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Homework answers / question archive / Chapter 17   Solubility and Simultaneous Equilibria   Multiple Choice   1)The expression for the solubility product of Ba3(AsO4)2 is                     a

Chapter 17   Solubility and Simultaneous Equilibria   Multiple Choice   1)The expression for the solubility product of Ba3(AsO4)2 is                     a

Chemistry

Chapter 17   Solubility and Simultaneous Equilibria

  Multiple Choice 

 1)The expression for the solubility product of Ba3(AsO4)2 is

 

                  a. [Ba2+]3[AsO43-]2

        1. [3 x Ba2+]3[2 x AsO43-]2
        2. 3[Ba2+] × 2[AsO43-]
        3. 3[Ba2+]3 + 2[AsO43-]2
        4. [Ba2+]3[AsO43-]2

 

 

  1. The expression for the solubility product of Ca3(PO4)2 is

 

                  a. [Ca2+]3 × [PO43-]2

        1. [3 x Ca2+]3 × [2 x PO43-]2
        2. 3[Ca2+] × 2[PO43-]
        3. 3[Ca2+]3 + 2[PO43-]2
        4. [Ca2+]3 × [PO43-]2

 

 

  1. The expression for the solubility product of Fe2(CrO4)3 is

 

        1. [Fe2+]3 × [CrO43-]2
        2. [2 x Fe2+]3 × [3 x CrO43-]2
        3. 3[Fe2+] × 2[CrO43-]
        4. 2[Fe2+]3 + 3[CrO43-]2   e. [Fe3+]2 × [CrO42-]3

 

 

  1. The expression for the solubility product of copper(II) hydroxide is

 

        1. [Cu2+][2 OH-]
        2. [Cu2+] × 2[OH-]2
        3. [Cu2+]2[OH-]   d. [Cu2+][OH-]2

                    e. [Cu2+] × ½[OH-]2

 

 

  1. The expression for the solubility product of calcium fluoride, CaF2 is

 

        1. [Ca2+][2 × F-]
        2. [Ca2+] × 2[F-]2
        3. [Ca2+]2[F-]   d. [Ca2+][F-]2

                     e. [Ca2+] × ½[F-]2

 

  1. The expression for the solubility product of silver oxalate (Ag2C2O4) is

 

        1. [Ag22+][C2O42-]
        2. [Ag+][C2O42-]2
        3. 2[Ag+][C2O42-]

                  d. [Ag+]2[C2O42-]

                     e. 2[Ag+]2[C2O42-

 

 

  1. The solubility of scandium(III) fluoride, ScF3, in pure water is 2.0 × 10-5 moles per liter.  Calculate the value of Ksp for scandium(III) fluoride from this data.  

 

        1. 1.3 × 10-17   
        2. 1.4 × 10-18     c. 4.3 × 10-18  
        1. 1.6 × 10-19   
        2. 4.8 × 10-19  

 

 

  1. The solubility of lead(II) fluoride, PbF2, in pure water is 2.1 × 10-3 moles per liter.  Calculate the value of Ksp for lead(II) fluoride from this data.  

 

        1. 1.3 × 10-7   
        2. 1.4 × 10-8     c. 3.7 × 10-8  
        1. 1.6 × 10-9   
        2. 4.8 × 10-9  

 

 

  1. The solubility of calcium fluoride, CaF2, in pure water is 2.15 × 10-4 moles per liter.  Calculate the value of Ksp for calcium fluoride from this data.  

 

        1. 1.85 × 10-7   
        2. 9.28 × 10-8  
        3. 1.99 × 10-11     d. 3.98 × 10-11       e. 9.94 × 10-12  

 

 

  1. The solubility of copper(II) arsenate, Cu3(AsO4)2, in pure water is 3.7 × 10-8 moles per liter.  Calculate the value of Ksp for copper(II) arsenate from this data.  

 

        1. 6.9 × 10-38   
        2. 4.2 × 10-37  
        3. 2.5 × 10-36  
        4. 3.7 × 10-36   

                  e. 7.5 × 10-36  

 

 

  1. The solubility of zinc(II) phosphate, Zn3(PO4)2, in pure water is 1.5 × 10-7 moles per liter.  Calculate the value of Ksp for zinc(II) phosphate from this data.  

