AP Chemistry

What is the molar solubility in water of Ag₂CrO₄ ? (The Ksp for Ag₂CrO₄ is 8 x 10^-12.) (Topic 7.11)

• 8 x 10^-12 M

• 2 x 10^-12 M

• 
• 
• 

Tags

NGSS.HS-PS1-2

Based on the K_sp values in the table above, a saturated solution of which of the following compounds has the highest [CI^-]? (Topic 7.11)

• PbCl₂

• CuCl

• AgCl

• Hg₂Cl₂

Tags

NGSS.HS-PS1-4

NGSS.HS-PS1-5

How many moles of NaF must be dissolved in 1.00 liter of a saturated solution of PbF₂ at 25˚C to reduce the [Pb²⁺] to 1 x 10^–6 molar?

(Ksp PbF₂ at 25˚C = 4.0 x 10^–8) (Topic 7.12)

• 0.020 mole

• 0.040 mole

• 0.10 mole

• 0.20 mole

• 0.40 mole

CuBr(s)⇄Cu⁺(aq)+Br⁻(aq)

Shown above is the chemical equation for the dissolution of the slightly soluble salt CuBr(s). Its K_sp value in pure water was experimentally determined. CuBr

was found to be much less soluble in a 0.001MNaBr

solution than in pure water. Which of the following correctly explains the decrease in solubility of CuBr in 0.001 M NaBr? (Topic 7.12)

• The concentration of water is much less in the NaBr

  solution than in pure water, reducing the rate of dissolution of the salt.

• The presence of additional Br⁻ ions already in the solution means equilibrium will be reached when much less CuBr has dissolved..

• The presence of additional Br⁻ already in the solution decreases the value of the Ksp for CuBr, causing the solubility to decrease.

• The presence of Na⁺ ions in the solution inhibits the dissolution of salts

Tags

NGSS.HS-PS1-5

Mg(OH)₂(s) ⇄ Mg²⁺(aq) + 2 OH^- (aq)

The exothermic dissolution of Mg(OH)₂(s) in water is represented by the equation above. The Ksp of Mg(OH)2 is 1.8 x 10^-11. Which of the following changes will increase the solubility of Mg(OH)₂ in an aqueous solution? (Topic 7.13)

• Decreasing the pH

• Increasing the pH

• Adding NH₃ to the solution

• Adding Mg(NO₃)₂ to the solution

High solubility of an ionic solid in water is favored by which of the following conditions?

I. The existence of strong ionic attractions in the crystal lattice

II. The formation of strong ion-dipole attractions

III. An increase in entropy upon dissolving (Topic 7.14)

• I only

• I and II only

• I and III only

• II and III only

• I, II, and III