What is the pH of the resulting solution if 45 mL of 0.432 mol L-1 methylamine, CH3NH2, is added to 15 mL of 0.234 mol L-1 HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+.

A) 2.77 B) 4.09 C) 9.91 D) 11.23 A) 2.77 B) 4.09 C) 9.91 D) 11.23

Determine the molar solubility of CaSO4 in a solution containing 0.100 mol L-1 Na2SO4. Ksp (CaSO4)= 2.4 × 10-5.

A) 4.9 × 10-3 mol L-1 B) 2.4 × 10-4 mol L-1 C) 5.8 × 10-10 mol L-1 D) 1.2 × 10-5 mol L-1 E) 0.10 mol L-1 A) 4.9 × 10-3 mol L-1 B) 2.4 × 10-4 mol L-1 C) 5.8 × 10-10 mol L-1 D) 1.2 × 10-5 mol L-1 E) 0.10 mol L-1

You wish to prepare a buffer containing CH3COOH with a pH of 4.24. If the pKa of acetic acid is 4.74, what ratio of CH3COO⁻/CH3COOH must you use?

A) 0.10 B) 0.50 C) 0.32 D) 2.0 E) 2.8 A) 0.10 B) 0.50 C) 0.32 D) 2.0 E) 2.8

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

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

Exam 16: Aqueous Ionic Equilibrium

A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite 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 nitrous acid is 1.36 × 10^-3.

(Multiple Choice)

4.7/5

(43)

Question 61

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 methylamine, CH₃NH₂, is added to 15 mL of 0.234 mol L^-1 HCl? Assume that the volumes of the solutions are additive. K_a = 2.70 × 10^-11for CH₃NH₃⁺.

(Multiple Choice)

4.8/5

(39)

Question 62

A 25.0 mL sample of 0.150 mol L^-1 hydrazoic acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH after 13.3 mL of base is added? The K_a of hydrazoic acid is 1.9 × 10^-5.

(Multiple Choice)

4.8/5

(35)

Question 63

Determine the molar solubility of CaSO₄ in a solution containing 0.100 mol L^-1 Na₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

(Multiple Choice)

4.8/5

(31)

Question 64

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 400.0 mL HBr.

(Multiple Choice)

4.9/5

(41)

Question 65

You wish to prepare a buffer containing CH₃COOH with a pH of 4.24. If the pK_a of acetic acid is 4.74, what ratio of CH₃COO⁻/CH₃COOH must you use?

(Multiple Choice)

4.9/5

(47)

Question 66

If the pK_a of HCOOH is 3.74 and the pH of an HCOOH/HCOONabuffer solution is 3.74, which of the following is TRUE?

(Multiple Choice)

4.8/5

(36)

Question 67

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

(Multiple Choice)

4.8/5

(28)

Question 68

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L^-1 HCl, followed by the addition of H₂S and 0.2 mol L^-1 HCl, and subsequently the addition of OH^- to a pH of 8.

(Multiple Choice)

4.9/5

(45)

Question 69

Which of the following solutions is a good buffer system?

(Multiple Choice)

4.7/5

(38)

Question 70

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)

4.7/5

(41)

Question 71

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)

4.8/5

(43)

Question 72

Which of the following acids (listed with pK_a values)and its conjugate base could form a buffer with a pH of 8.10?

(Multiple Choice)

5.0/5

(31)

Question 73

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L^-1 HClO with 100.0 mL of 0.20 mol L^-1 KClO. The K_a for HClO is 2.9 × 10^-8.

(Multiple Choice)

4.9/5

(37)

Question 74

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate after the addition of 6 mol L^-1 HCl; H₂S and 0.2 mol L^-1 HCl; OH^-to a pH of 8; and (NH₄)₂HPO₄ with NH₃.

(Multiple Choice)

4.9/5

(24)

Question 75

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 400.0 mL of KOH. The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

4.8/5

(31)

Question 76

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)

5.0/5

(42)

Question 77

Identify the expression for the solubility product constant for PbCl₂.

(Multiple Choice)

5.0/5

(37)

Question 78

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

(Multiple Choice)

4.8/5

(37)

Question 79

Identify the compound that is base-insoluble.

(Multiple Choice)

4.8/5

(31)

Question 80

Showing 61 - 80 of 161

Exam 16: Aqueous Ionic Equilibrium

What is the pH of the resulting solution if 45 mL of 0.432 mol L-1 methylamine, CH3NH2, is added to 15 mL of 0.234 mol L-1 HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+.

A 25.0 mL sample of 0.150 mol L-1 hydrazoic acid is titrated with a 0.150 mol L-1 NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hydrazoic acid is 1.9 × 10-5.

Determine the molar solubility of CaSO4 in a solution containing 0.100 mol L-1 Na2SO4. Ksp (CaSO4)= 2.4 × 10-5.

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 400.0 mL HBr.

You wish to prepare a buffer containing CH3COOH with a pH of 4.24. If the pKa of acetic acid is 4.74, what ratio of CH3COO⁻/CH3COOH must you use?

If the pKa of HCOOH is 3.74 and the pH of an HCOOH/HCOONa buffer solution is 3.74, which of the following is TRUE?

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

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L-1 HCl, followed by the addition of H2S and 0.2 mol L-1 HCl, and subsequently the addition of OH- to a pH of 8.

Which of the following solutions is a good buffer system?

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.

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.

Which of the following acids (listed with pKa values)and its conjugate base could form a buffer with a pH of 8.10?

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L-1 HClO with 100.0 mL of 0.20 mol L-1 KClO. The Ka for HClO is 2.9 × 10-8.

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 mol L-1 HCl; H2S and 0.2 mol L-1 HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3.

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 400.0 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.

Identify the expression for the solubility product constant for PbCl2.

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

Identify the compound that is base-insoluble.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

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 Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 methylamine, CH₃NH₂, is added to 15 mL of 0.234 mol L^-1 HCl? Assume that the volumes of the solutions are additive. K_a = 2.70 × 10^-11for CH₃NH₃⁺.

A 25.0 mL sample of 0.150 mol L^-1 hydrazoic acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH after 13.3 mL of base is added? The K_a of hydrazoic acid is 1.9 × 10^-5.

Determine the molar solubility of CaSO₄ in a solution containing 0.100 mol L^-1 Na₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

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 400.0 mL HBr.

You wish to prepare a buffer containing CH₃COOH with a pH of 4.24. If the pK_a of acetic acid is 4.74, what ratio of CH₃COO⁻/CH₃COOH must you use?

If the pK_a of HCOOH is 3.74 and the pH of an HCOOH/HCOONabuffer solution is 3.74, which of the following is TRUE?

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L^-1 HCl, followed by the addition of H₂S and 0.2 mol L^-1 HCl, and subsequently the addition of OH^- to a pH of 8.

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.

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.

Which of the following acids (listed with pK_a values)and its conjugate base could form a buffer with a pH of 8.10?

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L^-1 HClO with 100.0 mL of 0.20 mol L^-1 KClO. The K_a for HClO is 2.9 × 10^-8.

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate after the addition of 6 mol L^-1 HCl; H₂S and 0.2 mol L^-1 HCl; OH^-to a pH of 8; and (NH₄)₂HPO₄ with NH₃.

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 400.0 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.

Identify the expression for the solubility product constant for PbCl₂.

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