 

        1. 2.3 × 10-14   
        2. 5.1 × 10-28  
        3. 2.7 × 10-33     d. 8.2 × 10-33       e. 7.6 × 10-35  

 

 

  1. The solubility of silver oxalate, Ag2C2O4, in pure water is 2.06 × 10-4 moles per liter.  Calculate the value of Ksp for silver oxalate from this data.  

 

        1. 4.24 × 10-8  
        2. 8.49 × 10-8  
        3. 1.75 × 10-11     d. 3.50 × 10-11       e. 8.74 × 10-12  

 

 

  1. The solubility of silver carbonate, Ag2CO3, in pure water is 1.27 × 10-4 moles per liter.  Calculate the value of Ksp for silver carbonate from this data.  

 

        1. 1.64 × 10-11  
        2. 3.28 × 10-11  
        3. 2.04 × 10-12  
        4. 4.10 × 10-12   

                  e. 8.19 × 10-12  

 

 

  1. Which one of the following salts has the highest solubility in water, expressed in moles per liter?  

 

        1. PbF2, Ksp = 3.6 × 10-8  
        2. Ag2CrO4, Ksp = 1.2 × 10-12
        3. CaF2, Ksp = 3.9 × 10-11

                  d. BaF2, Ksp = 1.7 × 10-6

                    e. PbI2, Ksp = 7.9 × 10-9  

 

 

  1. Which one of the compounds below has the highest solubility in water, expressed in moles per liter?  

 

        1. SrF2, Ksp = 2.8 × 10-9  
        2. Sr(IO3)2, Ksp = 3.3 × 10-7
        3. Fe(OH)2, Ksp = 8.0 × 10-16
        4. PbCl2, Ksp = 1.6 × 10-5                   e. PbBr2, Ksp = 3.9 × 10-5  
  1. Which one of the compounds below has the highest solubility in water, expressed in moles per liter?  

 

        1. SrF2, Ksp = 2.8 × 10-9  
        2. Sr(IO3)2, Ksp = 3.3 × 10-7
        3. MgF2, Ksp = 6.5 × 10-9                   d. PbCl2, Ksp = 1.6 × 10-5                                e. BaF2, Ksp = 1.7 × 10-6

 

 

  1. Which one of the compounds below has the lowest solubility in water, expressed in moles per liter?  

 

                  a. SrF2, Ksp = 2.8 × 10-9  

        1. Sr(IO3)2, Ksp = 3.3 × 10-7
        2. MgF2, Ksp = 6.5 × 10-9
        3. PbCl2, Ksp = 1.6 × 10-5
        4. PbI2, Ksp = 7.9 × 10-9

 

 

  1. The solubility of silver sulfate (Ag2SO4), in moles per liter, can be expressed in terms of the resulting ion concentrations.  Which relationship is correct?   

 

        1. solubility = 2[Ag+]  
        2. solubility = [Ag+
        3. solubility = [2Ag+]   
        4. solubility = 2[SO42-]  

                  e. solubility = [SO42-]  

 

 

  1. The solubility of strontium fluoride, SrF2, in moles per liter, can be expressed in terms of the resulting ion concentrations.  Which relationship is correct?   

 

                     a. solubility = 2[Sr2+]  

                  b. solubility = [Sr2+

        1. solubility = [2 Sr2+]   
        2. solubility = 2[F-]  
        3. solubility = [F-]  

 

 

  1. The solubility of copper(II) iodate, Cu(IO3)2, in moles per liter, can be expressed in terms of the resulting ion concentrations.  Which relationship is correct?   

 

                     a. solubility = 2[Cu2+]  

                  b. solubility = [Cu2+

        1. solubility = [2 Cu2+]   
        2. solubility = 2[IO3-]  
        3. solubility = [IO3-]2  

 

 

 

  1. The solubility of silver phosphate, Ag3PO4, in moles per liter, can be expressed in terms of the resulting ion concentrations.  Which relationship is correct?   

 

        1. solubility = 3[Ag+]  
        2. solubility = [Ag+
        3. solubility = [Ag+]3      d. solubility = [PO43-]  

                     e. solubility = [PO43-]3  

 

 

  1. The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18.  What is the solubility of Ag3PO4 in water, in moles per liter? 

