What is the pH of a buffer that results when 0.40 mol NaHCO2 is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (Ka of HCO2H = 1.8 × 10-4)

A) −0.301 B) 3.05 C) 3.44 D) 3.74 E) 4.05 A) −0.301 B) 3.05 C) 3.44 D) 3.74 E) 4.05

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH3 with 100.0 mL of 0.100 M HCl.(Kb for NH3 = 1.8 × 10-5)

A) 9.98 B) 4.02 C) 8.53 D) 9.26 E) none of these A) 9.98 B) 4.02 C) 8.53 D) 9.26 E) none of these

What is the pH of a buffer composed of 0.35 M H2PO4-(aq)and 0.65 M HPO42-(aq)? (Ka of H2PO4- is 6.2 × 10-8)

A) 6.94 B) 7.21 C) 7.48 D) 7.73 E) 9.06 A) 6.94 B) 7.21 C) 7.48 D) 7.73 E) 9.06

What mass of solid NaCH3CO2 (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH3CO2H to make a buffer with a pH of 7.21? (pKa of CH3CO2H = 7.21)

A) 0.0 g B) 1.9 g C) 41 g D) 71 g E) 1.6 × 102 g A) 0.0 g B) 1.9 g C) 41 g D) 71 g E) 1.6 × 102 g

What is the pH of an aqueous solution composed of 0.64 M NH4+ and 0.20 M NH3? (Ka of NH4+ = 5.6 × 10-10)

A) 4.80 B) 8.75 C) 9.20 D) 9.25 E) 9.76 A) 4.80 B) 8.75 C) 9.20 D) 9.25 E) 9.76

Exam 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Why do salts containing basic anions have a greater solubility in water than predicted from calculations using K_sp values? Examples of such salts are CaCO₃,PbF₂,and Ca₃(PO₄)₂.

(Essay)

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Question 21

Which of the following combinations would be best to buffer an aqueous solution at a pH of 9.24?

(Multiple Choice)

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Question 22

What is the solubility product expression for La(OH)₃?

(Multiple Choice)

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Question 23

An aqueous solution contains 0.010 M bromide ion (Br^-)and 0.010 M iodide ion (I^-).If silver ions (Ag⁺)are added to the solution until silver bromide just begins to precipitate,what are the concentrations of silver ions and iodide ions? (K_sp of AgBr = 5.4 × 10^-13 and K_sp of AgI = 8.5 × 10^-17)

(Multiple Choice)

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Question 24

The concentration of calcium carbonate in a saturated aqueous solution at 25°C is M.What is the K_sp of this sparingly soluble salt?

(Multiple Choice)

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Question 25

A 50.00-mL solution of 0.0400 M hydrofluoric acid (K_a = 7.2 × 10^-4)is titrated with a 0.0153 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (K_w = 1.00 × 10^-14)

(Multiple Choice)

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Question 26

What is the pH of a buffer that results when 0.40 mol NaHCO₂ is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (K_a of HCO₂H = 1.8 × 10^-4)

(Multiple Choice)

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Question 27

A 5.0 × 10^-4 M solution of MnSO₄ is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? The K_sp of Mn(OH)₂ is 2.0 × 10^-13 and K_w = 1.01 × 10^-14.

(Multiple Choice)

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Question 28

A certain weak base B has a base-ionization constant K_b of 5.9 × 10^-4 at 25°C.If strong acid is added to a solution of B,at what pH will [B] = [BH⁺]?

(Multiple Choice)

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Question 29

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH₃ with 100.0 mL of 0.100 M HCl.(K_b for NH₃ = 1.8 × 10^-5)

(Multiple Choice)

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Question 30

What is the pH of a buffer composed of 0.35 M H₂PO₄^-(aq)and 0.65 M HPO₄^2-(aq)? (K_a of H₂PO₄^- is 6.2 × 10^-8)

(Multiple Choice)

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Question 31

You have 75.0 mL of 0.17 M HA.After adding 30.0 mL of 0.10 M NaOH,the pH is 5.50.What is the K_a value of HA?

