Solubility Product Constant (Ksp) Definition and Calculation Quiz

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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)?

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?

[Ag+] [Cl-] (correct)

[Ag+] [Cl-]^2

[Ag+]^2 [Cl-]

[Ag+]^2 [Cl-]^2

What is the solubility product constant (Ksp) expression for Ag2CrO4?

[Ag+]^2 [CrO4^2-] Signup and view all the answers

What is the general formula for the solubility product constant (Ksp) of a sparingly soluble salt AnBm?

Ksp_AnBm = [A^m+]^n [B^n-]^m Signup and view all the answers

Which statement is true regarding the effect of pH on solubility?

The solubility of many compounds decreases at low pH. Signup and view all the answers

True or false: Sparingly soluble salts will precipitate when the ionic product exceeds the solubility product constant (Ksp).

True Signup and view all the answers

In the presence of Ag+, which precipitate will form first when Cl- and I- ions are present?

AgI Signup and view all the answers

What is the correct relationship between the [Cl-] and [I-] ions for AgCl and AgI to precipitate simultaneously?

[Cl-] : [I-] = 1 : 106 Signup and view all the answers

Which factor enhances the solubility of salts of weak acids?

Formation of free weak acid molecules Signup and view all the answers

If the solubility of Pb3(PO4)2 is 0.00014 g/L, what is the solubility product constant (Ksp) for Pb3(PO4)2?

$2.33 \times 10^{-16}$ Signup and view all the answers

What is a characteristic of fractional precipitation when Ag+ is added to a solution containing both Cl- and I- ions?

Iodide will precipitate first due to lower solubility. Signup and view all the answers

If the solubility of AgCl is 1.05 x 10^-10 mol/L, what is the solubility product constant (Ksp) of AgCl?

1.05 x 10^-10 Signup and view all the answers

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?

1.5 x 10^-32 Signup and view all the answers

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?

0.00116 g/L Signup and view all the answers

According to Le Chatelier's principle, the presence of a common ion in a solution will:

Decrease solubility Signup and view all the answers

The theory of interionic attraction explains that a diverse ion in a solution:

Stabilizes the precipitate in its ionic form Signup and view all the answers

True or False: Increasing temperature increases the solubility of most inorganic salts.