Podcast
Questions and Answers
True or false: The solubility product constant (Ksp) is calculated by taking the product of the concentrations of the ions in a saturated solution of a sparingly soluble salt.
True or false: The solubility product constant (Ksp) is calculated by taking the product of the concentrations of the ions in a saturated solution of a sparingly soluble salt.
- False
- It depends on the stoichiometry of the salt
- True (correct)
- It depends on the solubility of the salt
What is the definition of the solubility product constant (Ksp)?
What is the definition of the solubility product constant (Ksp)?
- The rate at which a sparingly soluble salt dissolves in a given solvent
- The product of the concentrations of the ions in a saturated solution of a sparingly soluble salt (correct)
- The sum of the solubility constants of the ions in a solution
- The ratio of the solute's concentration to the solvent's concentration
What is the solubility product constant (Ksp) expression for AgCl?
What is the solubility product constant (Ksp) expression for AgCl?
- [Ag+] [Cl-] (correct)
- [Ag+] [Cl-]^2
- [Ag+]^2 [Cl-]
- [Ag+]^2 [Cl-]^2
What is the solubility product constant (Ksp) expression for Ag2CrO4?
What is the solubility product constant (Ksp) expression for Ag2CrO4?
What is the general formula for the solubility product constant (Ksp) of a sparingly soluble salt AnBm?
What is the general formula for the solubility product constant (Ksp) of a sparingly soluble salt AnBm?
Which statement is true regarding the effect of pH on solubility?
Which statement is true regarding the effect of pH on solubility?
True or false: Sparingly soluble salts will precipitate when the ionic product exceeds the solubility product constant (Ksp).
True or false: Sparingly soluble salts will precipitate when the ionic product exceeds the solubility product constant (Ksp).
In the presence of Ag+, which precipitate will form first when Cl- and I- ions are present?
In the presence of Ag+, which precipitate will form first when Cl- and I- ions are present?
What is the correct relationship between the [Cl-] and [I-] ions for AgCl and AgI to precipitate simultaneously?
What is the correct relationship between the [Cl-] and [I-] ions for AgCl and AgI to precipitate simultaneously?
Which factor enhances the solubility of salts of weak acids?
Which factor enhances the solubility of salts of weak acids?
If the solubility of Pb3(PO4)2 is 0.00014 g/L, what is the solubility product constant (Ksp) for Pb3(PO4)2?
If the solubility of Pb3(PO4)2 is 0.00014 g/L, what is the solubility product constant (Ksp) for Pb3(PO4)2?
What is a characteristic of fractional precipitation when Ag+ is added to a solution containing both Cl- and I- ions?
What is a characteristic of fractional precipitation when Ag+ is added to a solution containing both Cl- and I- ions?
If the solubility of AgCl is 1.05 x 10^-10 mol/L, what is the solubility product constant (Ksp) of AgCl?
If the solubility of AgCl is 1.05 x 10^-10 mol/L, what is the solubility product constant (Ksp) of AgCl?
If the solubility of Pb3(PO4)2 is 0.00014 g/L and its molar mass is 811.7 g/mol, what is the solubility product constant (Ksp) of Pb3(PO4)2?
If the solubility of Pb3(PO4)2 is 0.00014 g/L and its molar mass is 811.7 g/mol, what is the solubility product constant (Ksp) of Pb3(PO4)2?
What is the solubility of Mg(OH)2 in pure water if its Ksp is 3.4 x 10^-11 and molar mass is 58 g/mol?
What is the solubility of Mg(OH)2 in pure water if its Ksp is 3.4 x 10^-11 and molar mass is 58 g/mol?
According to Le Chatelier's principle, the presence of a common ion in a solution will:
According to Le Chatelier's principle, the presence of a common ion in a solution will:
The theory of interionic attraction explains that a diverse ion in a solution:
The theory of interionic attraction explains that a diverse ion in a solution:
True or False: Increasing temperature increases the solubility of most inorganic salts.
True or False: Increasing temperature increases the solubility of most inorganic salts.
