a more general theory than the Arrhenius theory of acids and bases.
What is the Arrhenius acid and base theory in Ionic Equilibrium?
The Arrhenius acid and base theory is a theory of acids and bases that defines an acid as a substance that increases the concentration of hydrogen ions (H+) in aqueous solution and a base as a substance that increases the concentration of hydroxide ions (OH-) in aqueous solution.
What is the definition of a salt in Ionic Equilibrium?
A salt is a compound that is formed when the hydrogen ion of an acid is replaced by a metal ion or another positive ion. It is a product of a neutralization reaction between an acid and a base.
What is the definition of a weak electrolyte in Ionic Equilibrium?
A weak electrolyte is a solute that only partially ionizes or dissociates in water. Examples include acetic acid, carbonic acid, and ammonia.
What is the definition of a strong base in Ionic Equilibrium?
A strong base is a base that is completely ionized or dissociated in water, meaning that all of the solute is present in the form of separated ions. Examples include NaOH, KOH, and Ca(OH)2.
What is the definition of solubility product in Ionic Equilibrium?
Solubility product is the equilibrium constant for a chemical reaction in which a solid ionic compound dissolves in water to form its respective ions. It is used to determine the solubility of a substance in a solution.
What is the common-ion effect in Ionic Equilibrium?
The common-ion effect is the effect on the equilibrium of a solution caused by the addition of an ion that already exists in the solution. It causes the equilibrium to shift towards the opposite side of the ion that was added.
What is the definition of ionic equilibrium?
Ionic equilibrium is a subtopic of physical chemistry which deals with the dynamic balance between the ionised and unionised molecules of an electrolyte solution. It is the equilibrium between the cations and anions in a solution.
What is meant by the term 'strong electrolyte' in Ionic Equilibrium?
A strong electrolyte is a solution that is completely ionized or dissociated in water, meaning that all of the solute is present as separated ions. Examples include HCl, NaOH, and HNO3.
What is the relationship between pH, pOH and the product of the concentration of H+ and OH- ions for a neutral solution?
pH + pOH = 14 and [H+] x [OH-] = 1 x 10^-14 for a neutral solution.
What is the Henderson-Hasselbalch equation?
The Henderson-Hasselbalch equation is an equation that relates the pH or pOH of a buffer solution to the dissociation constant and the ratio of the concentration of the conjugate base to the concentration of the weak acid or vice versa. It is commonly used in buffer calculations.
What is the definition of a buffer solution in Ionic Equilibrium?
Buffer solutions are solutions that resist changes in pH upon addition of small amounts of acid or base. They are usually a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid.
What is the significance of the Kw value in Ionic Equilibrium?
The Kw value is the ion product constant for water and it is used to describe the equilibrium between hydrogen ions (H+) and hydroxide ions (OH-) in aqueous solutions. It is used to calculate the pH or pOH of a solution.
What is the difference between a strong acid and a weak acid in Ionic Equilibrium?
A strong acid is an acid that is completely ionised in water, meaning that all of the acid molecules dissociate into ions. A weak acid is an acid that only partially dissociates into ions in an aqueous solution.
What is the common-ion effect in Ionic Equilibrium?
The common-ion effect is the effect on the equilibrium of a solution caused by the addition of an ion that already exists in the solution. It causes the equilibrium to shift towards the opposite side of the ion that was added.
What is the Bronsted-Lowry acid and base theory in Ionic Equilibrium?
The Bronsted-Lowry acid and base theory is a theory of acids and bases that defines an acid as a proton (H+) donor and a base as a proton acceptor. It is a more general theory than the Arrhenius theory of acids and bases.
What is the Arrhenius acid and base theory in Ionic Equilibrium?
The Arrhenius acid and base theory is a theory of acids and bases that defines an acid as a substance that increases the concentration of hydrogen ions (H+) in aqueous solution and a base as a substance that increases the concentration of hydroxide ions (OH-) in aqueous solution.
What is the definition of a salt in Ionic Equilibrium?
A salt is a compound that is formed when the hydrogen ion of an acid is replaced by a metal ion or another positive ion. It is a product of a neutralization reaction between an acid and a base.
What is the definition of a weak electrolyte in Ionic Equilibrium?
A weak electrolyte is a solute that only partially ionizes or dissociates in water. Examples include acetic acid, carbonic acid, and ammonia.
What is the definition of a strong base in Ionic Equilibrium?
A strong base is a base that is completely ionized or dissociated in water, meaning that all of the solute is present in the form of separated ions. Examples include NaOH, KOH, and Ca(OH)2.
What is the definition of solubility product in Ionic Equilibrium?
Solubility product is the equilibrium constant for a chemical reaction in which a solid ionic compound dissolves in water to form its respective ions. It is used to determine the solubility of a substance in a solution.
What is the common-ion effect in Ionic Equilibrium?
The common-ion effect is the effect on the equilibrium of a solution caused by the addition of an ion that already exists in the solution. It causes the equilibrium to shift towards the opposite side of the ion that was added.