Question 1

How many moles of CaF2 will dissolve in 3.0 L of 0.041 M NaF solution? (Ksp for CaF2 = 4.0 × 10-11)

Accepted Answer

A)  3.3 × 10-10
B)  2.4 × 10-8
C)  7.1 × 10-8
D)  7.9 × 10-9
E)  none of these

Question 2

Suppose 50.00 mL of 2.0 × 10-6 M Fe(NO3) 3 is added to 50.00 mL of 2.0 ×10-4 M KIO3.Which of the following statements is true? For Fe(IO3) 3,Ksp = 1.0 × 10-14.

Accepted Answer

A)  A precipitate forms because Qc > Ksp.
B)  A precipitate forms because Qc sp.
C)  No precipitate forms because Qc sp.
D)  No precipitate forms because Qc = Ksp.
E)  No precipitate forms because Qc > Ksp.

Question 3

An aqueous solution of Ag(CN) 2− is made by combining 0.0100 moles AgNO3 with 1.00 mole NaCN and diluting to 1.000 L.What is the molar concentration of Ag+ in the solution?
Ag+(aq) + 2CN-(aq)  2− is made by combining 0.0100 moles AgNO3 with 1.00 mole NaCN and diluting to 1.000 L.What is the molar concentration of Ag+ in the solution? Ag+(aq) + 2CN-(aq)   Ag(CN) 2-(aq) ; Kf = 5.6 × 1018 A) 1.9 × 10-21 M B) 5.3 × 1020 M C) 5.8 × 1016 M D) 1.7 × 10-17 M E) 0.010 M" class="answers-bank-image d-inline" rel="preload" >Ag(CN) 2-(aq) ; Kf = 5.6 × 1018

Accepted Answer

A)  1.9 × 10-21 M
B)  5.3 × 1020 M
C)  5.8 × 1016 M
D)  1.7 × 10-17 M
E)  0.010 M

Question 4

What is the solubility product expression for La2(CO3) 3?

Accepted Answer

A)  Ksp = [2La3+]2[3CO32-]3
B)  Ksp = [La2+]2[CO32-]3
C)  Ksp = [2La3+]2[CO32-]3
D)  Ksp = [2La3+][3CO32-]
E)  Ksp = [La3+]2[CO32-]3

Question 5

What is the maximum Sr2+ concentration possible in a solution that has a 2+ concentration possible in a solution that has a   M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7. A)    M B)    M C)    M D)    M E)    M" class="answers-bank-image d-inline" rel="preload" > M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7.

Accepted Answer

A)   2+ concentration possible in a solution that has a   M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7. 
A)     M 
B)     M 
C)     M 
D)     M 
E)     M" class="answers-bank-image d-inline" rel="preload" > M
B)   2+ concentration possible in a solution that has a   M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7. 
A)     M 
B)     M 
C)     M 
D)     M 
E)     M" class="answers-bank-image d-inline" rel="preload" > M
C)   2+ concentration possible in a solution that has a   M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7. 
A)     M 
B)     M 
C)     M 
D)     M 
E)     M" class="answers-bank-image d-inline" rel="preload" > M
D)   2+ concentration possible in a solution that has a   M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7. 
A)     M 
B)     M 
C)     M 
D)     M 
E)     M" class="answers-bank-image d-inline" rel="preload" > M
E)   2+ concentration possible in a solution that has a   M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7. 
A)     M 
B)     M 
C)     M 
D)     M 
E)     M" class="answers-bank-image d-inline" rel="preload" > M

Question 6

The best explanation for the dissolution of ZnS in dilute HCl is that

Accepted Answer

A)  the zinc ion is amphoteric.
B)  the sulfide ion concentration is decreased by the formation of H2S.
C)  the solubility product of ZnCl2 is less than that of ZnS.
D)  the zinc ion concentration is decreased by the formation of a chloro complex.
E)  the sulfide ion concentration is decreased by oxidation to sulfur.

Question 7

In which of the following solutions would CaC2O4 have the highest molar solubility?

Accepted Answer

A)  0.01 M Na2C2O4
B)  0.01 M NaCl
C)  0.01 M HCl
D)  0.01 M Ca(NO3) 2
E)  0.01 M NaHC2O4

Question 8

Given the following equilibrium constants,
​
Zn(IO3) 2 Ksp = 3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" >
Zn(NH3) 42+ Kf  = 3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" >
​
Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) .
Zn(IO3) 2(s) + 4NH3(aq)  3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" >Zn(NH3) 42+(aq) + 2IO3-(aq)

Accepted Answer

A)   3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   3) 2 Ksp =   Zn(NH3) 42+ Kf  =   ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq)   Zn(NH3) 42+(aq) + 2IO3-(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 9

If 430 mL of 1 × 10-4 M Ca(NO3) 2 is mixed with 430 mL of 1 × 10-4 M NaF,what will occur? For CaF2,Ksp = 3.4 × 10-11.

Accepted Answer

A)  No precipitate will form.
B)  Sodium nitrate will precipitate.
C)  Calcium nitrate will precipitate.
D)  Calcium fluoride will precipitate.
E)  Sodium fluoride will precipitate.

