# AP Chemistry : Solubility and Equilibrium

## Example Questions

### Example Question #1 : Solubility And Equilibrium

Calculate the molar solubility of AgBr in 0.050 M AgNO3 at room temperature.  The Ksp of AgBr is 5.4 x 10-13.

1.57 x 10-12 M

1.08 M

2.16 M

2.16 x 10-11 M

1.08 x 10-11 M

1.08 x 10-11 M

Explanation:

### Example Question #2 : Solubility And Equilibrium

Would the molar solubility of Cr(OH)3 increase or decrease as the pH is lowered (i.e. made more acidic)?

Can not be determined

Increase

There is no change

Decrease

Increase

Explanation:

Since Cr(OH)3 is a basic salt, decreasing the pH makes it more soluble.

### Example Question #1 : Solubility And Equilibrium

Calculate the molar solubility of SrF2 in 0.023M NaF.  The Ksp for SrF2 is 4.3 x 10-9.

5.2 x 10-4 M

8.1 x 10-6 M

3.2 x 10-3 M

3.2 x 10-5 M

1.6 x 10-3  M

8.1 x 10-6 M

Explanation:

### Example Question #1 : Solubility And Equilibrium

Calculate the molar solubility of Mn(OH)2 at pH 9.5.  The Ksp for Mn(OH)2 is 1.6 x 10-13.

1.6 x 10-4 M

2.4 x 10-3 M

2.1 x 10-5 M

1.5 x 10-3 M

3.5 x 10-4 M

1.6 x 10-4 M

Explanation:

### Example Question #1 : Solubility And Equilibrium

Calculate the molar solubility of CaF2 (Ksp  = 3.9 x 10-11) in a room temperature solution of 0.010 M Ca(C2H3O2)2.

1.6 x 10-2 M

3.7 x 10-4 M

3.1 x 10-5 M

3.2 x 10-2 M

4.2 x 10-4M