What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 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) 8.25 B) 9.28 C) 10.26 D) 11.13 A) 8.25 B) 9.28 C) 10.26 D) 11.13

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is 5.6 × 10-12.

A) 1.8 × 10-10 M B) 5.6 × 10-9 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M A) 1.8 × 10-10 M B) 5.6 × 10-9 M C) 2.4 × 10-6 M D) 1.1 × 10-4 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

Determine the molar solubility for Pb3(PO4)2 in pure water.Ksp for Pb3(PO4)2 is 1.0 × 10-54.

A) 4.1 × 10-28 M B) 5.8 × 10-10 M C) 1.1 × 10-11 M D) 6.2 × 10-12 M E) 1.0 × 10-54 M A) 4.1 × 10-28 M B) 5.8 × 10-10 M C) 1.1 × 10-11 M D) 6.2 × 10-12 M E) 1.0 × 10-54 M

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3.The Kb for NH3 is 1.8 × 10-5.

A) 9.13 B) 9.25 C) 9.53 D) 4.74 E) 8.98 A) 9.13 B) 9.25 C) 9.53 D) 4.74 E) 8.98

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

A) 6.44 B) 1.48 C) 2.00 D) 12.52 E) 12.00 A) 6.44 B) 1.48 C) 2.00 D) 12.52 E) 12.00

A sample contains MgNH4(PO4)2, Sb2S3,KBr,Cr(OH)3,and PbCl2.Identify the precipitate after the addition of 6 M HCl.

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

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.060 M NaC2H3O2.Which of the following actions will destroy the buffer?

A) adding 0.060 moles of NaC2H3O2 B) adding 0.060 moles of HC2H3O2 C) adding 0.060 moles of HCl D) adding 0.060 moles of KOH E) All of the above will destroy the buffer. A) adding 0.060 moles of NaC2H3O2 B) adding 0.060 moles of HC2H3O2 C) adding 0.060 moles of HCl D) adding 0.060 moles of KOH E) All of the above will destroy the buffer.

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

A) 4.89 B) 9.11 C) 4.74 D) 9.26 E) 4.60 A) 4.89 B) 9.11 C) 4.74 D) 9.26 E) 4.60

Calculate K. Cu(OH)2(aq)⇌ Cu2+(aq)+ 2 OH-(aq)Ksp = 1.6 × 10-19 Cu2+(aq)+ 4 NH3(aq)⇌ Cu(NH3)42+(aq)Kf = 1.7 × 1013 Cu(OH)2(aq)+ 4 NH3(aq)⇌ Cu(NH3)42+(aq)+ 2 OH-(aq)K = ?

A) 1.06 × 1032 B) 3.7 × 105 C) 9.4 × 10-33 D) 2.7 × 10-6 E) 1.7 × 1013 A) 1.06 × 1032 B) 3.7 × 105 C) 9.4 × 10-33 D) 2.7 × 10-6 E) 1.7 × 1013

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

A) 6.5 × 10-5 M B) 1.3 × 10-4 M C) 3.2 × 10-4 M D) 6.8 × 10-2 M A) 6.5 × 10-5 M B) 1.3 × 10-4 M C) 3.2 × 10-4 M D) 6.8 × 10-2 M

Exam 17: Aqueous Ionic Equilibrium

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 5.00 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 141

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 142

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is 5.6 × 10^-¹².

(Multiple Choice)

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Question 143

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 144

Determine the molar solubility for Pb₃(PO₄)₂ in pure water.Ksp for Pb₃(PO₄)₂ is 1.0 × 10^-54.

(Multiple Choice)

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Question 145

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 100.0 mL of 0.20 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 146

Identify the indicator that can be used at the highest pH.

(Multiple Choice)

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Question 147

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 148

A sample contains MgNH₄(PO₄)₂,Sb₂S₃,KBr,Cr(OH)₃,and PbCl₂.Identify the precipitate after the addition of 6 M HCl.

(Multiple Choice)

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Question 149

A 1.0 L buffer solution is 0.250 M HC₂H₃O₂ and 0.060 M NaC₂H₃O₂.Which of the following actions will destroy the buffer?

(Multiple Choice)

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Question 150

What is the pH of a solution made by mixing 30.00 mL of 0.10 M HI with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.

(Multiple Choice)

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Question 151

Calculate the pH of a buffer that is 0.225 M HC₂H₃O₂ and 0.162 M KC₂H₃O₂.The K_a for HC₂H₃O₂ is 1.8 × 10^-5.

