What volume of 5.00 × 10-3 M HNO3 is needed to titrate 100.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

A) 12.5 mL B) 50.0 mL C) 100.mL D) 200.mL A) 12.5 mL B) 50.0 mL C) 100.mL D) 200.mL

The following pictures represent solutions at various points in the titration of a weak acid HA with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0 initially present,OHS1U1P1-S1S1P0 initially present and solvent water molecules have been omitted for clarity). -Which picture represents the solution before the equivalence point?

A) (1) B) (2) C) (3) D) (4) A) (1) B) (2) C) (3) D) (4)

What is the common ion in a solution prepared by mixing 0.55 M LiCH3CO2 with 0.10 M CH3CO2H?

A) H3O+ B) Li+ C) CH3CO2- D) OH- A) H3O+ B) Li+ C) CH3CO2- D) OH-

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH3NH2,with 25.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

A) 10.27 B) 10.57 C) 10.87 D) 11.78 A) 10.27 B) 10.57 C) 10.87 D) 11.78

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH. -Which point a-d represents pKa2?

A) point a B) point b C) point c D) point d A) point a B) point b C) point c D) point d

What is the molar solubility of AgCl in 0.10 M NH3? Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(NH3)2+ is 1.7 × 107.

A) 1.3 × 10-5 M B) 5.0 × 10-3 M C) 5.5 × 10-3 M D) 5.5 × 10-2 M A) 1.3 × 10-5 M B) 5.0 × 10-3 M C) 5.5 × 10-3 M D) 5.5 × 10-2 M

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 20.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

A) 8.86 B) 10.26 C) 9.65 D) 11.13 A) 8.86 B) 10.26 C) 9.65 D) 11.13

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.

A) 5.6 × 10-10 M B) 5.6 × 10-8 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M A) 5.6 × 10-10 M B) 5.6 × 10-8 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M

What is the molar solubility of AgCl in 0.50 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021.

A) 0.25 M B) 0.50 M C) 1.0 M D) 2.0 M A) 0.25 M B) 0.50 M C) 1.0 M D) 2.0 M

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

A) (1) B) (2) C) (3) D) (4) A) (1) B) (2) C) (3) D) (4)

The following pictures represent solutions of CuS,which may also contain ions other than CuS1U1P12+S1S1P0 and SS1U1P12-S1S1P0 which are not shown.Gray spheres represent CuS1U1P12+S1S1P0 ions and dotted spheres represent SS1U1P12-S1S1P0 ions. -If solution (1)is a saturated solution of CuS,which of solutions (2)-(4)are saturated?

A) (2) B) (3) C) (4) D) None of these A) (2) B) (3) C) (4) D) None of these

Exam 16: Applications of Aqueous Equilibria

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1.8 × 10^-5. HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

(Multiple Choice)

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Question 141

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with potassium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq)+ KOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)

(Multiple Choice)

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Question 142

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 100.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

(Multiple Choice)

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Question 143

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HCl and CH₃CH₂NH₂ is ________.

(Essay)

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Question 144

What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?

(Short Answer)

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Question 145

The following pictures represent solutions at various points in the titration of a weak acid HA with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent A^- ions.(K⁺,H₃O⁺ initially present,OH^- initially present and solvent water molecules have been omitted for clarity). -Which picture represents the solution before the equivalence point?

(Multiple Choice)

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Question 146

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H₂PO₄^- and 0.100 M HPO₄^2- and the K_a2 = 6.2 × 10^-8?

(Multiple Choice)

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Question 147

What is the common ion in a solution prepared by mixing 0.55 M LiCH₃CO₂ with 0.10 M CH₃CO₂H?

(Multiple Choice)

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Question 148

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

(Multiple Choice)

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Question 149

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents pK_a2?

(Multiple Choice)

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Question 150

What is the K_a of the amino acid glutamine if it is 33.0% dissociated at pH = 8.82?

(Short Answer)

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Question 151

What is the pH of 1 L of 0.30 M TRIS,0.60 M TRISH⁺ buffer to which one has added 5.0 mL of 12 M HCl? The K_b for the TRIS/TRISH⁺ is 1.2 × 10^-6.

(Multiple Choice)

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Question 152

What is the molar solubility of AgCl in 0.10 M NH₃? K_sp for AgCl is 1.8 × 10^-10 and the K_f for Ag(NH₃)₂⁺ is 1.7 × 10⁷.

