Solubility

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

What is the K_sp expression for an ionic compund of BaSO₄

• K_sp= [Ba²⁺][SO₄^2-]

• K_sp= [Ba²⁺][4SO₄^2-]⁴

• K_sp= [Ba²⁺][4SO₄^2-]

• K_sp= [2Ba²⁺][4SO₄^2-]

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

The solubility product of silver chromate (VI) at room temperature is 2.4 x 10^-12. Calculate the molar solubility of Ag⁺_(aq) and CrO₄^2-_(aq) ions in a saturated solution of silver chromate (VI) at room temperature.

• Ag⁺ = 1.68 x 10⁴ M and CrO₄^2- = 8.4 x 10^-5 M

• Ag⁺ = 1.68 x 10⁴ M and CrO₄^2- = 8.4 x 10⁵ M

• Ag⁺ = 1.68 x 10^-4 M and CrO₄^2- = 8.4 x 10⁵ M

• Ag⁺ = 1.68 x 10^-4 M and CrO₄^2- = 8.4 x 10^-5 M

Tags

NGSS.HS-PS1-7

What will happen if some solid AgNO₃ is added to a saturated solution of AgCl ?

• The AgNO₃ will not dissolve

• More solid AgCl will dissolve

• More solid AgCl will produced

• There will be no effect on AgCl equilibrium

Tags

NGSS.HS-PS1-5

The K_sp value for PbF₂ is 4 x 10^-8. Calculate the molar solubility of solid PbF₂ in a 0.5M NaF solution.

• 8 x 10⁸

• 1.6 x 10⁷

• 8 x 10^-8

• 1.6 x 10^-7

A person mixes 100.0 mL of 0.0015M CaCl₂ and 50.0 mL of 0.0081M K₂SO₄. If the K_sp for CaSO₄ is 2.4 x 10^-5 , will a CaSO₄ precipitate be observed?

• No precipitate occur

• Precipitate occur

Tags

NGSS.HS-PS1-7

The solubility of CuI is 2 × 10^–6 molar. What is the solubility product constant, Ksp, for CuI?

• 1.4 × 10^–3

• 2 × 10^–6

• 4 × 10^–12

• 2 × 10^–12

Tags

NGSS.HS-PS1-7

Which of the following statements is held true about the common-ion effect on the equilibrium of solubility of salt ?

(you may choose more than one answer)

• Adding common-ion to the solution containing dissolved salt cause the solubility equilibrium shifts to the formation of undissolved salt

• Adding common-ion to the solution containing dissolved salt cause the numerical value of Ksp of corresponding salt changes

• Solubility of salt in solution containing common-ion is greater than that of pure water.

Consider a beaker containing 100 ml of water, with solid AgCl on the bottom.

Which of the following statements is held true if NaCl is added to the solution?

(you may choose more than one answer)

• The amount of AgCl solid at the bottom of the beaker increases

• The amount of AgCl solid at the bottom of the beaker decreases

• The concentration of dissolved Ag⁺ ion in the solution stays the same

• The concentration of dissolved Ag⁺ ion in the solution changes

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7