 

                  a. 1.8 × 10-5

        1. 2.5 × 10-5 M    
        2. 1.9 × 10-86 M   
        3. 3.1 × 10-5
        4. 4.1 × 10-5 M    

 

 

  1. The solubility product for BaSO4 is 1.1 × 10-10.  Calculate the solubility of BaSO4 in pure water, in moles per liter.  

 

                     a. 5.5 × 10-11 mol L-1  

                  b. 1.0 × 10-5 mol L-1

        1. 2.1 × 10-5 mol L-1   
        2. 1.1 × 10-10 mol L-1  
        3. 2.2 × 10-10 mol L-1  

  

 

  1. The solubility product for PbCl2 is 1.7 × 10-5.  What is the solubility of PbCl2 in pure water, in moles per liter?  

 

        1. 2.4 × 10-4 mol L-1   
        2. 6.2 × 10-2 mol L-1   
        3. 7.7 × 10-3 mol L-1              d. 1.6 × 10-2 mol L-1                                        e. 6.0 × 10-5 mol L-1   

 

 

  1. Calculate the concentration of chloride ions in a saturated solution of lead(II) chloride.  The Ksp =

1.7 × 10-5.

 

        1. 2.4 × 10-4 M    
        2. 4.8 × 10-4
        3. 3.9 × 10-2
        4. 1.2 × 10-1 M                       e. 3.2 × 10-2
  1. Calculate the concentration of iodate ions in a saturated solution of lead(II) iodate, Pb(IO3)2.  The Ksp = 2.6 × 10-13.

 

        1. 3.2 × 10-5 M    
        2. 4.0 × 10-5
        3. 6.4 × 10-5

                        d. 8.0 × 10-5 M                                     e. 5.1 × 10-7

 

 

  1. Calculate the concentration of iodate ions in a saturated solution of barium iodate, Ba(IO3)2.  The Ksp = 1.5 × 10-9.

 

                        a. 1.4 × 10-3 M                                      b. 2.3 × 10-3

        1. 7.2 × 10-4
        2. 3.9 × 10-5 M    
        3. 7.7 × 10-5

 

 

  1. The solubility product of barium fluoride (BaF2) is 1.7 × 10-6.  Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

 

                    a. 7.6 × 10-3

                        b. 1.5 × 10-2 M                                     c. 3.4 × 10-5

        1. 1.7 × 10-6
        2. 3.4 × 10-6 M    

 

 

  1. The solubility product for Mg3(PO4)2 is 6.3 × 10-26.  What is the solubility of Mg3(PO4)2 in pure water, in grams per liter?    

  

        1. 1.7 × 10-23 g L-1   
        2. 3.4 × 10-7 g L-1               c. 9.4 × 10-4 g L-1                                  d. 1.2 × 10-3 g L-1 

                     e. 2.4 × 10-3 g L-1 

 

 

  1. The solubility of lead iodide is 578 mg L-1 at 25 °C.  What is the solubility product for PbI2?  

 

  a. 7.9 × 10-9    b. 1.6 × 10-6

        1. 1.1 × 10-11
        2. 2.7 × 10-12
        3. 6.3 × 10-6

 

  1. The solubility of barium carbonate is 14.8 mg L-1 at 30 °C.  Calculate the Ksp value for BaCO3. 

 

        1. 7.5 × 10-5
        2. 1.5 × 10-4   c. 5.6 × 10-9
        1. 7.5 × 10-6   
        2. 1.5 × 10-3   

 

 

  1. What is the solubility, in moles per liter, of Fe(OH)2 (Ksp = 7.9 × 10-16) in 0.0500 molar NaOH solution? 

                        a. 3.16 × 10-13                                      b. 3.13 × 10-16

        1. 1.58 × 10-14
        2. 1.14 × 10-14
        3. 3.16 × 10-16

 

 

  1. What is the solubility, in moles per liter, of PbSO4 (Ksp = 6.3 × 10-7) in 0.0230 molar MgSO4 solution? 
        1. 2.14 × 10-5
        2. 7.24 × 10-5            c. 2.74 × 10-5                                   d. 4.72 × 10-5

                    e. 4.27 × 10-5

 