(Multiple Choice)

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Question 32

A volume of 25.0 mL of 0.100 M C₆H₅CO₂H(aq)is titrated with 0.100 M NaOH(aq).What is the pH after the addition of 12.5 mL of NaOH? (K_a of benzoic acid = 6.3 × 10^-5)

(Multiple Choice)

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Question 33

Potassium hydrogen phthalate (KHP)is used to standardize sodium hydroxide.If 35.39 mL of NaOH(aq)is required to titrate 0.8246 g KHP to the equivalence point,what is the concentration of the NaOH(aq)? (The molar mass of KHP = 204.2 g/mol) HC₈H₄O₄^-(aq)+ OH^-(aq) C₈H₄O₄^2-(aq)+ H₂O( )

(Multiple Choice)

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Question 34

A 1.0 liter solution contains 0.25 M hydrogen fluoride (HF)and 0.38 M sodium fluoride (NaF).What is the pH of this solution? (K_a for HF is 7.2 × 10^-4)

(Multiple Choice)

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Question 35

A 50.00-mL solution of 0.0350 M ethylamine (K_b = 5.6 × 10^-4)is titrated with a 0.0135 M solution of hydrochloric acid as the titrant.What is the pH at the equivalence point? (K_w = 1.0 × 10^-14)

(Multiple Choice)

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Question 36

What mass of solid NaCH₃CO₂ (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH₃CO₂H to make a buffer with a pH of 7.21? (pK_a of CH₃CO₂H = 7.21)

(Multiple Choice)

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Question 37

Hyperventilation can cause your blood pH to rise.One way to lower your blood pH is to breathe into a paper bag,thus recycling the air you exhale.Why does this procedure lower your blood pH?

(Essay)

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Question 38

What is the pH of an aqueous solution composed of 0.64 M NH₄⁺ and 0.20 M NH₃? (K_a of NH₄⁺ = 5.6 × 10^-10)

(Multiple Choice)

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Question 39

A 1.0-liter solution contains 0.25 M HF and 0.33 M NaF (K_a for HF is 7.2 × 10^-4). If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the change in pH?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 86

Exam 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Why do salts containing basic anions have a greater solubility in water than predicted from calculations using Ksp values? Examples of such salts are CaCO3,PbF2,and Ca3(PO4)2.

Which of the following combinations would be best to buffer an aqueous solution at a pH of 9.24?

What is the solubility product expression for La(OH)3?

An aqueous solution contains 0.010 M bromide ion (Br-)and 0.010 M iodide ion (I-).If silver ions (Ag+)are added to the solution until silver bromide just begins to precipitate,what are the concentrations of silver ions and iodide ions? (Ksp of AgBr = 5.4 × 10-13 and Ksp of AgI = 8.5 × 10-17)

The concentration of calcium carbonate in a saturated aqueous solution at 25°C is M.What is the Ksp of this sparingly soluble salt?

A 50.00-mL solution of 0.0400 M hydrofluoric acid (Ka = 7.2 × 10-4)is titrated with a 0.0153 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (Kw = 1.00 × 10-14)

What is the pH of a buffer that results when 0.40 mol NaHCO2 is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (Ka of HCO2H = 1.8 × 10-4)

A 5.0 × 10-4 M solution of MnSO4 is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? The Ksp of Mn(OH)2 is 2.0 × 10-13 and Kw = 1.01 × 10-14.

A certain weak base B has a base-ionization constant Kb of 5.9 × 10-4 at 25°C.If strong acid is added to a solution of B,at what pH will [B] = [BH+]?

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH3 with 100.0 mL of 0.100 M HCl.(Kb for NH3 = 1.8 × 10-5)

What is the pH of a buffer composed of 0.35 M H2PO4-(aq)and 0.65 M HPO42-(aq)? (Ka of H2PO4- is 6.2 × 10-8)

You have 75.0 mL of 0.17 M HA.After adding 30.0 mL of 0.10 M NaOH,the pH is 5.50.What is the Ka value of HA?