Question 10

What is the solubility product expression for Zn3(PO4) 2?

Accepted Answer

A)  Ksp = [Zn32+][(PO43-) 2]
B)  Ksp = [3Zn2+]3[2PO43-]2
C)  Ksp = [Zn2+][2PO43-]
D)  Ksp = [Zn3+]2[PO42-]3
E)  Ksp = [Zn2+]3[PO43-]2

Question 11

The solubility of La(IO3) 3 in a 0.71 M KIO3 solution is 1.0 ×10-7 mol/L.Calculate Ksp for La(IO3) 3.

Accepted Answer

A)  7.1 × 10-8
B)  3.6 × 10-22
C)  3.6 × 10-1
D)  3.6 × 10-8
E)  none of these

Question 12

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) 2? For Ni(OH) 2,Ksp = 2.0 × 10-15.

Accepted Answer

A)  2.8 × 10-3 M
B)  7.9 × 10-6 M
C)  1.0 × 10-7 M
D)  2.7 × 10-2 M
E)  1.6 × 10-5 M

Question 13

In which of the following solutions would silver(I) phosphate,Ag3PO4,be least soluble?

Accepted Answer

A)  0.10 M Na3PO4
B)  0.10 M AgNO3
C)  0.10 M Na2HPO4
D)  0.10 M HNO3
E)  0.10 M NaH2PO4

Question 14

You have two salts,AgX and AgY,with very similar Ksp values.You know that Ka for HX is much greater than Ka for HY.Which statement will be true?

Accepted Answer

A)  AgX and AgY are less soluble in acidic solution than in pure water.
B)  AgX is more soluble in acidic solution.
C)  AgX and AgY are equally soluble in acidic solution.
D)  AgY is more soluble in acidic solution.
E)  none of these

Question 15

Which of the following salts has the lowest molar solubility?

Accepted Answer

A)  SrCO3 (Ksp = 9.3 × 10-10) 
B)  MnS (Ksp = 2.5 × 10-10) 
C)  BaF2 (Ksp = 1 × 10-6) 
D)  BaSO4 (Ksp = 1.1 × 10-10) 
E)  AgCl (Ksp = 1.8 × 10-10)

Exam 17: Solubility and Complex-Ion Equilibria

The solubility of La(IO₃) ₃ in a 0.71 M KIO₃ solution is 1.0 ×10^-7 mol/L.Calculate K_sp for La(IO₃) ₃.

Correct Answer
verified

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) ₂? For Ni(OH) ₂,K_sp = 2.0 × 10^-15.

Correct Answer
verified

Given the following equilibrium constants, Zn(IO₃) ₂ K_sp = Zn(NH₃) ₄²⁺K_f = Determine K_c for the dissolution of the sparingly soluble salt Zn(IO₃) ₂ in aqueous ammonia (shown below) . Zn(IO₃) ₂(s) + 4NH₃(aq) Zn(NH₃) ₄²⁺(aq) + 2IO₃^-(aq)

Correct Answer
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What is the solubility product expression for Zn₃(PO₄) ₂?

Correct Answer
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What is the maximum Sr²⁺ concentration possible in a solution that has a M sulfide-ion concentration without precipitating strontium sulfate? For SrSO₄,K_sp = 2.5 × 10^-7.

Correct Answer
verified

Suppose 50.00 mL of 2.0 × 10^-6 M Fe(NO₃) ₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃) ₃,K_sp = 1.0 × 10^-14.

Correct Answer
verified

An aqueous solution of Ag(CN) ₂− is made by combining 0.0100 moles AgNO₃ with 1.00 mole NaCN and diluting to 1.000 L.What is the molar concentration of Ag⁺ in the solution? Ag⁺(aq) + 2CN^-(aq) Ag(CN) ₂^-(aq) ; K_f = 5.6 × 10¹⁸

Correct Answer
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You have two salts,AgX and AgY,with very similar K_sp values.You know that K_a for HX is much greater than K_a for HY.Which statement will be true?

Correct Answer
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In which of the following solutions would CaC₂O₄ have the highest molar solubility?

Correct Answer
verified

What is the solubility product expression for La₂(CO₃) ₃?

Correct Answer
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How many moles of CaF₂ will dissolve in 3.0 L of 0.041 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

Correct Answer
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If 430 mL of 1 × 10^-4 M Ca(NO₃) ₂ is mixed with 430 mL of 1 × 10^-4 M NaF,what will occur? For CaF₂,K_sp = 3.4 × 10^-11.

Correct Answer
verified

Which of the following salts has the lowest molar solubility?

Correct Answer
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In which of the following solutions would silver(I) phosphate,Ag₃PO₄,be least soluble?

Correct Answer
verified

The best explanation for the dissolution of ZnS in dilute HCl is that

Correct Answer
verified

Exam 17: Solubility and Complex-Ion Equilibria

The solubility of La(IO3) 3 in a 0.71 M KIO3 solution is 1.0 ×10-7 mol/L.Calculate Ksp for La(IO3) 3.

