Question 1

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

Accepted Answer

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

Question 2

Give the equation for a saturated solution in comparing Q with Ksp.

Accepted Answer

A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  none of the above 
A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  none of the above C

Question 3

Animals will lick up ethylene glycol (antifreeze)due to its sweet taste.The antidote for ethylene glycol poisoning is the administration of

Accepted Answer

A)  ethyl alcohol ( alcoholic drinks). 
B)  methyl alcohol (window washer fluid). 
C)  mineral oil (laxative). 
D)  vinegar. 
E)  sodium carbonate (washing soda). 
A)  ethyl alcohol ( alcoholic drinks). 
B)  methyl alcohol (window washer fluid). 
C)  mineral oil (laxative). 
D)  vinegar. 
E)  sodium carbonate (washing soda). A

Question 4

What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH3CO2H with 30.00 mL of 0.030 M CH3CO2K? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A)  2.87 
B)  4.22 
C)  4.75 
D)  5.27 
A)  2.87 
B)  4.22 
C)  4.75 
D)  5.27

Question 5

Describe what happens at high pH for aluminum hydroxide.

Accepted Answer

A)  Al(H2O)33+ precipitates. 
B)  Al(H2O)2(OH)4- dissolves. 
C)  Al(OH)5 dissolves. 
D)  Al precipitates. 
E)  Al dissolves. 
A)  Al(H2O)33+ precipitates. 
B)  Al(H2O)2(OH)4- dissolves. 
C)  Al(OH)5 dissolves. 
D)  Al precipitates. 
E)  Al dissolves.

Question 6

A sample contains MgNH4(PO4)2, Sb2S3,KBr,Cr(OH)3,and PbCl2.Identify the soluble ions after the addition of 6 M HCl; then H2S and 0.2 M HCl; then OH- to a pH of 8; and then (NH4)2HPO4 with NH3.

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 7

Calculate the solubility (in g/L)of silver chromate in water at 25°C if the Ksp for Ag2CrO4 is 1.1 × 10-12.

Accepted Answer

A)  3.5 × 10-4 g/L 
B)  2.2 × 10-2 g/L 
C)  2.7 × 10-2 g/L 
D)  3.4 × 10-2 g/L 
A)  3.5 × 10-4 g/L 
B)  2.2 × 10-2 g/L 
C)  2.7 × 10-2 g/L 
D)  3.4 × 10-2 g/L

Question 8

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A)  1.12 × 10-4 
B)  0.0450 
C)  4.25 
D)  0.342 
E)  5.53 
A)  1.12 × 10-4 
B)  0.0450 
C)  4.25 
D)  0.342 
E)  5.53

Question 9

A 900.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M NaOH.Determine the pH of the solution after the addition of 270.0 mL of NaOH.

Accepted Answer

A)  0.86 
B)  1.21 
C)  2.00 
D)  1.12 
E)  2.86 
A)  0.86 
B)  1.21 
C)  2.00 
D)  1.12 
E)  2.86

Question 10

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2.The Ka for HC7H5O2 is 6.5 × 10-5.

Accepted Answer

A)  4.19 
B)  9.69 
C)  4.49 
D)  4.31 
E)  10.51 
A)  4.19 
B)  9.69 
C)  4.49 
D)  4.31 
E)  10.51

Question 11

In the blood,the concentration of bicarbonate is ________ times higher than the concentration of carbonic acid.

Accepted Answer

A)  15 
B)  25 
C)  30 
D)  10 
E)  20 
A)  15 
B)  25 
C)  30 
D)  10 
E)  20

Question 12

What is the molar solubility of AgCl in 0.30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3)2+ is 1.7 × 107.

Accepted Answer

A)  1.3 × 10-5 M 
B)  1.6 × 10-2 M 
C)  1.7 × 10-2 M 
D)  5.5 × 10-2 M 
A)  1.3 × 10-5 M 
B)  1.6 × 10-2 M 
C)  1.7 × 10-2 M 
D)  5.5 × 10-2 M

Question 13

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2.The Ka for HCHO2 is 1.8 × 10-4.

Accepted Answer

A)  3.87 
B)  3.74 
C)  10.53 
D)  3.47 
E)  10.13 
A)  3.87 
B)  3.74 
C)  10.53 
D)  3.47 
E)  10.13

Question 14

Calculate the Ksp for hydroxide if the solubility of Sr(OH)2 in pure water is 1.42 × 101 g/L.

Accepted Answer

A)  1.16 × 10-1 
B)  6.40 × 10-3 
C)  1.42 × 101 
D)  1.60 × 10-3 
E)  7.70 × 10-11 
A)  1.16 × 10-1 
B)  6.40 × 10-3 
C)  1.42 × 101 
D)  1.60 × 10-3 
E)  7.70 × 10-11

Question 15

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3. Ksp (Al(OH)3)= 1.3 × 10-33.

Accepted Answer

A)  2.6 × 10-9 M 
B)  5.2 × 10-31 M 
C)  2.6 × 10-32 M 
D)  9.87 × 10-12 M 
E)  6.5 × 10-35 M 
A)  2.6 × 10-9 M 
B)  5.2 × 10-31 M 
C)  2.6 × 10-32 M 
D)  9.87 × 10-12 M 
E)  6.5 × 10-35 M

Question 16

Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

Accepted Answer

In order to choose an appropriate indica

Question 17

You wish to prepare an HC2H3O2 buffer with a pH of 5.14.If the pKa of is 4.74,what ratio of C2H3O2-/HC2H3O2 must you use?