A volume of 25.0 mL of 0.100 M C6H5CO2H(aq)is titrated with 0.100 M NaOH(aq).What is the pH after the addition of 12.5 mL of NaOH? (Ka of benzoic acid = 6.3 × 10-5)

Potassium hydrogen phthalate (KHP)is used to standardize sodium hydroxide.If 35.39 mL of NaOH(aq)is required to titrate 0.8246 g KHP to the equivalence point,what is the concentration of the NaOH(aq)? (The molar mass of KHP = 204.2 g/mol) HC8H4O4-(aq)+ OH-(aq) C8H4O42-(aq)+ H2O( )

A 1.0 liter solution contains 0.25 M hydrogen fluoride (HF)and 0.38 M sodium fluoride (NaF).What is the pH of this solution? (Ka for HF is 7.2 × 10-4)

A 50.00-mL solution of 0.0350 M ethylamine (Kb = 5.6 × 10-4)is titrated with a 0.0135 M solution of hydrochloric acid as the titrant.What is the pH at the equivalence point? (Kw = 1.0 × 10-14)

What mass of solid NaCH3CO2 (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH3CO2H to make a buffer with a pH of 7.21? (pKa of CH3CO2H = 7.21)

Hyperventilation can cause your blood pH to rise.One way to lower your blood pH is to breathe into a paper bag,thus recycling the air you exhale.Why does this procedure lower your blood pH?

What is the pH of an aqueous solution composed of 0.64 M NH4+ and 0.20 M NH3? (Ka of NH4+ = 5.6 × 10-10)

A 1.0-liter solution contains 0.25 M HF and 0.33 M NaF (Ka for HF is 7.2 × 10-4). If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the change in pH?

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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Why do salts containing basic anions have a greater solubility in water than predicted from calculations using K_sp values? Examples of such salts are CaCO₃,PbF₂,and Ca₃(PO₄)₂.

What is the solubility product expression for La(OH)₃?

The concentration of calcium carbonate in a saturated aqueous solution at 25°C is M.What is the K_sp of this sparingly soluble salt?

A 50.00-mL solution of 0.0400 M hydrofluoric acid (K_a = 7.2 × 10^-4)is titrated with a 0.0153 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (K_w = 1.00 × 10^-14)

What is the pH of a buffer that results when 0.40 mol NaHCO₂ is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (K_a of HCO₂H = 1.8 × 10^-4)

A 5.0 × 10^-4 M solution of MnSO₄ is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? The K_sp of Mn(OH)₂ is 2.0 × 10^-13 and K_w = 1.01 × 10^-14.

A certain weak base B has a base-ionization constant K_b of 5.9 × 10^-4 at 25°C.If strong acid is added to a solution of B,at what pH will [B] = [BH⁺]?

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH₃ with 100.0 mL of 0.100 M HCl.(K_b for NH₃ = 1.8 × 10^-5)

What is the pH of a buffer composed of 0.35 M H₂PO₄^-(aq)and 0.65 M HPO₄^2-(aq)? (K_a of H₂PO₄^- is 6.2 × 10^-8)

You have 75.0 mL of 0.17 M HA.After adding 30.0 mL of 0.10 M NaOH,the pH is 5.50.What is the K_a value of HA?

A volume of 25.0 mL of 0.100 M C₆H₅CO₂H(aq)is titrated with 0.100 M NaOH(aq).What is the pH after the addition of 12.5 mL of NaOH? (K_a of benzoic acid = 6.3 × 10^-5)

Potassium hydrogen phthalate (KHP)is used to standardize sodium hydroxide.If 35.39 mL of NaOH(aq)is required to titrate 0.8246 g KHP to the equivalence point,what is the concentration of the NaOH(aq)? (The molar mass of KHP = 204.2 g/mol) HC₈H₄O₄^-(aq)+ OH^-(aq) C₈H₄O₄^2-(aq)+ H₂O( )

A 1.0 liter solution contains 0.25 M hydrogen fluoride (HF)and 0.38 M sodium fluoride (NaF).What is the pH of this solution? (K_a for HF is 7.2 × 10^-4)

A 50.00-mL solution of 0.0350 M ethylamine (K_b = 5.6 × 10^-4)is titrated with a 0.0135 M solution of hydrochloric acid as the titrant.What is the pH at the equivalence point? (K_w = 1.0 × 10^-14)

What mass of solid NaCH₃CO₂ (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH₃CO₂H to make a buffer with a pH of 7.21? (pK_a of CH₃CO₂H = 7.21)

What is the pH of an aqueous solution composed of 0.64 M NH₄⁺ and 0.20 M NH₃? (K_a of NH₄⁺ = 5.6 × 10^-10)

A 1.0-liter solution contains 0.25 M HF and 0.33 M NaF (K_a for HF is 7.2 × 10^-4). If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the change in pH?