 

  1. What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10) in 0.0300 M CaCl2 solution?                                      a. 9.0 × 10-3
        1. 9.0 × 10-6
        2. 6.0 × 10-9            d. 3.0 × 10-9                             e. 6.0 × 10-3

 

 

  1. What is the solubility, in moles per liter, of BaSO4 (Ksp = 1.1 × 10-10) in 0.0100 M Na2SO4 solution? 

                  a. 1.1 × 10-8

        1. 1.1 × 10-6
        2. 1.1 × 10-7
        3. 1.1 × 10-5
        4. 1.1 × 10-4

 

 

  1. What is the solubility, in moles per liter, of MgCO3 (Ksp = 3.5 × 10-8) in 0.0200 M Na2CO3 solution?                                      a. 4.4 × 10-6
        1. 8.1 × 10-4
        2. 4.4 × 10-3
        3. 8.8 × 10-5

                  e. 1.8 × 10-6

 

 

  1. What is the solubility, in moles per liter, of Ag2CO3 (Ksp = 8.1 × 10-12) in 0.0300 M Na2CO3 solution? 

                        a. 2.7 × 10-10                             b. 9.0 × 10-9

        1. 3.0 × 10-7
        2. 4.0 × 10-10
        3. 2.7 × 10-9

 

 

  1. What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10)  in 0.0100 molar aqueous potassium chloride solution?

 

                                    a. 7.5 × 10-5 mol L-1                       b. 1.8 × 10-8 mol L-1                             c. 1.3 × 10-6 mol L-1

        1. 3.6 × 10-8 mol L-1    
        2. 1.5 × 10-7 mol L-1 

 

 

  1. The solubility of barium sulfate varies with the composition of the solvent in which it was dissolved.  In which solvent mixture would BaSO4 have the lowest solubility?

  

        1. pure water
        2. 0.10 M Na2SO4(aq)

  c. 1.0 M (NH4)2SO4(aq)       d. 0.5 M Ba(NO3)2(aq)

                    e. 1.0 M HCl(aq)

 

 

  1. Which solid would be more soluble in a strong acid solution than in pure water? 

 

        1. KCl 
        2. MgCl2   
        3. NaNO3   
        4. LiBr 

                  e. ZnCO3   

 

  1. Which solid would be more soluble in a strong acid solution than in pure water? 

 

        1. NaCl 
        2. MgBr2   
        3. LiNO3      d. CaCO3     e. AgBr 

 

 

  1. What is the maximum concentration of Mg2+ ion that can exist in a 0.10 M NaF(aq) solution without causing any precipitate of magnesium fluoride to form?  The Ksp of MgF2 is 6.6 × 10-9.

 

        1. 1.3 × 10-7 M  
        2. 6.6 × 10-9
        3. 6.6 × 10-8
        4. 1.6 × 10-7

                  e. 6.6 × 10-7 M    

 

 

  1. Calculate the minimum concentration of Ag+ ion that must be added to (or built up in) a 0.140 M Na2CrO4 solution in order to initiate a precipitation of silver chromate.  The Ksp of Ag2CrO4 is 1.2 × 10-12

 

                                    a. 4.8 × 10-9 mol L-1                    b. 2.9 × 10-6 mol L-1

        1. 2.0 × 10-6 mol L-1    
        2. 9.5 × 10-7 mol L-1 
        3. 1.4 × 10-6 mol L-1

 

 

  1. The solubility product for Ag3PO4 is 2.8 × 10-18.  What is the solubility of silver phosphate in solution which also contains 0.10 moles of silver nitrate per liter?

 

        1. 4.4 × 10-4 mol L-1
        2. 4.4 × 10-15 mol L-1   

                  c. 2.8 × 10-15 mol L-1

        1. 3.6 × 10-16 mol L-1   
        2. 2.8 × 10-13 mol L-1   

 

 

  1. Will a precipitate form when 20.0 mL of 1.8 × 10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 × 10-4 M Na2SO4?  The Ksp of (PbSO4) is 6.3 × 10-7.

