Determine the molar solubility of Fe(OH)2 in pure water.Ksp (Fe(OH)2)= 4.87 × 10-17.

A) 2.44 × 10-17 M B) 1.62 × 10-17 M C) 4.03 × 10-9 M D) 3.65 × 10-6 M E) 2.30 × 10-6 M A) 2.44 × 10-17 M B) 1.62 × 10-17 M C) 4.03 × 10-9 M D) 3.65 × 10-6 M E) 2.30 × 10-6 M

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55 A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55

Calculate the Ksp of Fe2S3 in pure water.The molar solubility is 1.05 × 10-18.

A) 7.00 × 10-88 B) 1.28 × 10-90 C) 1.40 × 10-88 D) 6.30 × 10-18 E) exceeds ability of calculator A) 7.00 × 10-88 B) 1.28 × 10-90 C) 1.40 × 10-88 D) 6.30 × 10-18 E) exceeds ability of calculator

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?

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.

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) 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

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF.Ksp (BaF2)= 1.7 × 10-6.

A) 2.3 × 10-5 M B) 8.5 × 10-7 M C) 1.2 × 10-2 M D) 0.0750 M E) 3.0 × 10-4 M A) 2.3 × 10-5 M B) 8.5 × 10-7 M C) 1.2 × 10-2 M D) 0.0750 M E) 3.0 × 10-4 M

Exam 16: Aqueous Ionic Equilibrium

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 101

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

(Multiple Choice)

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Question 102

Which solution is a buffer?

(Multiple Choice)

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Question 103

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

(Multiple Choice)

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Question 104

Match the following. -pH < 7

(Multiple Choice)

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Question 105

Give the expression for the solubility product constant for Cr₂(CO₃)₃.

(Multiple Choice)

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Question 106

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 100.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 107

What is the pH of a solution made by mixing 25.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

(Multiple Choice)

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Question 108

Which of the following is true?

(Multiple Choice)

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Question 109

Determine the molar solubility of Fe(OH)₂in pure water.K_sp (Fe(OH)₂)= 4.87 × 10^-17.

(Multiple Choice)

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Question 110

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5 for CH₃CO₂H.

(Multiple Choice)

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Question 111

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 112

Formic acid (HCO₂H,K_a = 1.8 × 10^-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

(Multiple Choice)

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Question 113

Calculate the Ksp of Fe₂S₃ in pure water.The molar solubility is 1.05 × 10^-18.

(Multiple Choice)

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Question 114

If the pK_a of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.74,which of the following is true?

(Multiple Choice)

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Question 115

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?

(Multiple Choice)

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Question 116

Which of the following compounds will have the highest molar solubility in pure water?

(Multiple Choice)

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Question 117

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K_a = 6.76 × 10^-4 for HF.

(Multiple Choice)

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Question 118

Determine the molar solubility of BaF₂ in a solution containing 0.0750 M LiF.K_sp (BaF₂)= 1.7 × 10^-6.

(Multiple Choice)

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Question 119

Which of the following solutions is a good buffer system?

(Multiple Choice)

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Question 120

Showing 101 - 120 of 148

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

Which solution is a buffer?

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

Match the following. -pH < 7

Give the expression for the solubility product constant for Cr₂(CO₃)₃.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 100.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

What is the pH of a solution made by mixing 25.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

Which of the following is true?

Determine the molar solubility of Fe(OH)₂in pure water.K_sp (Fe(OH)₂)= 4.87 × 10^-17.

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5 for CH₃CO₂H.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Formic acid (HCO₂H,K_a = 1.8 × 10^-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

Calculate the Ksp of Fe₂S₃ in pure water.The molar solubility is 1.05 × 10^-18.

If the pK_a of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.74,which of the following is true?

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?

Which of the following compounds will have the highest molar solubility in pure water?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K_a = 6.76 × 10^-4 for HF.

Determine the molar solubility of BaF₂ in a solution containing 0.0750 M LiF.K_sp (BaF₂)= 1.7 × 10^-6.

Which of the following solutions is a good buffer system?

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Exam 16: Aqueous Ionic Equilibrium

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 × 10-8 for HOCl.

Which solution is a buffer?

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

Match the following. -pH < 7

Give the expression for the solubility product constant for Cr2(CO3)3.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 100.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

What is the pH of a solution made by mixing 25.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

Which of the following is true?

Determine the molar solubility of Fe(OH)2 in pure water.Ksp (Fe(OH)2)= 4.87 × 10-17.

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.34? Ka = 1.8 × 10-5 for CH3CO2H.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

Formic acid (HCO2H,Ka = 1.8 × 10-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

Calculate the Ksp of Fe2S3 in pure water.The molar solubility is 1.05 × 10-18.

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?

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?

Which of the following compounds will have the highest molar solubility in pure water?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? Ka = 6.76 × 10-4 for HF.

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF.Ksp (BaF2)= 1.7 × 10-6.

Which of the following solutions is a good buffer system?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Free Energy and Thermodynamics

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A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

Give the expression for the solubility product constant for Cr₂(CO₃)₃.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 100.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

Determine the molar solubility of Fe(OH)₂in pure water.K_sp (Fe(OH)₂)= 4.87 × 10^-17.

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5 for CH₃CO₂H.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Formic acid (HCO₂H,K_a = 1.8 × 10^-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

Calculate the Ksp of Fe₂S₃ in pure water.The molar solubility is 1.05 × 10^-18.

If the pK_a of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.74,which of the following is true?

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?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K_a = 6.76 × 10^-4 for HF.

Determine the molar solubility of BaF₂ in a solution containing 0.0750 M LiF.K_sp (BaF₂)= 1.7 × 10^-6.