Worksheet: Molar Solubilities from Solubility Products

In this worksheet, we will practice calculating the molar solubility of an ionic solid from its molecular formula and solubility product.

Q1:

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

Calcium Salt C a ( O H ) 2 C a C O 3 C a S O · 2 H O 4 2 C a C O · H O 2 4 2 C a ( P O ) 3 4 2
𝐾 s p 1 . 3 × 1 0 8 . 7 × 1 0 6 . 1 × 1 0 1 . 9 6 × 1 0 1 . 3 × 1 0
  • A C a ( O H ) 2
  • B C a ( P O ) 3 4 2
  • C C a S O · 2 H O 4 2
  • D C a C O · H O 2 4 2
  • E C a C O 3

Q2:

Solutions of HgI22 contain Hg22+ and I ions. What is the molar solubility of HgI22, given that its solubility product, 𝐾sp, is 4.5×10? Assume that dissolution is the only process affecting the value of 𝐾sp.

  • A 2 . 2 × 1 0 M
  • B 3 . 6 × 1 0 M
  • C 4 . 1 × 1 0 M
  • D 1 . 4 × 1 0 M
  • E 3 . 7 × 1 0 M

Q3:

What is the molar solubility of Ag[Fe(CN)]46, a salt containing the [Fe(CN)]64 ion, given that its solubility product, 𝐾sp, is 1.55×10? Assume that dissolution is the only process affecting the value of 𝐾sp.

  • A 6 . 8 9 × 1 0 M
  • B 1 . 5 7 × 1 0 M
  • C 2 . 2 7 × 1 0 M
  • D 9 . 3 8 × 1 0 M
  • E 3 . 2 1 × 1 0 M

Q4:

What is the molar solubility of PbI2, given that its solubility product, 𝐾sp, is 1.4×10? Assume that dissolution is the only process affecting the value of 𝐾sp.

  • A 1 . 2 × 1 0 M
  • B 8 . 0 × 1 0 M
  • C 2 . 4 × 1 0 M
  • D 1 . 5 × 1 0 M
  • E 7 . 0 × 1 0 M

Q5:

What is the molar solubility of aluminum hydroxide, Al(OH)3, in a 0.015 M solution of aluminum nitrate, Al(NO)33? The 𝐾sp of Al(OH)3 is 2×10.

  • A 2 × 1 0 M
  • B 8 × 1 0 M
  • C 4 × 1 0 M
  • D 2 × 1 0 M
  • E 1 × 1 0 M

Q6:

What is the molar solubility of cadmium sulfide (CdS) in a 0.010 M solution of cadmium bromide (CdBr)2? The 𝐾sp of CdS is 1.0×10.

  • A 1 . 0 × 1 0 M
  • B 1 . 0 × 1 0 M
  • C 1 . 0 × 1 0 M
  • D 1 . 0 × 1 0 M
  • E 1 . 0 × 1 0 M

Q7:

What is the molar solubility of MgF2 if its solubility product, 𝐾sp, is 6.4×10?

  • A 8 . 0 × 1 0 M
  • B 2 . 3 × 1 0 M
  • C 1 . 9 × 1 0 M
  • D 1 . 2 × 1 0 M
  • E 1 . 5 × 1 0 M

Q8:

Calomel, HgCl22, is a compound composed of the diatomic ion of mercury(I), Hg22+, and chloride ions, Cl. 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. HgCl()Hg()+2Cl()2222+spsaqaq,𝐾=1.1×10 What is the molar solubility of HgCl22?

  • A 6 . 5 × 1 0 M
  • B 1 . 3 × 1 0 M
  • C 1 . 6 × 1 0 M
  • D 1 . 0 × 1 0 M
  • E 8 . 2 × 1 0 M

Q9:

The 𝐾sp of lead(II) iodide, PbI2, is 1.4×10. What is the molar solubility of lead(II) iodide?

  • A 2 . 4 × 1 0 M
  • B 1 . 2 × 1 0 M
  • C 2 . 0 × 1 0 M
  • D 1 . 5 × 1 0 M
  • E 1 . 9 × 1 0 M

Q10:

The 𝐾sp of copper(I) bromide, CuBr, is 6.3×10. What is the molar solubility of copper bromide?

  • A 1 . 8 × 1 0 M
  • B 4 . 0 × 1 0 M
  • C 7 . 9 × 1 0 M
  • D 3 . 2 × 1 0 M
  • E 6 . 3 × 1 0 M

Q11:

The 𝐾sp of silver iodide, AgI, is 1.5×10. What is the molar solubility of silver iodide?

  • A 1 . 5 × 1 0 M
  • B 1 . 2 × 1 0 M
  • C 3 . 4 × 1 0 M
  • D 5 . 3 × 1 0 M
  • E 2 . 3 × 1 0 M

Q12:

The 𝐾sp of calcium hydroxide, Ca(OH)2, is 1.3×10. What is the molar solubility of calcium hydroxide?