 

                        a. no, because the ion product < Ksp                                         b. no, because the ion product > Ksp

        1. yes, because the ion product < Ksp  
        2. yes, because the ion product > Ksp  
        3. no, because Ksp is less than the ion product   
  1. Will a precipitate of MgF2 form when 300 mL of 1.1 × 10-3 M MgCl2 solution is added to 500 mL of 1.2 × 10-3 M NaF?  The Ksp of MgF2 is 6.9 × 10-9.  

 

                                    a. yes, because the ion product, Q  > Ksp                   b. no, because the ion product, Q  < Ksp                                  c. no, because the ion product, Q  = Ksp

        1. yes, because the ion product, Q  < Ksp  
        2. no, because the ion product, Q  > Ksp  

 

 

  1. In an experiment, it is planned to add 300 mL of 2.0 × 10-5 M AgNO3 to 200 mL of 2.5 × 10-9 M NaI.  Will a precipitate form?  What is the precipitate?  Ksp (AgI) = 8.3 × 10-17.

 

        1. yes, the ppt is AgNO3(s) 
        2. yes, the ppt is NaNO3(s) 
        3. yes, the ppt is NaI(s)                     d. yes, the ppt is AgI(s)

                    e. no   

 

 

  1. For PbCl2, Ksp = 1.7 × 10-5.  Will a precipitate of PbCl2 form when 200 mL of 3.0 × 10-2 M Pb(NO3)2 solution is added to 300 mL of 5.0 × 10-2 M KCl?  Choose one of the following.    

 

                    a. yes, the ion product, Q > Ksp   

                  b. no, the ion product, Q < Ksp 

        1. no, the ion product, Q = Ksp    
        2. yes, the ion product, Q < Ksp   
        3. no, because the ion product, Q > Ksp

 

 

  1. Zinc carbonate, a slightly soluble substance, is most soluble in which of the following solvents?

 

        1. water   
        2. 0.1 M ZnCl2(aq)
        3. 0.1 M NaOH(aq

                  d. 0.1 M HCl(aq)  

                     e. 0.2 M Na2CO3(aq)  

 

 

  1. The pH of a saturated solution of cerium(III) hydroxide in water is 9.20.  Calculate a value for the solubility product constant of cerium(III) hydroxide from this data.

 

        1. 2.5 × 10-10 
        2. 8.4 × 10-11
        3. 4.0 × 10-19   d. 2.1 × 10-20    e. 6.3 × 10-20

 

  1. The value of the solubility product constant for barium carbonate is 5.0 × 10-9 and that of barium chromate is 2.1 × 10-10.  From this data, what is the value of Kc for the reaction, 

BaCO3(s)  +  CrO42-(aq)  BaCrO4(s)  +  CO32-(aq)

 

        1. 1.1 × 10-18 
        2. 4.2 × 10-2
        3. 4.8 × 10-9  
        4. 4.9

                  e. 24

 

 

  1. Hydrazine, N2H4, is a weak molecular base with a value of 9.6 × 10-7 for Kb.  An aqueous solution contains 0.200 M N2H4 and 0.376 M N2H5Cl per liter as the only solutes.  If the Ksp of Fe(OH)2 is 7.9 × 10-16, what is the maximum [Fe2+] that can coexist with these solutes in the solution?  

 

        1. 1.5 × 10-9 M
        2. 4.1 × 10-9 M
        3. 0.00024 M
        4. 0.00086 M

                  e. 0.0030 M

 

 

  1. Methylamine, CH3NH2, is a weak molecular base with a value of 4.4 × 10-4 for Kb.  An aqueous solution contains 0.200 M CH3NH2 and 0.400 M CH3NH3Cl per liter as the only solutes.  If the Ksp of Mg(OH)2 is 7.1 × 10-12, what is the maximum [Mg2+] that can coexist with these solutes in the solution?    

 

        1. 8.1 × 10-9  
        2. 3.2 × 10-8
        3. 9.2 × 10-6   d. 1.5 × 10-4      e. 3.7 × 10-1  

 

 

  1. Methylamine, CH3NH2, is a weak molecular base with a value of 4.4 × 10-4 for Kb.  An aqueous solution contains 0.200 M CH3NH2 and 0.300 M CH3NH3Cl per liter as the only solutes.  If the Ksp of Fe(OH)2 is 7.9 × 10-16, what is the maximum [Fe2+] that can coexist with these solutes in the solution?    

