Which of the following can act as buffer solutions? I.0.1 M HC2H3O2/0.1 M NaC2H3O2 II.0.1 M NH3/0.1 M NH4Cl III.0.1 M HNO3/0.1 M NaNO3 IV.0.1 M H2SO3/0.1 M NaHSO3 V.0.1 M KHSO4/ 0.1 M H2SO4

A) I,II,and III B) II,IIIand IV C) IIIand IV D) I,IIand IV E) III,IVand V A) I,II,and III B) II,IIIand IV C) IIIand IV D) I,IIand IV E) III,IVand V

What will the pH at the neutralization point of 0.00812 M Ba(OH)2(aq)be when titrated with HCl(aq)?

A) 7.0 B) 12.2 C) 8.0 D) 9.0 E) 6.0 A) 7.0 B) 12.2 C) 8.0 D) 9.0 E) 6.0

If 30.0 mmol HCl(g)is added to 1.00 L of a buffer that is 0.340 M NH3(aq)and 0.290 M NH4Cl(aq),what are the final concentrations of NH3(aq)and NH4Cl(aq),respectively? Assume no volume change.

A) 0.310 M and 0.320 M B) 0.310 M and 0.290 M C) 0.370 M and 0.290 M D) 0.370 M and 0.320 M A) 0.310 M and 0.320 M B) 0.310 M and 0.290 M C) 0.370 M and 0.290 M D) 0.370 M and 0.320 M

For HClO2,Ka = 1.2 × 10-2.What is the pH of an aqueous solution in which [NaClO2] = 0.193 M and [HClO2] = 0.203 M?

A) 3.32 B) 0.11 C) 1.92 D) 1.94 E) 1.90 A) 3.32 B) 0.11 C) 1.92 D) 1.94 E) 1.90

Exam 17: Additional Aspects of Acidbase Equilibria

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: HCl(aq)is titrated with NH₃(aq)

(Multiple Choice)

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Question 61

What is the pH of a buffer that is 0.88 M HCN(aq)and 0.53 M NaCN(aq)? The K_a of HCN is 6.2 × 10^-10.

(Multiple Choice)

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Question 62

Formic acid (HCOOH,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 aqueous formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH(aq)to reach the equivalence point?

(Multiple Choice)

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Question 63

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: KOH(aq)is titrated with HI(aq)

(Multiple Choice)

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Question 64

How will addition of sodium acetate to an aqueous acetic acid solution affect the pH?

(Multiple Choice)

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Question 65

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,K_a for HF is 6.6 × 10^-4

(Multiple Choice)

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Question 66

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which K_b(NH₃)is 1.8 × 10^-5,as:

(Multiple Choice)

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Question 67

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is

(Multiple Choice)

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Question 68

Acid-base indicators have two forms: an acid of one color and a base of another color.

(True/False)

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Question 69

An aqueous 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 Of nitrous acid is 1.36 × 10^-3.

(Multiple Choice)

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Question 70

The buffer capacity of a solution may be defined as the number of moles of H⁺ that will change the pH of 1.00 L of the buffer by 1.00 pH units.What is the buffer capacity of an aqueous solution which is 0.10 M in acetic acid (K_a = 1.8 × 10^-5)and 0.30 M in sodium acetate,in units of mol (H⁺)per liter?

(Multiple Choice)

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Question 71

Twenty-five milliliters of 0.10 M HCl(aq)is titrated with 0.10 M NaOH(aq).What is the pH before any NaOH(aq)is added?

(Multiple Choice)

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Question 72

Which of the following can act as buffer solutions? I.0.1 M HC₂H₃O₂/0.1 M NaC₂H₃O₂ II.0.1 M NH₃/0.1 M NH₄Cl III.0.1 M HNO₃/0.1 M NaNO₃ IV.0.1 M H₂SO₃/0.1 M NaHSO₃ V.0.1 M KHSO₄/ 0.1 M H₂SO₄

(Multiple Choice)

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Question 73

What will the pH at the neutralization point of 0.00812 M Ba(OH)₂(aq)be when titrated with HCl(aq)?

(Multiple Choice)

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Question 74

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (K_b = 1.8 × 10^-5).To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

(Multiple Choice)

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Question 75

An aqueous solution containing equimolar amounts of a weak acid with K_a = 10^-5 and its sodium salt has:

(Multiple Choice)

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Question 76

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq).What is the pH after 30 mL of NaOH have been added? K_a for acetic acid = 1.8 × 10^-5.

