HW07 - Solubility Equilibria

Question 12.0 pts

What is the net ionic equation for the reaction between aqueous solutions of Na3PO4 and CuSO4?
  1. No reaction occurs since no precipitate is formed.
  2. Cu2+ + PO43- \longrightarrow CuPO4
  3. 2Na+ + SO42- \longrightarrow Na2SO4
  4. 3Cu2+ + 2PO43- \longrightarrow Cu3(PO4)2

Question 22.0 pts

What ions are present in solution after aqueous solutions of Cu(NO3)2 and K2S are mixed? Assume we mixed stoichiometric equivalent amounts of both reactants and 100% reaction.
  1. No ions are present as both products form precipitates.
  2. Cu2+, S2-
  3. K+, NO3-
  4. Cu2+, NO3-, K+, S2-

Question 32.0 pts

Molar solubility is...
  1. the number of moles that dissolve to give one liter of saturated solution.
  2. the total molarity of the solution.
  3. equal to the Ksp.
  4. the number of moles that dissolve to give one liter of super-saturated solution.

Question 42.0 pts

The Ksp equation for sodium bicarbonate (NaHCO3) should be written as:
  1. Ksp = [Na+][H+][C4+][O2-]3
  2. Ksp = [Na+][HCO3-]
  3. Ksp = [Na+][H+][CO32-]
  4. Ksp = [NaH2+][CO32-]

Question 52.0 pts

Pure water is saturated with PbCl2. In this saturated solution, which of the following is true?
  1. Ksp = [Pb2+]2[Cl-]
  2. [Pb2+] = 0.5[Cl-]
  3. Ksp = [Pb2+][Cl-]
  4. [Pb2+] = [Cl-]

Question 62.0 pts

A hypothetical ionic substance T3U2 ionizes to form T2+ and U3- ions. The solubility of T3U2 is 4.04x10-20 mol/L. What is the value of the solubility-product constant?
  1. 1.63x10-39
  2. 1.16 x 10-95
  3. 9.79x10-39
  4. 1.08x10-97

Question 72.0 pts

The value of Ksp for SrSO4 is 2.8x10-7. What is the solubility of SrSO4 in moles per liter?
  1. 5.3 x 10-4
  2. 1.4 x 10-7
  3. 2.8 x 10-7
  4. 7.6 x 10-7

Question 82.0 pts

Determine the molar solubility of some salt with the generic formula AB2 if Ksp = 2.56x102.
  1. 10 M
  2. 4 M
  3. 0.1 M
  4. 1 M

Question 92.0 pts

Rank the following salts from least to most molar solubility:

BiI                             Ksp = 7.7x10-19

Cd3(AsO4)2               Ksp = 2.2x10-33

AlPO4                             Ksp = 9.8x10-21

CaSO4                       Ksp = 4.9x10-5

  1. Cd3(AsO4)2 < AlPO4 < BiI < CaSO4 
  2. CaSO4 < BiI < AlPO4 < Cd3(AsO4)2
  3. Cd3(AsO4)2 < BiI < AlPO4 < CaSO4 
  4. AlPO4 < BiI < Cd3(AsO4)2 < CaSO4

Question 103.0 pts

A hypothetical compound MX3 has a molar solubility of 0.00562 M. What is the value of Ksp for MX3?
  1. 3.16 x 10-5
  2. 2.69 x 10-8
  3. 2.99 x 10-9
  4. 9.48 x 10-5

Question 112.0 pts

Determine if a precipitate will form when 0.96g Na2CO3 is combined with 0.2g BaBr2 in a 10L solution. (For BaCO3, Ksp = 2.8x10-9).
  1. BaBr2 will remain in solid form as it is insoluble in water.
  2. BaCO3 does not precipitate
  3. It is impossible to know if any BaCO3 will precipitate with the information given.
  4. BaCO3 precipitates

Question 122.0 pts

CaSO4 has a Ksp = 3x10-5. In which of the following would CaSO4 be the most soluble?
  1. 0.5 M K2SO4(aq)
  2. 1.0 M CaCl2(aq)
  3. pure water
  4. CaSO4 would have the same solubility in all three of these solutions

Question 132.0 pts

A solution of AgI contains 1.9 M Ag+. Ksp of AgI is 8.3 x 10-17. What is the maximum I- concentration that can exist in this solution?
  1. 1.9 M
  2. 8.3x10-17 M
  3. 1.6x10-16 M
  4. 4.4x10-17 M

Question 143.0 pts

What would be the molar solubility of Li3PO4 (Ksp = 2.37 x 10-4) in a 1M LiCl solution?
  1. 5.44 x 10-2
  2. 1.24 x 10-1
  3. 2.37 x 10-4
  4. 1.54 x 10-2













CH302 · 50520 Principles of Chemistry II


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