 

        1. 1.8 × 10-12  
        2. 9.0 × 10-12
        3. 1.8 × 10-9   d. 9.2 × 10-9      e. 9.2 × 10-6  

 

  1. Dimethylamine, (CH3)2NH, is a weak molecular base with a value of 9.6 × 10-4.for Kb.  An aqueous solution contains 0.350 M (CH3)2NH and 0.250 M (CH3)2NH2Cl per liter as the only solutes. If the Ksp of Mg(OH)2 is 7.1 × 10-12, what is the maximum [Mg2+] that can coexist with these solutes in the solution?    

 

                    a. 1.7 × 10-7  

  b. 3.9 × 10-6    c. 7.7 × 10-6

        1. 1.5 × 10-5  
        2. 4.9 × 10-3  

 

 

  1. The Ksp of calcium fluoride is 3.9 × 10-11.  A 0.420 g sample of NaF and a 1.110 g sample of calcium chloride were added to a 1.000 liter volumetric flask, and distilled water was added to the mark.  After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, what would be the calcium ion concentration remaining in solution afterwards?  Be mindful that a precipitate may be formed.

 

                                    a. 0.0036 mole per liter                  b. 0.0050 mole per liter                                      c. 0.0054 mole per liter

        1. 0.0058 mole per liter
        2. 0.0100 mole per liter

 

 

  1. The Ksp of calcium fluoride is 3.9 × 10-11.  A 0.420 g sample of NaF and a 1.110 g sample of calcium chloride were added to a 1.000 liter volumetric flask, and distilled water was added to the mark.  After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, how many grams of precipitate, if any, would be formed? 

 

        1. 0.00 g
        2. 0.039 g    c. 0.39 g     d. 0.41 g

                    e. 0.77 g

 

 

  1. The Ksp value for barium chromate is  2.1 × 10-10.  A 4.16 g sample of BaCl2 and a 5.83 g sample of potassium chromate were added to a 1.000 liter volumetric flask, and distilled water was added to the mark.  After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, what would be the barium ion concentration remaining in solution afterwards?  Be mindful that a precipitate may be formed.

 

                                    a. 2.5 × 10-8 mole per liter                  b. 2.1 × 10-8 mole per liter                                c. 2.5 × 10-7 mole per liter

        1. 1.5 × 10-6 mole per liter
        2. 1.5 × 10-5 mole per liter

 

 

 

  1. The Ksp value for barium chromate is 2.1 × 10-10.  A 4.16 g sample of BaCl2 and a 5.83 g sample of potassium chromate were added to a 1.000 liter volumetric flask, and distilled water was added to the mark.  After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, how many grams of precipitate, if any, would be formed? 

 

        1. 0.00 g
        2. 0.0454 g
        3. 4.54 g   d. 5.06 g    e. 5.31 g

 

 

  1. Given the following information: 

Ni(OH)2(s)Ni2+(aq)  +  2 OH-(aq)   Ksp = 6.0 x 10-16

                                                   H2O(l)H+(aq)  +  OH-(aq)       Kw  = 1.0 x 10-14

        What is the equilibrium constant for the reaction,  

                        Ni(OH)2(s)  +  2 H+(aq)Ni2+(aq)  +  2 H2O(l)

 

        1. Ksp/Kw
        2. 10 x Ksp/Kw

  c. Ksp/Kw2    d. Kw2/Ksp

                     e. 2 x Kw/Ksp 

 

 

  1. PbCO3, PbCl2, PbI2, and PbS are all only very slightly soluble in pure water.  Which one (ones) should be significantly more soluble in acidic solution than in pure water?   

 

        1. PbI2, PbS and PbCO3 
        2. only PbCO3 and PbS
        3. only PbCl2 and PbI2

                  d. only PbCO3

                     e. All four are significantly more soluble in acidic solution.

 

 

  1. The group Zn(NO3)2, Zn(CO3)2, ZnCl2, and ZnS contains some salts which are only very slightly soluble in pure water.  Of those salts, which one(s) should be significantly more soluble in acidic solution than in pure water?