  • A 1 . 3 × 1 0 M
  • B 6 . 9 × 1 0 M
  • C 8 . 7 × 1 0 M
  • D 1 . 1 × 1 0 M
  • E 1 . 1 × 1 0 M

Q13:

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 BaSO4 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 BaSO4? The 𝐾sp for BaSO4 is 2.30×10.

  • A 6 . 1 9 × 1 0 g
  • B 5 . 9 1 × 1 0 g
  • C 4 . 1 1 × 1 0 g
  • D 2 . 0 8 × 1 0 g
  • E 3 . 6 4 × 1 0 g

Q14:

The 𝐾sp of NiCO3 is 1.36×10. What is the minimum volume of water needed to dissolve 0.100 g of NiCO3?

Q15:

The 𝐾sp of silver(I) bromide (AgBr) is 5.0×10. What is the molar solubility of AgBr in a 0.025 M aqueous solution of NaBr?

  • A 6 . 1 × 1 0 M
  • B 7 . 0 × 1 0 M
  • C 1 . 7 × 1 0 M
  • D 5 . 0 × 1 0 M
  • E 2 . 0 × 1 0 M

Q16:

The 𝐾sp of milk of magnesia (Mg(OH))2 is 7.1×10. How many grams of milk of magnesia would be soluble in 200 mL of water at 25C?

  • A 1 . 4 × 1 0 g
  • B 9 . 1 × 1 0 g
  • C 4 . 1 × 1 0 g
  • D 6 . 0 × 1 0 g
  • E 3 . 8 × 1 0 g

Q17:

The 𝐾sp of zinc(II) cyanide (Zn(CN))2 is 3.0×10 and the molar mass is 117.44 g/mol. How many grams of Zn(CN)2 would be soluble in 125 mL of water?

  • A 5 . 0 × 1 0 g
  • B 6 . 2 × 1 0 g
  • C 4 . 4 × 1 0 g
  • D 5 . 3 × 1 0 g
  • E 7 . 0 × 1 0 g

Q18:

Two hypothetical salts, LM2 and LQ3, have the same molar solubility in water. If 𝐾sp of LM2 is 3.20×10, what is the 𝐾sp of LQ3?

  • A 1 . 0 2 × 1 0 M
  • B 5 . 6 1 × 1 0 M
  • C 4 . 3 2 × 1 0 M
  • D 1 . 0 9 × 1 0 M
  • E 8 . 3 9 × 1 0 M

Q19:

What is the molar solubility of BaSO4 in a 0.250 M solution of NaHSO4? Take 𝐾=2.3×10sp4(BaSO) and 𝐾=1.2×10a4(HSO).

  • A 8 . 7 × 1 0 M
  • B 4 . 7 × 1 0 M
  • C 1 . 5 × 1 0 M
  • D 2 . 3 × 1 0 M
  • E 9 . 2 × 1 0 M

Q20:

What is the molar solubility of Tl(OH)3 in a 0.15 M solution of NH3? Take 𝐾=6.3×10sp3(Tl(OH)) and 𝐾=1.8×10b3(NH).

  • A 7 . 6 × 1 0 M
  • B 2 . 5 × 1 0 M
  • C 1 . 4 × 1 0 M
  • D 2 . 1 × 1 0 M
  • E 6 . 9 × 1 0 M

Q21:

The acid dissociation constant, 𝐾a, of HF is 7.2×10 and the solubility product, 𝐾sp, of CaF2 is 4.0×10. Calculate, to 2 significant figures, the molar solubility of CaF2 in a 0.125 M solution of HF.

  • A 4 . 2 × 1 0 M
  • B 5 . 4 × 1 0 M
  • C 4 . 8 × 1 0 M
  • D 4 . 4 × 1 0 M
  • E 3 . 6 × 1 0 M

Q22:

The solubility product, 𝐾sp, of Pb(OH)2 is 1.2×10 and the base dissociation constant, 𝐾b, of CHNH32 is 4.4×10. Calculate, to 2 significant figures, the molar solubility of Pb(OH)2 in a 0.138 M solution of CHNH32.

  • A 9 . 8 × 1 0 M
  • B 1 . 7 × 1 0 M
  • C 2 . 1 × 1 0 M
  • D 1 . 6 × 1 0 M
  • E 3 . 5 × 1 0 M

Q23:

The acid dissociation constant, 𝐾a, of HF is 6.8×10 and the solubility product, 𝐾sp, of BaF2 is 2.4×10. Calculate, to 2 significant figures, the molar solubility of BaF2 in a buffer solution containing 0.15MHF and 0.25MNaF.

  • A 3 . 8 × 1 0 M
  • B 9 . 6 × 1 0 M
  • C 5 . 6 × 1 0 M
  • D 1 . 4 × 1 0 M
  • E 7 . 7 × 1 0 M

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