Which of the following solubility product expressions is incorrect?

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1. 2.

3.

4. 5.

Calculate the solubility product constant for lead fluoride, PbF2. Its molar solubility is 2.1 x 10-3 mole per liter at 25°C.

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1. 4.4 x 10-6

2. 4.2 x 10-7

3. 9.3 x 10-7

4. 9.3 x 10-9

5. 3.7 x 10-8

The solubility of bismuth sulfide is 1.8 x 10-5 g/100. mL of water at 18°C. Calculate the Kspfor Bi2S3 at 18°C.

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1. 6.0 x 10-36

2. 3.4 x 10-23

3. 5.7 x 10-31

4. 5.8 x 10-12

5. 3.2 x 10-8

Calculate the molar solubility of aluminum hydroxide at 25°C. Its Kspis 1.9 x 10-33.

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1. 1.2 x 10-9 M

2. 4.2 x 10-15 M

3. 2.9 x 10-9 M

4. 4.4 x 10-14 M

5. 9.3 x 10-9 M

How many grams of AgCl will dissolve in 1.0 L of 0.25 M KCl? Ksp (AgCl)= 1.8 x 10-10

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1. 1.0 x 10-7

2. 2.6 x 10-8

3. 6.4 x 10-9

4. 7.8 x 10-8

5. 2.5 x 10-9

If NaCl is added to a 0.010 M solution of AgNO3in water at 25°C, at what [Cl-] does precipitation of AgCl begin? Ksp for AgCl = 1.8 x 10-10.

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1. 1.0 x 10-10 M

2. 1.3 x 10-6 M

3. 1.8 x 10-8 M

4. 1.8 x 10-12 M

5. 1.3 x 10-10 M

Calculate the concentration of sulfate ion in a saturated solution of barium sulfate to which barium chloride has been added until [Ba+2] = 0.1 M at 25°C. Ksp for BaSO4 = 1 x 10-10.

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1. 1 x 10-5 M

2. 1 x 10-8 M

3. 1 x 10-9 M

4. 1 x 10-7 M

5. 1 x 10-6 M

What is the minimum concentration of bromide ion required to limit the concentration of silver ion in solution to a maximum of 1.0 x 10-9 M? Ksp for AgBr is 3.3 x 10-13.

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1. 1.0 x 10-9 M

2. 3.3 x 10-4 M

3. 1.1 x 10-7 M

4. 5.0 x 10-6 M

5. 3.3 x 10-22 M

Which of the following salts would not be expected to be more soluble in acidic solution than in pure water?

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1. Fe(OH)3

2. FeS

3. ZnCO3

4. AgI

5. Hg2(CH3COO)2

Consider the following system: Some solid AgCl is in contact with its saturated aqueous solution. Gaseous NH3is then bubbled through the solution slowly with swirling until all the AgCl dissolves. Choose the response which includes all the true statements, and no others. I. At the point at which all the AgCl has dissolved [Ag+] = [Cl-]. II. The AgCl dissolves due to formation of the complex ion, [Ag(NH3)2]+. III. As the NH3 is added to the solution, the [Cl-] increases. IV. The solution remains saturated with silver chloride as long as any solid AgCl remains. V. The solubility of silver chloride in aqueous ammonia solution is greater than in pure water.

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1. I, II, and IV

2. II, III, and IV

3. I, IV, and V

4. II and V

5. II, III, IV, and V

Calculate the concentration of free Ni2+ in 1.0 M [Ni(NH3)6](NO3)2 at 25°C. Kd for [Ni(NH3)6]2+ is 1.8 x 10-9.

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1. 1.6 x 10-5 M

2. 0.012 M

3. 3.2 x 10-4 M

4. 0.084 M

5. 4.4 x 10-5 M