 

        1. Zn(NO3)2, Zn(CO3)2, and ZnCl2   
        2. Zn(NO3)2, and Zn(CO3)2 
        3. ZnCl2, and ZnS
        4. Zn(CO3)2, and ZnCl2    

                  e. Zn(CO3)2, and ZnS   

 

 

 

  1. A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M) and K+ (1.0 × 10-3 M).  Drops of a 5.0

× 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 1.5 × 10-3 M.  Should a precipitate form?  If so, what is the precipitate?  The Kspvalues are—BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9.  (Neglect the slight change in volume resulting from the added NaF solution.) 

 

        1. a precipitate consisting of BaF2 only should form
        2. a precipitate consisting of CaF2 and KF should form
        3. a precipitate consisting of BaF2 and CaF2 should form
        4. a precipitate consisting of CaF2 only should form

                  e. no precipitate should form

 

 

  1. A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M) and K+ (1.0 × 10-3 M).  Drops of a 5.0

× 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 3.0 × 10-3 M.  Should a precipitate form?  If so, what is the precipitate?  The Kspvalues are—BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9.  (Neglect the slight change in volume resulting from the added NaF solution.)  

 

        1. a precipitate consisting of BaF2 only should form
        2. a precipitate consisting of CaF2 and KF should form
        3. a precipitate consisting of BaF2 and CaF2 should form                d. a precipitate consisting of CaF2 only should form                                      e. no precipitate should form

 

 

  1. A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M) and K+ (1.0 × 10-3 M).  Drops of a 5.0

× 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 6.0 × 10-3 M.  Should a precipitate form?  If so, what is the precipitate?  The Kspvalues are—BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9.  (Neglect the slight change in volume resulting from the added NaF solution.)  

 

        1. a precipitate consisting of BaF2 only should form
        2. a precipitate consisting of CaF2 and KF should form
        3. a precipitate consisting of BaF2 and CaF2 should form                d. a precipitate consisting of CaF2 only should form                                      e. no precipitate should form

 

 

  1. Silver bromide, AgBr, is more soluble in ammonia solution than in pure water.  The reaction is, 

AgBr(s)  +  2 NH3(aq)  Ag(NH3)2+  +  Br-(aq)

        Using Ksp (AgBr) = 5.0 x 10-13 and Kform (Ag(NH3)2+) = 1.60 x 107, calculate the solubility of AgBr in 0.800 M ammonia solution..

 

                     a. 1.6 x 10-3 mole per liter  

                  b. 2.3 x 10-3 mole per liter

                         

        1. 2.8 x 10-3 mole per liter 
        2. 4.2 x 10-3 mole per liter    
        3. 6.1 x 10-2

 

 

Fill in the Blanks

 

 

  1. A precipitate will form when a solution containing a cation and a solution containing an anion are mixed if the _____________ exceeds the value of the ________________________ 

 

 

  1. Addition of a common ion to a solution of a slightly soluble salt will __________ the solubility of the slightly soluble salt.

 

 

  1. The pH of a saturated solution of Mg(OH)2, whose Ksp is 7.1 × 10-12, is ______ 

 

 

  1. The pH of a saturated solution of Ca(OH)2 is 12.37.  What is the Ksp of Ca(OH)2?  ______

 

 

  1. For the H2CO3?HCO3-?CO32- system at room temperature Ka1 = 4.5 × 10-7, while Ka2 = 4.7 ×  10-

          11                                                                    -9

. The Ksp for BaCO3 is 5.0 ×  10 . Calculate the equilibrium constant for the reaction, 

 

 

  1. The formation constant for the diammine silver(I) ion is 1.6 × 107, while the solubility product constant for silver chloride is 1.8 × 10-10.  What is the equilibrium constant for the reaction, 

                   AgCl(s)  +  2 NH3(aq)  Ag(NH3)2+(aq)  +  Cl-(aq)?  ______ 

 

 

  1. The formation constant for the bis(thiosulfato)argentate(I) ion is 2.0 × 1013, while the solubility product constant for silver bromide is 5.0 × 10-13.  What is the equilibrium constant for the reaction,

