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In this lesson, we will learn how to calculate the molar solubility of an ionic solid from its molecular formula and solubility product.

Q1:

The 𝐾 s p of silver iodide, A g I , is 1 . 5 × 1 0 − 1 6 . What is the molar solubility of silver iodide?

Q2:

Calomel, H g C l 2 2 , is a compound composed of the diatomic ion of mercury(I), H g 2 2 + , and chloride ions, C l – . Although most mercury compounds are now known to be poisonous, eighteenth-century physicians used calomel as a medication. Their patients rarely suffered any mercury poisoning from the treatments because calomel is quite insoluble: What is the molar solubility of H g C l 2 2 ?

Q3:

Which of the following calcium salts is the most soluble, in moles per liter?

Q4:

The 𝐾 s p of Milk of Magnesia ( M g ( O H ) ) 2 is 7 . 1 × 1 0 . How many grams of Milk of Magnesia would be soluble in 200 mL of water at 2 5 ∘ C ?

Q5:

Solutions of H g I 2 2 contain H g 2 2 + and I – ions. What is the molar solubility of H g I 2 2 , given that its solubility product, 𝐾 s p , is 4 . 5 × 1 0 ? Assume that dissolution is the only process affecting the value of 𝐾 s p .

Q6:

What is the molar solubility of A g [ F e ( C N ) ] 4 6 , a salt containing the [ F e ( C N ) ] 6 4 – ion, given that its solubility product, 𝐾 s p , is 1 . 5 5 × 1 0 − 4 1 ? Assume that dissolution is the only process affecting the value of 𝐾 s p .

Q7:

The 𝐾 s p of N i C O 3 is 1 . 3 6 × 1 0 − 7 . What is the minimum volume of water needed to dissolve 0.100 g of N i C O 3 ?

Q8:

The 𝐾 s p of copper(I) bromide, C u B r , is 6 . 3 × 1 0 − 9 . What is the molar solubility of copper bromide?

Q9:

Two hypothetical salts, L M 2 and L Q 3 , have the same molar solubility in water. If 𝐾 s p of L M 2 is 3 . 2 0 × 1 0 − 5 , what is the 𝐾 s p of L Q 3 ?

Q10:

What is the molar solubility of cadmium sulfide ( C d S ) in a 0.010 M solution of cadmium bromide ( C d B r ) 2 ? The 𝐾 s p of C d S is 1 . 0 × 1 0 − 2 8 .

Q11:

What is the molar solubility of P b I 2 , given that its solubility product, 𝐾 s p , is 1 . 4 × 1 0 − 8 ? Assume that dissolution is the only process affecting the value of 𝐾 s p .

Q12:

What is the molar solubility of aluminum hydroxide, A l ( O H ) 3 , in a 0.015 M solution of aluminum nitrate, A l ( N O ) 3 3 ? The 𝐾 s p of A l ( O H ) 3 is 2 × 1 0 − 3 2 .

Q13:

The 𝐾 s p of silver(I) bromide ( A g B r ) is 5 . 0 × 1 0 − 1 3 . What is the molar solubility of A g B r in a 0.025 M aqueous solution of N a B r ?

Q14:

The 𝐾 s p of zinc(II) cyanide ( Z n ( C N ) ) 2 is 3 . 0 × 1 0 − 1 6 and the molar mass is 117.44 g/mol. How many grams of Z n ( C N ) 2 would be soluble in 125 mL of water?

Q15:

The 𝐾 s p of calcium hydroxide, C a ( O H ) 2 , is 1 . 3 × 1 0 − 6 . What is the molar solubility of calcium hydroxide?

Q16:

What is the molar solubility of M g F 2 if its solubility product, 𝐾 s p , is 6 . 4 × 1 0 − 9 ?

Q17:

The 𝐾 s p of lead(II) iodide, P b I 2 , is 1 . 4 × 1 0 − 8 . What is the molar solubility of lead(II) iodide?

Q18:

Most barium compounds are very poisonous; however, barium sulfate is often administered internally as an aid in the X-ray examination of the lower intestinal tract. This use of B a S O 4 is possible because of its low solubility. To 3 significant figures, what is the mass of barium present in 1.75 L of water saturated with B a S O 4 ? The 𝐾 s p for B a S O 4 is 2 . 3 0 × 1 0 − 8 .

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