(Multiple Choice)

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Question 77

If 30.0 mmol HCl(g)is added to 1.00 L of a buffer that is 0.340 M NH₃(aq)and 0.290 M NH₄Cl(aq),what are the final concentrations of NH₃(aq)and NH₄Cl(aq),respectively? Assume no volume change.

(Multiple Choice)

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Question 78

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

(Multiple Choice)

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Question 79

For HClO₂,K_a = 1.2 × 10^-2.What is the pH of an aqueous solution in which [NaClO₂] = 0.193 M and [HClO₂] = 0.203 M?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 130

Exam 17: Additional Aspects of Acidbase Equilibria

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: HCl(aq)is titrated with NH3(aq)

What is the pH of a buffer that is 0.88 M HCN(aq)and 0.53 M NaCN(aq)? The Ka of HCN is 6.2 × 10-10.

Formic acid (HCOOH,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 aqueous formic acid solution requires 29.80 mL of 0.0567 mol L-1 NaOH(aq)to reach the equivalence point?

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: KOH(aq)is titrated with HI(aq)

How will addition of sodium acetate to an aqueous acetic acid solution affect the pH?

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,Ka for HF is 6.6 × 10-4

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which Kb(NH3)is 1.8 × 10-5,as:

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L-1 in nitrous acid And 0.112 mol L-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is

Acid-base indicators have two forms: an acid of one color and a base of another color.

Twenty-five milliliters of 0.10 M HCl(aq)is titrated with 0.10 M NaOH(aq).What is the pH before any NaOH(aq)is added?

Which of the following can act as buffer solutions? I.0.1 M HC2H3O2/0.1 M NaC2H3O2 II.0.1 M NH3/0.1 M NH4Cl III.0.1 M HNO3/0.1 M NaNO3 IV.0.1 M H2SO3/0.1 M NaHSO3 V.0.1 M KHSO4/ 0.1 M H2SO4

What will the pH at the neutralization point of 0.00812 M Ba(OH)2(aq)be when titrated with HCl(aq)?

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (Kb = 1.8 × 10-5).To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

An aqueous solution containing equimolar amounts of a weak acid with Ka = 10-5 and its sodium salt has:

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq).What is the pH after 30 mL of NaOH have been added? Ka for acetic acid = 1.8 × 10-5.

If 30.0 mmol HCl(g)is added to 1.00 L of a buffer that is 0.340 M NH3(aq)and 0.290 M NH4Cl(aq),what are the final concentrations of NH3(aq)and NH4Cl(aq),respectively? Assume no volume change.

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 HCN with 50.00 mL of 0.010 mol L-1 NaCN? Assume that the volumes of the solutions are additive and that Ka =

For HClO2,Ka = 1.2 × 10-2.What is the pH of an aqueous solution in which [NaClO2] = 0.193 M and [HClO2] = 0.203 M?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: HCl(aq)is titrated with NH₃(aq)

What is the pH of a buffer that is 0.88 M HCN(aq)and 0.53 M NaCN(aq)? The K_a of HCN is 6.2 × 10^-10.

Formic acid (HCOOH,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 aqueous formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH(aq)to reach the equivalence point?

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,K_a for HF is 6.6 × 10^-4

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which K_b(NH₃)is 1.8 × 10^-5,as:

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is

Which of the following can act as buffer solutions? I.0.1 M HC₂H₃O₂/0.1 M NaC₂H₃O₂ II.0.1 M NH₃/0.1 M NH₄Cl III.0.1 M HNO₃/0.1 M NaNO₃ IV.0.1 M H₂SO₃/0.1 M NaHSO₃ V.0.1 M KHSO₄/ 0.1 M H₂SO₄

What will the pH at the neutralization point of 0.00812 M Ba(OH)₂(aq)be when titrated with HCl(aq)?

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (K_b = 1.8 × 10^-5).To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

An aqueous solution containing equimolar amounts of a weak acid with K_a = 10^-5 and its sodium salt has:

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq).What is the pH after 30 mL of NaOH have been added? K_a for acetic acid = 1.8 × 10^-5.

If 30.0 mmol HCl(g)is added to 1.00 L of a buffer that is 0.340 M NH₃(aq)and 0.290 M NH₄Cl(aq),what are the final concentrations of NH₃(aq)and NH₄Cl(aq),respectively? Assume no volume change.

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

For HClO₂,K_a = 1.2 × 10^-2.What is the pH of an aqueous solution in which [NaClO₂] = 0.193 M and [HClO₂] = 0.203 M?