Question 1

Give the expression for Kf for Fe(CN)63-.

Accepted Answer

A)    
B)    
C)    
D)  [Fe3+] [CN-]6 
E)    
A)    
B)    
C)    
D)  [Fe3+] [CN-]6 
E)

Question 2

A 650.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M NaOH.Determine the pH of the solution after the addition of 650.0 mL of NaOH.

Accepted Answer

A)  13.13 
B)  12.65 
C)  1.35 
D)  0.87 
E)  12.95 
A)  13.13 
B)  12.65 
C)  1.35 
D)  0.87 
E)  12.95

Question 3

Which of the following compounds solubility will NOT be affected by a low pH in solution?

Accepted Answer

A)  AgCl 
B)  Sr(OH)2 
C)  CaF2 
D)  CuS 
E)  SrCO3 
A)  AgCl 
B)  Sr(OH)2 
C)  CaF2 
D)  CuS 
E)  SrCO3

Question 4

Calculate the molar solubility of thallium chloride in 0.50 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

Accepted Answer

A)  8.5 × 10-5 M 
B)  3.4 × 10-4 M 
C)  9.2 × 10-3 M 
D)  1.3 × 10-2 M 
A)  8.5 × 10-5 M 
B)  3.4 × 10-4 M 
C)  9.2 × 10-3 M 
D)  1.3 × 10-2 M

Question 5

When titrating a weak base with a monoprotic acid at 25°C,the

Accepted Answer

A)  pH will be 7 at the equivalence point. 
B)  pH will be greater than 7 at the equivalence point. 
C)  titration will require more moles of the base than acid to reach the equivalence point. 
D)  titration will require more moles of acid than base to reach the equivalence point. 
E)  pH will be less than 7 at the equivalence point. 
A)  pH will be 7 at the equivalence point. 
B)  pH will be greater than 7 at the equivalence point. 
C)  titration will require more moles of the base than acid to reach the equivalence point. 
D)  titration will require more moles of acid than base to reach the equivalence point. 
E)  pH will be less than 7 at the equivalence point.

Question 6

What is the hydronium ion concentration in a solution prepared by mixing 150.0 mL of 0.10 M HCN with 150.0 mL of 0.050 M NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 × 10-10 for HCN.

Accepted Answer

A)  2.4 × 10-10 M 
B)  4.9 × 10-10 M 
C)  9.8 × 10-10 M 
D)  7.0 × 10-6 M 
A)  2.4 × 10-10 M 
B)  4.9 × 10-10 M 
C)  9.8 × 10-10 M 
D)  7.0 × 10-6 M

Question 7

A 500.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M CsOH.Determine the pH of the solution after the addition of 250.0 mL of CsOH.

Accepted Answer

A)  12.48 
B)  0.68 
C)  2.35 
D)  1.52 
E)  3.22 
A)  12.48 
B)  0.68 
C)  2.35 
D)  1.52 
E)  3.22

Question 8

A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF.If the Kf for AlF63- is 7 × 1019,how much aluminum ion remains at equilibrium?

Accepted Answer

A)  1.1 × 10-19 M 
B)  3.1 × 10-22 M 
C)  9.1 × 10-19 M 
D)  1.9 × 10-21 M 
E)  4.4 × 10-20 M 
A)  1.1 × 10-19 M 
B)  3.1 × 10-22 M 
C)  9.1 × 10-19 M 
D)  1.9 × 10-21 M 
E)  4.4 × 10-20 M

Question 9

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+.When the concentration of   exceeds ________ M,BaF2 will precipitate.Neglect volume changes.For BaF2,Ksp = 1.7 × 10-6.

Accepted Answer

A)  5.9 × 10-5 
B)  1.1 × 10-2 
C)  2.4 × 10-8 
D)  2.7 × 10-3 
E)  1.2 × 10-4 
A)  5.9 × 10-5 
B)  1.1 × 10-2 
C)  2.4 × 10-8 
D)  2.7 × 10-3 
E)  1.2 × 10-4

Question 10

Identify the salts that are in hard water.

