Ksp - Solubility Product Constant

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 product constant of calcium chlorate, Ca(ClO₃)₂ of water is 7.1 x 10^-7 at 25 ^oC. How many grams of Ca(ClO₃)₂ were dissolved in 750mL?

• 3.61 x 10⁵ g

• 2.03 x 10^-5 g

• 8.72 x 10^-1 g

• 3.61 x 10^-5 g

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