Solubility equilibrium

The concentration of OH– in a saturated solution of Mg(OH)₂ is 3.6 x 10^–4 M. The Ksp of Mg(OH)₂ is

• 1.3 x 10^–7

• 4.7 x 10^–11

• 3.6 x 10^–4

• 2.3 x 10^–11

The correct mathematical expression for finding the molar solubility (X) of Sn(OH)₂ is:

• 2(X)³ = Ksp

• 108(X)⁵ = Ksp

• 4(X)³ = Ksp

• 8(X)³ = Ksp

Barium carbonate has a measured solubility of 4.0 x 10^–5 at 25°C. Determine the Ksp.

• 5.3 x 10^–10

• 6.1 x 10^–5

• 9.1 x 10^–7

• 1.6 x 10^–9

The [IO₃^–] in a saturated solution of Ce(IO₃)₃ is 5.55 x 10^–3 M. Calculate the Ksp for Ce(IO₃)₃.

• 3.16 x 10^–10

• 1.03 x 10^–5

• 2.56 x 10^–8

• 3.51 x 10^–11

Determine the concentration of the Ag+ ion in a saturated solution of silver phosphate (Ag₃PO₄). The solubility of silver phosphate at 25°is 1.6 x 10^–5 mol/L.

• 1.6 x 10^–5 M

• 3.2 x 10^–5 M

• 4.8 x 10^–5 M

• 6.4 x 10^–5 M

Tags

NGSS.HS-PS1-5

The molar solubility of PbI₂ is 1.5 x 10^-3 M. Calculate the value of Ksp for PbI₂.

• 1.5 x 10^-3

• 2.3 x 10^-6

• 1.4 x 10^-8

• 3.4 x 10^-9

What is the equilibrium expression for the solubility product (K_sp) of the following salt :

MgCO₃

• K_sp = [Mg²⁺] [CO₃^-]

• K_sp = [Mg²⁺] [CO₃^2-]

• K_sp = [Mg²⁺]² [CO₃^2-]

• K_sp = [Mg²⁺] [CO₃^2-]²

What is the equilibrium expression for the solubility product (K_sp) of the following salt :

Al(OH)₃

• K_sp = [Al⁺] [OH^-]³

• K_sp = [Al²⁺] [OH^-]³

• K_sp = [Al⁺]³ [OH^3-]

• K_sp = [Al³⁺] [OH^-]³

What is the equilibrium expression for the solubility product (K_sp) of the following salt :

Fe₂S₃

• K_sp = [Fe²⁺]³ [S^3-]²

• K_sp = [Fe⁺]² [S^-]³

• K_sp = [Fe³⁺]² [S^2-]³

• K_sp = [Fe²⁺] [S^3-]

Which of the following equation represents the equilibrium equation of solubility of BaSO₄ in water ?

• BaSO₄(s) ↔ Ba²⁺(aq) + 2SO₄^-(aq)

• BaSO₄(s) ↔ Ba⁺(aq) + 4SO^-(aq)

• BaSO₄(s) ↔ Ba⁺(aq) + SO₄^-(aq)

• BaSO₄(s) ↔ Ba²⁺(aq) + SO₄^2-(aq)