(Multiple Choice)

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Question 152

A 100.0 mL sample of 0.10 M Ba(OH)₂ is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 100.0 mL HCl.

(Multiple Choice)

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Question 153

Calculate K. Cu(OH)₂(aq)⇌ Cu²⁺(aq)+ 2 OH^-(aq)K_sp = 1.6 × 10^-19 Cu²⁺(aq)+ 4 NH₃(aq)⇌ Cu(NH₃)₄²⁺(aq)K_f = 1.7 × 10¹³ Cu(OH)₂(aq)+ 4 NH₃(aq)⇌ Cu(NH₃)₄²⁺(aq)+ 2 OH^-(aq)K = ?

(Multiple Choice)

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Question 154

Identify the compound that is base-insoluble.

(Multiple Choice)

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Question 155

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 156

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

(Multiple Choice)

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Question 157

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K_sp (AgBr)= 7.7 × 10^-13.

(Multiple Choice)

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Question 158

A 110.0 mL sample of 0.20 M HF is titrated with 0.10 M CsOH.Determine the pH of the solution after the addition of 440.0 mL of CsOH.The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 159

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO₃ and 0.50 M Ba(NO₃)₂.What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-1⁰,respectively.

(Multiple Choice)

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Question 160

Showing 141 - 160 of 187

Exam 17: Aqueous Ionic Equilibrium

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 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 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HF is 3.5 × 10-4.

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is 5.6 × 10-12.

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

Determine the molar solubility for Pb3(PO4)2 in pure water.Ksp for Pb3(PO4)2 is 1.0 × 10-54.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3.The Kb for NH3 is 1.8 × 10-5.

Identify the indicator that can be used at the highest pH.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

A sample contains MgNH4(PO4)2, Sb2S3,KBr,Cr(OH)3,and PbCl2.Identify the precipitate after the addition of 6 M HCl.

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.060 M NaC2H3O2.Which of the following actions will destroy the buffer?

What is the pH of a solution made by mixing 30.00 mL of 0.10 M HI with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

A 100.0 mL sample of 0.10 M Ba(OH)2 is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 100.0 mL HCl.

Calculate K. Cu(OH)2(aq)⇌ Cu2+(aq)+ 2 OH-(aq)Ksp = 1.6 × 10-19 Cu2+(aq)+ 4 NH3(aq)⇌ Cu(NH3)42+(aq)Kf = 1.7 × 1013 Cu(OH)2(aq)+ 4 NH3(aq)⇌ Cu(NH3)42+(aq)+ 2 OH-(aq)K = ?

Identify the compound that is base-insoluble.

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.

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

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr)= 7.7 × 10-13.

A 110.0 mL sample of 0.20 M HF is titrated with 0.10 M CsOH.Determine the pH of the solution after the addition of 440.0 mL of CsOH.The Ka of HF is 3.5 × 10-4.

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

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What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 5.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is 5.6 × 10^-¹².

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

Determine the molar solubility for Pb₃(PO₄)₂ in pure water.Ksp for Pb₃(PO₄)₂ is 1.0 × 10^-54.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 100.0 mL of 0.20 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A sample contains MgNH₄(PO₄)₂,Sb₂S₃,KBr,Cr(OH)₃,and PbCl₂.Identify the precipitate after the addition of 6 M HCl.

A 1.0 L buffer solution is 0.250 M HC₂H₃O₂ and 0.060 M NaC₂H₃O₂.Which of the following actions will destroy the buffer?

Calculate the pH of a buffer that is 0.225 M HC₂H₃O₂ and 0.162 M KC₂H₃O₂.The K_a for HC₂H₃O₂ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 M Ba(OH)₂ is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 100.0 mL HCl.

Calculate K. Cu(OH)₂(aq)⇌ Cu²⁺(aq)+ 2 OH^-(aq)K_sp = 1.6 × 10^-19 Cu²⁺(aq)+ 4 NH₃(aq)⇌ Cu(NH₃)₄²⁺(aq)K_f = 1.7 × 10¹³ Cu(OH)₂(aq)+ 4 NH₃(aq)⇌ Cu(NH₃)₄²⁺(aq)+ 2 OH^-(aq)K = ?

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.

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K_sp (AgBr)= 7.7 × 10^-13.

A 110.0 mL sample of 0.20 M HF is titrated with 0.10 M CsOH.Determine the pH of the solution after the addition of 440.0 mL of CsOH.The K_a of HF is 3.5 × 10^-4.

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO₃ and 0.50 M Ba(NO₃)₂.What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-1⁰,respectively.