(Multiple Choice)

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Question 153

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 20.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

(Multiple Choice)

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Question 154

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_spfor Mg(OH)₂ is 5.6 × 10^-12.

(Multiple Choice)

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Question 155

What is the molar solubility of AgCl in 0.50 M NaCN if the colorless complex ion Ag(CN)₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN)₂^- is 1.0 × 10²¹.

(Multiple Choice)

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Question 156

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

(Multiple Choice)

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Question 157

Which is a net ionic equation for the neutralization of a strong acid with a strong base?

(Multiple Choice)

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Question 158

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which points a-d represent the half-equivalence point and the equivalence point,respectively,for the titration of a weak acid?

(Multiple Choice)

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Question 159

The following pictures represent solutions of CuS,which may also contain ions other than Cu²⁺ and S^2- which are not shown.Gray spheres represent Cu²⁺ ions and dotted spheres represent S^2- ions. -If solution (1)is a saturated solution of CuS,which of solutions (2)-(4)are saturated?

(Multiple Choice)

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Question 160

Showing 141 - 160 of 201

Exam 16: Applications of Aqueous Equilibria

What is the approximate value of the equilibrium constant,Kn,for the neutralization of nitrous acid with ammonia,shown in the equation below? The Ka for HNO2 is 4.5 × 10-4 and the Kb for NH3 is 1.8 × 10-5. HNO2(aq)+ NH3(aq)⇌ NH4NO2(aq)

What is the approximate value of the equilibrium constant,Kn,for the neutralization of acetic acid with potassium hydroxide,shown in the equation below? The Ka for acetic acid is 1.8 × 10-5. CH3CO2H(aq)+ KOH(aq)⇌ H2O(l)+ NaCH3CO2(aq)

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 100.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HCl and CH3CH2NH2 is ________.

What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H2PO4- and 0.100 M HPO42- and the Ka2 = 6.2 × 10-8?

What is the common ion in a solution prepared by mixing 0.55 M LiCH3CO2 with 0.10 M CH3CO2H?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH3NH2,with 25.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -Which point a-d represents pKa2?

What is the Ka of the amino acid glutamine if it is 33.0% dissociated at pH = 8.82?

What is the pH of 1 L of 0.30 M TRIS,0.60 M TRISH+ buffer to which one has added 5.0 mL of 12 M HCl? The Kb for the TRIS/TRISH+ is 1.2 × 10-6.

What is the molar solubility of AgCl in 0.10 M NH3? Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(NH3)2+ is 1.7 × 107.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 20.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.

What is the molar solubility of AgCl in 0.50 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021.

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A- ions.(K+,H3O+,OH-,and solvent H2O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

Which is a net ionic equation for the neutralization of a strong acid with a strong base?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which points a-d represent the half-equivalence point and the equivalence point,respectively,for the titration of a weak acid?

The following pictures represent solutions of CuS,which may also contain ions other than Cu2+ and S2- which are not shown.Gray spheres represent Cu2+ ions and dotted spheres represent S2- ions. -If solution (1)is a saturated solution of CuS,which of solutions (2)-(4)are saturated?

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What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1.8 × 10^-5. HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with potassium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq)+ KOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 100.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HCl and CH₃CH₂NH₂ is ________.

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H₂PO₄^- and 0.100 M HPO₄^2- and the K_a2 = 6.2 × 10^-8?

What is the common ion in a solution prepared by mixing 0.55 M LiCH₃CO₂ with 0.10 M CH₃CO₂H?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents pK_a2?

What is the K_a of the amino acid glutamine if it is 33.0% dissociated at pH = 8.82?

What is the pH of 1 L of 0.30 M TRIS,0.60 M TRISH⁺ buffer to which one has added 5.0 mL of 12 M HCl? The K_b for the TRIS/TRISH⁺ is 1.2 × 10^-6.

What is the molar solubility of AgCl in 0.10 M NH₃? K_sp for AgCl is 1.8 × 10^-10 and the K_f for Ag(NH₃)₂⁺ is 1.7 × 10⁷.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 20.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_spfor Mg(OH)₂ is 5.6 × 10^-12.

What is the molar solubility of AgCl in 0.50 M NaCN if the colorless complex ion Ag(CN)₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN)₂^- is 1.0 × 10²¹.

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

The following pictures represent solutions of CuS,which may also contain ions other than Cu²⁺ and S^2- which are not shown.Gray spheres represent Cu²⁺ ions and dotted spheres represent S^2- ions. -If solution (1)is a saturated solution of CuS,which of solutions (2)-(4)are saturated?