Accepted Answer

A)  CaCO3 and MgCO3 
B)  MgSO4 and CaSO4 
C)  NaCl and KBr 
D)  KHSO4 and Na2SO4 
E)  NaOCl and HOCl 
A)  CaCO3 and MgCO3 
B)  MgSO4 and CaSO4 
C)  NaCl and KBr 
D)  KHSO4 and Na2SO4 
E)  NaOCl and HOCl

Question 11

In which of the following solutions would solid AgCl  be expected to be the least soluble at 25°C?

Accepted Answer

A)  0.1 M HCl 
B)  0.1 M KCl 
C)  0.1 M BaCl2 
D)  0.1 M NH4NO3 
A)  0.1 M HCl 
B)  0.1 M KCl 
C)  0.1 M BaCl2 
D)  0.1 M NH4NO3

Question 12

A 200.0 mL sample of 0.18 M HClO4 is titrated with 0.36 M NaOH.Determine the pH of the solution before the addition of any NaOH.

Accepted Answer

A)  1.74 
B)  1.05 
C)  0.74 
D)  0.57 
E)  1.57 
A)  1.74 
B)  1.05 
C)  0.74 
D)  0.57 
E)  1.57

Question 13

Determine the molar solubility of AgI in pure water.Ksp (AgI)= 8.51 × 10-17.

Accepted Answer

A)  9.22 × 10-9 M 
B)  4.26 × 10-17 M 
C)  8.51 × 10-17 M 
D)  2.77 × 10-6 M 
E)  4.40 × 10-6 M 
A)  9.22 × 10-9 M 
B)  4.26 × 10-17 M 
C)  8.51 × 10-17 M 
D)  2.77 × 10-6 M 
E)  4.40 × 10-6 M

Question 14

A sample contains MgNH4(PO4)2, Sb2S3,KBr,Cr(OH)3,and PbCl2.Identify the precipitate after the addition of 6 M HCl; then H2S and 0.2 M HCl; and then OH- to a pH of 8.

Accepted Answer

A)  MgNH4(PO4)2 
B)  Sb2S3 
C)  KBr 
D)  Cr(OH)3 
E)  PbCl2 
A)  MgNH4(PO4)2 
B)  Sb2S3 
C)  KBr 
D)  Cr(OH)3 
E)  PbCl2

Question 15

A ligand is a molecule or ion that acts as a

Accepted Answer

A)  Lewis acid. 
B)  Brønsted-Lowry base. 
C)  Arrhenius base. 
D)  Lewis base. 
E)  conjugate base. 
A)  Lewis acid. 
B)  Brønsted-Lowry base. 
C)  Arrhenius base. 
D)  Lewis base. 
E)  conjugate base.

Question 16

Which of the following is TRUE?

Accepted Answer

A)  The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. 
B)  At the equivalence point, the pH is always 7. 
C)  An indicator is not pH sensitive. 
D)  A titration curve is a plot of pH vs. the [base]/[acid] ratio. 
E)  None of the above is true. 
A)  The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. 
B)  At the equivalence point, the pH is always 7. 
C)  An indicator is not pH sensitive. 
D)  A titration curve is a plot of pH vs. the [base]/[acid] ratio. 
E)  None of the above is true.

Question 17

Give the expression for the solubility product constant for Ca3(PO4)2.

Accepted Answer

A)    
B)    
C)    
D)  [ Ca2+]2[ PO43-]3 
E)  [Ca2+]3[PO43-]2 
A)    
B)    
C)    
D)  [ Ca2+]2[ PO43-]3 
E)  [Ca2+]3[PO43-]2

Question 18

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.74,which of the following is TRUE?

Accepted Answer

A)  [HCHO2] > [NaCHO2] 
B)  [HCHO2] = [NaCHO2] 
C)  [HCHO2] 2] 
D)  [HCHO2] 2] 
E)  It is not possible to make a buffer of this pH from HCHO2 and NaCHO2. 
A)  [HCHO2] > [NaCHO2] 
B)  [HCHO2] = [NaCHO2] 
C)  [HCHO2] 2] 
D)  [HCHO2] 2] 
E)  It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

Question 19

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH3NH2,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+.

