Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 mol L-1 C6H5COOH with 100.0 mL of 0.30 mol L-1 C6H5COONa.The Ka for C6H5COOH is 6.5 × 10-5.

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

What is the molar solubility of AgCl in 0.10 mol L-1 NaCN if the colourless 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) 0.050 mol L-1 B) 0.10 mol L-1 C) 0.20 mol L-1 D) 0.40 mol L-1 A) 0.050 mol L-1 B) 0.10 mol L-1 C) 0.20 mol L-1 D) 0.40 mol L-1

The molar solubility of Ag2S is 1.26 × 10-16 mol L-1 in pure water.Calculate the Ksp for Ag2S.

A) 1.59 × 10-32 B) 1.12 × 10-8 C) 6.81 × 10-63 D) 3.78 × 10-12 E) 8.00 × 10-48 A) 1.59 × 10-32 B) 1.12 × 10-8 C) 6.81 × 10-63 D) 3.78 × 10-12 E) 8.00 × 10-48

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH)2 with 50.00 mL of 0.300 mol L-1 NaOH? Assume that the volumes are additive.

A) 13.05 B) 13.10 C) 13.28 D) 13.58 A) 13.05 B) 13.10 C) 13.28 D) 13.58

Exam 16: Aqueous Ionic Equilibrium

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 mol L^-1 C₆H₅COOH with 100.0 mL of 0.30 mol L^-1 C₆H₅COONa.The K_a for C₆H₅COOH is 6.5 × 10^-5.

(Multiple Choice)

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Question 121

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

(Multiple Choice)

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Question 122

What is the molar solubility of AgCl in 0.10 mol L^-1 NaCN if the colourless 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 123

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 2.1 × 10^-5 mol L^-1 in calcium ion and 4.75 × 10^-5mol L^-1 in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

(Multiple Choice)

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Question 124

What happens at high pH to aluminum hydroxide precipitate?

(Multiple Choice)

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Question 125

Name the chemical compound that forms stalactites and stalagmites.

(Short Answer)

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Question 126

The molar solubility of ZnS is 1.6 × 10^-12 mol L^-1 in pure water.Calculate the K_sp for ZnS.

(Multiple Choice)

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Question 127

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-¹ HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

(Multiple Choice)

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Question 128

What is the pH of a solution made by mixing 25.00 mL of 0.100 mol L^-1 HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

(Multiple Choice)

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Question 129

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution before the addition of any HBr.

(Multiple Choice)

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Question 130

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

(Multiple Choice)

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Question 131

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is $4.50 \times 10 ^ { - 4 }$

(Multiple Choice)

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Question 132

The molar solubility of Ag₂S is 1.26 × 10^-16 mol L^-1 in pure water.Calculate the K_sp for Ag₂S.

(Multiple Choice)

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Question 133

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution after the addition of 100.0 mL HBr.

(Multiple Choice)

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Question 134

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

(Multiple Choice)

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Question 135

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH.Determine the pH of the solution after the addition of 200.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 136

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH)₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

(Multiple Choice)

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Question 137

Calculate the pH of a buffer that is 0.040 mol L^-1 HF and 0.020 mol L^-1 LiF.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 138

A solution is prepared by dissolving 0.23 mol of formic acid and 0.27 mol of sodium formate in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly.The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution.The $K _ { a }$ of formic acid is 1.36 × 10^-3.

(Multiple Choice)

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Question 139

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

(Multiple Choice)

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Question 140

Showing 121 - 140 of 159

Exam 16: Aqueous Ionic Equilibrium

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 mol L-1 C6H5COOH with 100.0 mL of 0.30 mol L-1 C6H5COONa.The Ka for C6H5COOH is 6.5 × 10-5.

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

What is the molar solubility of AgCl in 0.10 mol L-1 NaCN if the colourless 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 solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10-5 mol L-1 in calcium ion and 4.75 × 10-5 mol L-1 in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

What happens at high pH to aluminum hydroxide precipitate?

Name the chemical compound that forms stalactites and stalagmites.

The molar solubility of ZnS is 1.6 × 10-12 mol L-1 in pure water.Calculate the Ksp for ZnS.

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

What is the pH of a solution made by mixing 25.00 mL of 0.100 mol L-1 HCl with 40.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr.Determine the pH of the solution before the addition of any HBr.

What is the [CH3COO-]/[CH3COOH] ratio necessary to make a buffer solution with a pH of 4.34? Ka = 1.8 × 10-5 for CH3COOH.

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L-1 in nitrous acid.The acid dissociation constant of nitrous acid is 4.50×10−44.50 \times 10 ^ { - 4 }4.50×10−4

The molar solubility of Ag2S is 1.26 × 10-16 mol L-1 in pure water.Calculate the Ksp for Ag2S.

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr.Determine the pH of the solution after the addition of 100.0 mL HBr.

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH.Determine the pH of the solution after the addition of 200.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH)2 with 50.00 mL of 0.300 mol L-1 NaOH? Assume that the volumes are additive.

Calculate the pH of a buffer that is 0.040 mol L-1 HF and 0.020 mol L-1 LiF.The Ka for HF is 3.5 × 10-4.

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

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Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 mol L^-1 C₆H₅COOH with 100.0 mL of 0.30 mol L^-1 C₆H₅COONa.The K_a for C₆H₅COOH is 6.5 × 10^-5.

What is the molar solubility of AgCl in 0.10 mol L^-1 NaCN if the colourless 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.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 2.1 × 10^-5 mol L^-1 in calcium ion and 4.75 × 10^-5mol L^-1 in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

The molar solubility of ZnS is 1.6 × 10^-12 mol L^-1 in pure water.Calculate the K_sp for ZnS.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-¹ HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

What is the pH of a solution made by mixing 25.00 mL of 0.100 mol L^-1 HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution before the addition of any HBr.

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is $4.50 \times 10 ^ { - 4 }$

The molar solubility of Ag₂S is 1.26 × 10^-16 mol L^-1 in pure water.Calculate the K_sp for Ag₂S.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution after the addition of 100.0 mL HBr.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH.Determine the pH of the solution after the addition of 200.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH)₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

Calculate the pH of a buffer that is 0.040 mol L^-1 HF and 0.020 mol L^-1 LiF.The K_a for HF is 3.5 × 10^-4.