Ksp and Solubility Product Constant

What is the solubility product constant, Ksp, used for?

• Measuring the pH of a solution

• Determining the solubility of a compound in a saturated solution

• Calculating the boiling point of a liquid

• Estimating the density of a solid

What does the term "maximum quantity" refer to in molar solubility?

• The least amount of solute that can dissolve

• The greatest amount of solute that can dissolve

• The average amount of solute that can dissolve

• The exact amount of solute that must dissolve

What is the concentration of Ag⁺ ions at equilibrium?

• 2.6x10⁻⁴ M

• 1.3x10⁻⁴ M

• 8.8x10⁻¹² M

• 5.2x10⁻⁴ M

What is the expression for Ksp in terms of x for Cu(OH)₂?

• (x)(2x)²

• (x)(x)²

• (2x)(2x)²

• (x)(3x)²

What is the final step in calculating the molar solubility of Cu(OH)₂?

• Taking the cube root of 4.0 x 10⁻²⁰

• Multiplying by 2

• Dividing by 4

• Adding 1.6 x 10⁻¹⁹

What is the unit for molar solubility?

• M (mol/L)

• g/L

• mol

• L/mol

What happens when two aqueous solutions containing dissolved ions are mixed?

• A precipitate may form.

• The solutions will always remain clear.

• The ions will evaporate.

• The solutions will become acidic.

What does the term "equilibrium" mean in the context of Q = Ksp?

• The solution is boiling

• The solution is freezing

• The rates of dissolution and precipitation are equal

• The solution is evaporating

The K_sp expression for a saturated solution of Ca₃(PO₄)₂ is

• K_sp = [Ca²⁺][PO₄^3-]

• K_sp = [3Ca²⁺][2PO₄^3-]

• K_sp = [Ca²⁺]³[PO₄^3-]²

• K_sp = [3Ca²⁺]³[2PO₄^3-]²

The molar solubility of silver sulphide is 5.0 x 10^-17 mol/L. Calculate its solubility product.

• K_sp = 5 x 10⁴⁹

• K_sp = 5 x 10³³

• K_sp = 5 x 10^-49

• K_sp = 5 x 10^-33