Correct AnswerverifiedShow Answer

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) 2? For Ni(OH) 2,Ksp = 2.0 × 10-15.

Correct AnswerverifiedShow Answer

Given the following equilibrium constants, ​ Zn(IO3) 2 Ksp = Zn(NH3) 42+ Kf = ​ Determine Kc for the dissolution of the sparingly soluble salt Zn(IO3) 2 in aqueous ammonia (shown below) . Zn(IO3) 2(s) + 4NH3(aq) Zn(NH3) 42+(aq) + 2IO3-(aq)

Correct AnswerverifiedShow Answer

What is the solubility product expression for Zn3(PO4) 2?

Correct AnswerverifiedShow Answer

What is the maximum Sr2+ concentration possible in a solution that has a M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4,Ksp = 2.5 × 10-7.

Correct AnswerverifiedShow Answer

Suppose 50.00 mL of 2.0 × 10-6 M Fe(NO3) 3 is added to 50.00 mL of 2.0 ×10-4 M KIO3.Which of the following statements is true? For Fe(IO3) 3,Ksp = 1.0 × 10-14.

Correct AnswerverifiedShow Answer

An aqueous solution of Ag(CN) 2− is made by combining 0.0100 moles AgNO3 with 1.00 mole NaCN and diluting to 1.000 L.What is the molar concentration of Ag+ in the solution? Ag+(aq) + 2CN-(aq) Ag(CN) 2-(aq) ; Kf = 5.6 × 1018

Correct AnswerverifiedShow Answer

You have two salts,AgX and AgY,with very similar Ksp values.You know that Ka for HX is much greater than Ka for HY.Which statement will be true?

Correct AnswerverifiedShow Answer

In which of the following solutions would CaC2O4 have the highest molar solubility?

Correct AnswerverifiedShow Answer

What is the solubility product expression for La2(CO3) 3?

Correct AnswerverifiedShow Answer

How many moles of CaF2 will dissolve in 3.0 L of 0.041 M NaF solution? (Ksp for CaF2 = 4.0 × 10-11)

Correct AnswerverifiedShow Answer

If 430 mL of 1 × 10-4 M Ca(NO3) 2 is mixed with 430 mL of 1 × 10-4 M NaF,what will occur? For CaF2,Ksp = 3.4 × 10-11.

Correct AnswerverifiedShow Answer

Which of the following salts has the lowest molar solubility?

Correct AnswerverifiedShow Answer

In which of the following solutions would silver(I) phosphate,Ag3PO4,be least soluble?

Correct AnswerverifiedShow Answer

The best explanation for the dissolution of ZnS in dilute HCl is that

Correct AnswerverifiedShow Answer

The solubility of La(IO₃) ₃ in a 0.71 M KIO₃ solution is 1.0 ×10^-7 mol/L.Calculate K_sp for La(IO₃) ₃.

Correct Answer
verified

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) ₂? For Ni(OH) ₂,K_sp = 2.0 × 10^-15.

Correct Answer
verified

Given the following equilibrium constants, Zn(IO₃) ₂ K_sp = Zn(NH₃) ₄²⁺K_f = Determine K_c for the dissolution of the sparingly soluble salt Zn(IO₃) ₂ in aqueous ammonia (shown below) . Zn(IO₃) ₂(s) + 4NH₃(aq) Zn(NH₃) ₄²⁺(aq) + 2IO₃^-(aq)

Correct Answer
verified

What is the solubility product expression for Zn₃(PO₄) ₂?

Correct Answer
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What is the maximum Sr²⁺ concentration possible in a solution that has a M sulfide-ion concentration without precipitating strontium sulfate? For SrSO₄,K_sp = 2.5 × 10^-7.

Correct Answer
verified

Suppose 50.00 mL of 2.0 × 10^-6 M Fe(NO₃) ₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃) ₃,K_sp = 1.0 × 10^-14.

Correct Answer
verified

An aqueous solution of Ag(CN) ₂− is made by combining 0.0100 moles AgNO₃ with 1.00 mole NaCN and diluting to 1.000 L.What is the molar concentration of Ag⁺ in the solution? Ag⁺(aq) + 2CN^-(aq) Ag(CN) ₂^-(aq) ; K_f = 5.6 × 10¹⁸

Correct Answer
verified

You have two salts,AgX and AgY,with very similar K_sp values.You know that K_a for HX is much greater than K_a for HY.Which statement will be true?

Correct Answer
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In which of the following solutions would CaC₂O₄ have the highest molar solubility?

Correct Answer
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What is the solubility product expression for La₂(CO₃) ₃?

Correct Answer
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How many moles of CaF₂ will dissolve in 3.0 L of 0.041 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

Correct Answer
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If 430 mL of 1 × 10^-4 M Ca(NO₃) ₂ is mixed with 430 mL of 1 × 10^-4 M NaF,what will occur? For CaF₂,K_sp = 3.4 × 10^-11.

Correct Answer
verified

Correct Answer
verified

In which of the following solutions would silver(I) phosphate,Ag₃PO₄,be least soluble?

Correct Answer
verified

Correct Answer
verified