Accepted Answer

A)  2.77 
B)  4.09 
C)  9.91 
D)  11.23 
A)  2.77 
B)  4.09 
C)  9.91 
D)  11.23

Question 20

A 200.0 mL sample of 0.50 M Sr(OH)2 is titrated with 0.50 M HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.

Accepted Answer

A)  2.62 
B)  2.00 
C)  1.48 
D)  12.52 
E)  7.00 
A)  2.62 
B)  2.00 
C)  1.48 
D)  12.52 
E)  7.00

Exam 17: Aqueous Ionic Equilibrium

Give the expression for Kf for Fe(CN)63-.

A 650.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M NaOH.Determine the pH of the solution after the addition of 650.0 mL of NaOH.

Which of the following compounds solubility will NOT be affected by a low pH in solution?

Calculate the molar solubility of thallium chloride in 0.50 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

When titrating a weak base with a monoprotic acid at 25°C,the

What is the hydronium ion concentration in a solution prepared by mixing 150.0 mL of 0.10 M HCN with 150.0 mL of 0.050 M NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 × 10-10 for HCN.

A 500.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M CsOH.Determine the pH of the solution after the addition of 250.0 mL of CsOH.

A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF.If the Kf for AlF63- is 7 × 1019,how much aluminum ion remains at equilibrium?

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+.When the concentration of exceeds ________ M,BaF2 will precipitate.Neglect volume changes.For BaF2,Ksp = 1.7 × 10-6.

Identify the salts that are in hard water.

In which of the following solutions would solid AgCl be expected to be the least soluble at 25°C?

A 200.0 mL sample of 0.18 M HClO4 is titrated with 0.36 M NaOH.Determine the pH of the solution before the addition of any NaOH.

Determine the molar solubility of AgI in pure water.Ksp (AgI)= 8.51 × 10-17.

A sample contains MgNH4(PO4)2, Sb2S3,KBr,Cr(OH)3,and PbCl2.Identify the precipitate after the addition of 6 M HCl; then H2S and 0.2 M HCl; and then OH- to a pH of 8.

A ligand is a molecule or ion that acts as a

Which of the following is TRUE?

Give the expression for the solubility product constant for Ca3(PO4)2.

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.74,which of the following is TRUE?

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH3NH2,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+.

A 200.0 mL sample of 0.50 M Sr(OH)2 is titrated with 0.50 M HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.

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Filters

Give the expression for K_f for Fe(CN)₆^3-.

A 650.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M NaOH.Determine the pH of the solution after the addition of 650.0 mL of NaOH.

Calculate the molar solubility of thallium chloride in 0.50 M NaCl at 25°C.K_sp for TlCl is 1.7 × 10^-⁴.

What is the hydronium ion concentration in a solution prepared by mixing 150.0 mL of 0.10 M HCN with 150.0 mL of 0.050 M NaCN? Assume that the volumes of the solutions are additive and that K_a = 4.9 × 10^-¹⁰ for HCN.

A 500.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M CsOH.Determine the pH of the solution after the addition of 250.0 mL of CsOH.

A solution contains 3.8 × 10^-2M in Al³⁺ and 0.29 M in NaF.If the K_f for AlF₆^3- is 7 × 10¹⁹,how much aluminum ion remains at equilibrium?

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺.When the concentration of exceeds ________ M,BaF₂ will precipitate.Neglect volume changes.For BaF₂,K_sp = 1.7 × 10^-6.

A 200.0 mL sample of 0.18 M HClO₄ is titrated with 0.36 M NaOH.Determine the pH of the solution before the addition of any NaOH.

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

A sample contains MgNH₄(PO₄)₂,Sb₂S₃,KBr,Cr(OH)₃,and PbCl₂.Identify the precipitate after the addition of 6 M HCl; then H₂S and 0.2 M HCl; and then OH^-to a pH of 8.

Give the expression for the solubility product constant for Ca₃(PO₄)₂.

If the pKa of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.74,which of the following is TRUE?

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH₃NH₂,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. K_a = 2.70 × 10^-11for CH₃NH₃⁺.

A 200.0 mL sample of 0.50 M Sr(OH)₂ is titrated with 0.50 M HBr.Determine the pH of the solution after the addition of 400.0 mL HBr.