AgBr(s)  +  2 S2O32-(aq)  Ag(S2O3)23-(aq)  +  Br-(aq)? ______

 

 

  1. The formation constant for the diammine silver(I) ion is 1.6 × 107, while the solubility product constant for silver chloride is 1.8 × 10-10.  Given the reaction,

AgCl(s)  +  2 NH3(aq)  Ag(NH3)2+(aq)  +  Cl-(aq)

        What is the solubility, in moles per liter, of silver chloride in 1.00 molar ammonia solution? _______ 

 

 

  1. The formation constant for the bis(thiosulfato)argentate(I) ion is 2.0 × 1013, while the solubility product constant for silver bromide is 5.0 × 10-13.  Considering the reaction, 

AgBr(s)  +  2 S2O32-(aq)  Ag(S2O3)23-(aq)  +  Br-(aq)

        What is the solubility, in moles per liter, of silver bromide in 0.200 molar sodium thiosulfate solution? ______

 

 

  1. The formation constant for the bis(thiosulfato)argentate(I) ion, [Ag(S2O3)2]3-, is 2.0 × 1013, while the solubility product constant for silver iodide is 8.3 × 10-17.  A 0.200 molar solution of Na2S2O3 is saturated with AgI.  What is the concentration of free iodide ion in the saturated solution? _______

 

 

  1. The formation constant for the tris(ethylenediammine)nickel(II) complex ion, [Ni(en)3]2+, is 4.1 × 1017.  What is the concentration of the free nickel(II) ion in a solution in which the equilibrium concentration of free ethylenediamine is 0.400 molar, and that of the nickel complex above is 0.0100 molar? ____________ 

 

 

True and False

 

 

  1. The oxide ion can exist in aqueous solutions provided the pH is higher than 11.00.  ___ 

 

  1. The sulfide ion is too basic to exist as such in aqueous solutions.  ___

 

  1. Even though silver chloride is only very slightly soluble in water, addition of a reagent which forms complexes with silver ion increases this solubility.  ___

 

 

Critical Thinking Questions

 

 

  1. NaOH is added to sea water containing 0.050 moles per liter of Mg2+ ion until the pH reaches 12.0.  A certain quantity of Mg(OH)2 precipitates.  How many parts per billion of magnesium are left behind in the solution?  The Ksp of Mg(OH)2 is 7.1 × 10-12.

 

    1. 1.2 ppb
    2. 12 ppb
    3. 0.17 ppb

                  d. 1.7 ppb

                    e. 173 ppb

 

 

  1. Consider the equilibrium, 

AgCl(s)  +  Br-(aq)  AgBr(s)  +  Cl-(aq)

       whose equilibrium constant is related to Ksp(AgCl) = 1.8  ×  10-10 and Ksp(AgBr) = 5.0 × 10-13

Calculate the equilibrium constant for the reaction, and tell whether AgCl will react with 1.00 molar

KBr(aq) to a significant extent.  ______, ______

  

 

  1. The value Ka2 for the H2CO3?HCO3-?CO32- system at room temperature is 5.6 × 10-11, while the

Ksp for BaCO3 is 5.0 × 10-9.  Based on the reaction, BaCO3(s)  +  H+(aq)  Ba2+(aq)  +  HCO3(aq), calculate the solubility of  BaCO3(s) in a non-interacting buffer whose pH is 9.00.              __________ 

 

 

Short Answers

 

  1. What is the molar solubility of Ca(OH)2 in a 0.300 M NaOH solution? The Ksp of Ca(OH)2 is 6.5 x

10-6.

 

 

  1. What is the molar solubility of AgCl in a 0.450 M solution of KCl? The Ksp of AgCl is 1.8 x 10-10

 

 

  1. A student mixes 100.00 mL of 0.250 M MgSO4 with 250.00 mL 0.100 M NaOH. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text. 

 

 

  1. A student mixes 50.00 mL of 0.500 M NaCl with 75.00 mL of 0.200 M AgNO3. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text. 

 

 

  1. How many grams of AgCl can dissolve in 1.0 L of 1.5 M NH3? The Ksp of AgCl is 1.8 × 10-10, and the formation constant of [Ag(NH3)2]+ is 1.6 × 107.  

 

 

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