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

Which of the following compounds has the lowest molar solubility in mol/L in water at 25°C?

• Ag₃PO₄ Ksp = 1.8 x 10^–18

• Sn(OH)₂ Ksp = 5 x 10^–26

• CdS Ksp = 3.6 x 10^–29

• Al(OH)₃ Ksp = 2 x 10^–33

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

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 x 10^-7, 1,6 x 10^-10, and 2.0 x 10^-13, respectively. Which compound will precipitate first?

• CuCl(s)

• AgCl(s)

• AuCl(s)

• All will precipitate at the same time.

Tags

NGSS.HS-PS1-2

If 30 mL of 5.0 x 10^-4 M Ca(NO₃)₂ are added to 70 mL of 2.0 x 10^-4 M NaF, will a precipitate occur? (Ksp of CaF₂ = 4.0 x 10^–11)

• No, because the ion product (Qsp) is greater than Ksp.

• Yes, because the ion product (Qsp) is less than Ksp.

• No, because the ion product (Qsp) is less than Ksp

• Yes, because the ion product is (Qsp) greater than Ksp.

How many moles of Ca(NO₃)₂ must be added to 1.0 L of a 0.100 M HF solution to begin precipitation of CaF₂ (s)? For CaF₂, Ksp = 4.0 x 10^–11.

• 5.8 x 10^–7

• 1.6 x 10^–9

• 7.0 x 10^–11

• 4.0 x 10^–9

Tags

NGSS.HS-PS1-7

Will precipitation occur when 3.5 x 10² mL of 3.2 M Pb(NO₃)² and 2.0 x 10² mL of 0.020 M NaCl are added together. Ksp for the lead chloride is 1.6 x 10^–5.

• Yes, Q_sp is greater than K_sp

• No, Q_sp is less than K_sp

• Maybe, it depends on the temperature.

• Maybe, it depends on the limiting reagent

Tags

NGSS.HS-PS1-5

A 300.0-mL saturated solution of copper(II) periodate, Cu(IO₄)₂, contains 0.44 grams of dissolved salt. Determine the Ksp.

• 1.4 x 10^–7

• 6.72 x 10^–7

• 9.2 x 10^–6

• 6.1 x 10^–5

Calculate the solubility of Ca₃(PO₄)₂(s) (Ksp = 1.3 x 10^–32) in a 1.0 x 10^–2 M Ca(NO₃)₂ solution.

• 5.7 x 10^–14 mol/L

• 6.2 x 10^–7 mol/L

• 1.6 x 10^–14 mol/L

• 3.16 x 10^–12 mol/L