Accepted Answer

A)  0.10 
B)  0.30 
C)  0.40 
D)  2.51 
E)  5.0 
A)  0.10 
B)  0.30 
C)  0.40 
D)  2.51 
E)  5.0

Question 18

The molar solubility of ZnS is 1.6 × 10-12 M in pure water.Calculate the Ksp for ZnS.

Accepted Answer

A)  8.0 × 10-13 M 
B)  3.2 × 10-12 M 
C)  1.6 × 10-35 M 
D)  2.6 × 10-24 M 
E)  6.80 × 10-5 M 
A)  8.0 × 10-13 M 
B)  3.2 × 10-12 M 
C)  1.6 × 10-35 M 
D)  2.6 × 10-24 M 
E)  6.80 × 10-5 M

Question 19

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 M NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Accepted Answer

A)  9.08 
B)  9.26 
C)  9.43 
D)  11.32 
A)  9.08 
B)  9.26 
C)  9.43 
D)  11.32

Question 20

Calculate the pH of a solution formed by mixing 120.0 mL of 0.30 M HClO with 1180.0 mL of 0.20 M KClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A)  5.99 
B)  8.01 
C)  7.54 
D)  7.06 
E)  6.46 
A)  5.99 
B)  8.01 
C)  7.54 
D)  7.06 
E)  6.46

Exam 17: Aqueous Ionic Equilibrium

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

Give the equation for a saturated solution in comparing Q with Ksp.

Animals will lick up ethylene glycol (antifreeze)due to its sweet taste.The antidote for ethylene glycol poisoning is the administration of

What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH3CO2H with 30.00 mL of 0.030 M CH3CO2K? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

Describe what happens at high pH for aluminum hydroxide.

A sample contains MgNH4(PO4)2, Sb2S3,KBr,Cr(OH)3,and PbCl2.Identify the soluble ions after the addition of 6 M HCl; then H2S and 0.2 M HCl; then OH- to a pH of 8; and then (NH4)2HPO4 with NH3.

Calculate the solubility (in g/L)of silver chromate in water at 25°C if the Ksp for Ag2CrO4 is 1.1 × 10-12.

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10-4.

A 900.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M NaOH.Determine the pH of the solution after the addition of 270.0 mL of NaOH.

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2.The Ka for HC7H5O2 is 6.5 × 10-5.

In the blood,the concentration of bicarbonate is ________ times higher than the concentration of carbonic acid.

What is the molar solubility of AgCl in 0.30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3)2+ is 1.7 × 107.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2.The Ka for HCHO2 is 1.8 × 10-4.

Calculate the Ksp for hydroxide if the solubility of Sr(OH)2 in pure water is 1.42 × 101 g/L.

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3. Ksp (Al(OH)3)= 1.3 × 10-33.

Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

You wish to prepare an HC2H3O2 buffer with a pH of 5.14.If the pKa of is 4.74,what ratio of C2H3O2-/HC2H3O2 must you use?

The molar solubility of ZnS is 1.6 × 10-12 M in pure water.Calculate the Ksp for ZnS.

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 M NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Calculate the pH of a solution formed by mixing 120.0 mL of 0.30 M HClO with 1180.0 mL of 0.20 M KClO.The Ka for HClO is 2.9 × 10-8.

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Give the equation for a saturated solution in comparing Q with K_sp.

What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH₃CO₂H with 30.00 mL of 0.030 M CH₃CO₂K? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

A sample contains MgNH₄(PO₄)₂,Sb₂S₃,KBr,Cr(OH)₃,and PbCl₂.Identify the soluble ions after the addition of 6 M HCl; then H₂S and 0.2 M HCl; then OH^-to a pH of 8; and then (NH₄)₂HPO₄ with NH₃.

Calculate the solubility (in g/L)of silver chromate in water at 25°C if the K_sp for Ag₂CrO₄ is 1.1 × 10^-¹².

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

A 900.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M NaOH.Determine the pH of the solution after the addition of 270.0 mL of NaOH.

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC₇H₅O₂ with 100.0 mL of 0.30 M NaC₇H₅O₂.The K_a for HC₇H₅O₂ is 6.5 × 10^-5.

What is the molar solubility of AgCl in 0.30 M NH₃? K_sp for AgCl is 1.8 × 10^-¹⁰ and K_f for Ag(NH₃)₂⁺ is 1.7 × 10⁷.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO₂ with 100.0 mL of 0.20 M LiCHO₂.The K_a for HCHO₂ is 1.8 × 10^-4.

Calculate the K_sp for hydroxide if the solubility of Sr(OH)₂ in pure water is 1.42 × 10¹g/L.

Determine the molar solubility of Al(OH)₃ in a solution containing 0.0500 M AlCl₃. K_sp (Al(OH)₃)= 1.3 × 10^-33.

You wish to prepare an HC₂H₃O₂ buffer with a pH of 5.14.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use?

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp for ZnS.

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 M NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

Calculate the pH of a solution formed by mixing 120.0 mL of 0.30 M HClO with 1180.0 mL of 0.20 M KClO.The K_a for HClO is 2.9 × 10^-8.