Calculate the molar concentration of uncomplexed Zn2+(aq) in a solution that contains 0.17 M Zn(NH3)42+ and 0.3775 M NH3 at equilibrium. Kf for Zn(NH3)42+ is $2.9 \times 10 ^ { 9 }$ .

A) $2.9 \times 10 ^ { - 9 }$ M B) $1.6 \times 10 ^ { - 10 }$ M C) $3.5 \times 10 ^ { 8 }$ M D) $4.1 \times 10 ^ { - 10 }$ M E) $2.7 \times 10 ^ { 0 }$ M A) $2.9 \times 10 ^ { - 9 }$ M B) $1.6 \times 10 ^ { - 10 }$ M C) $3.5 \times 10 ^ { 8 }$ M D) $4.1 \times 10 ^ { - 10 }$ M E) $2.7 \times 10 ^ { 0 }$ M

What is the pH of the buffer that results when 12.0 g of NaH2PO4 and 8.00 g of Na2HPO4 are diluted with water to a volume of 0.50 L? (Ka of H2PO4- = 6.2 × 10-8, the molar masses of NaH2PO4 and Na2HPO4 are 120.0 g/mol and 142.0 mol, respectively)

A) 4.10 B) 6.96 C) 7.21 D) 7.46 E) 9.90 A) 4.10 B) 6.96 C) 7.21 D) 7.46 E) 9.90

What is the molar solubility of Mn(OH)2(s) in a solution that is buffered at pH 8.00 at 25 °C? The Ksp of Mn(OH)2 is 1.9 × 10-13 at 25 °C.

A) 3.6 × 10-8 mol/L B) 1.9 × 10-7 mol/L C) 3.6 × 10-5 mol/L D) 1.9 × 10-1 mol/L E) 1.9 × 103 mol/L A) 3.6 × 10-8 mol/L B) 1.9 × 10-7 mol/L C) 3.6 × 10-5 mol/L D) 1.9 × 10-1 mol/L E) 1.9 × 103 mol/L

If 25 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC2H3O2, what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 × 10-5 at 25°C.

A) 10.1 B) 4.2 C) 5.1 D) 2.7 E) 4.4 A) 10.1 B) 4.2 C) 5.1 D) 2.7 E) 4.4

What is the concentration of Cd2+(aq) in a mixture of 0.014 mol Cd(NO3)2 and 1.0 mol NH3 diluted to 1.00 L? For Cd(NH3)42+, Kf = 1.0 × 107.

A) 3.7 × 10-5 M B) 1.5 × 10-9 M C) 1.8 × 10-9 M D) 3.2 × 10-4 M E) 1.4 × 10-2 M A) 3.7 × 10-5 M B) 1.5 × 10-9 M C) 1.8 × 10-9 M D) 3.2 × 10-4 M E) 1.4 × 10-2 M

The concentration of Pb2+ in an aqueous solution is 5.5 × 10-3 M. What concentration of SO42- is required to begin precipitating PbSO4? The Ksp of PbSO4 is 2.5 × 10-8.

A) 1.4 × 10-10 M B) 4.5 × 10-6 M C) 1.6 × 10-4 M D) 8.3 × 10-4 M E) 2.9 × 10-2 M A) 1.4 × 10-10 M B) 4.5 × 10-6 M C) 1.6 × 10-4 M D) 8.3 × 10-4 M E) 2.9 × 10-2 M

The Ksp of BaSO4 is 1.1 × 10-10 at 25 °C. What mass of BaSO4 will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

A) 2.6 × 10−8 g B) 4.5 × 10−8 g C) 1.0 × 10−5 g D) 1.6 × 10−4 g E) 2.4 × 10−3 g A) 2.6 × 10−8 g B) 4.5 × 10−8 g C) 1.0 × 10−5 g D) 1.6 × 10−4 g E) 2.4 × 10−3 g

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

The solubility of strontium carbonate (SrCO3) in water at 25°C is $4.5 \times 10 ^ { - 3 }$ g/L. What is the Ksp of this sparingly soluble salt?

A) $9.3 \times 10 ^ { - 10 }$ B) $1.13 \times 10 ^ { - 13 }$ C) $2.34 \times 10 ^ { - 17 }$ D) $5.52 \times 10 ^ { - 3 }$ E) $3.12 \times 10 ^ { - 2 }$ A) $9.3 \times 10 ^ { - 10 }$ B) $1.13 \times 10 ^ { - 13 }$ C) $2.34 \times 10 ^ { - 17 }$ D) $5.52 \times 10 ^ { - 3 }$ E) $3.12 \times 10 ^ { - 2 }$

Exam 18: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Calculate the molar concentration of uncomplexed Zn²⁺(aq) in a solution that contains 0.17 M Zn(NH₃)₄²⁺ and 0.3775 M NH₃ at equilibrium. K_f for Zn(NH₃)₄²⁺ is $2.9 \times 10 ^ { 9 }$ .

(Multiple Choice)

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Question 61

What is the pH of the buffer that results when 12.0 g of NaH₂PO₄ and 8.00 g of Na₂HPO₄ are diluted with water to a volume of 0.50 L? (K_a of H₂PO₄^- = 6.2 × 10^-8, the molar masses of NaH₂PO₄ and Na₂HPO₄ are 120.0 g/mol and 142.0 mol, respectively)

(Multiple Choice)

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Question 62

What mass of sodium hydroxide must be added to 65.0 mL of 0.926 M acetic acid in order to create a buffer with a pH of 4.83? K_a for acetic acid is 1.8 × 10^-5.

(Multiple Choice)

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Question 63

The K_sp of Ca(OH)₂ is 5.5 × 10^-5 at 25 °C. What is the concentration of OH^-(aq) in a saturated solution of Ca(OH)₂(aq)?

(Multiple Choice)

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Question 64

What is the molar solubility of Mn(OH)₂(s) in a solution that is buffered at pH 8.00 at 25 °C? The K_sp of Mn(OH)₂ is 1.9 × 10^-13 at 25 °C.

(Multiple Choice)

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Question 65

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 66

If 25 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC₂H₃O₂, what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5 at 25°C.

(Multiple Choice)

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Question 67

Which of the following is the common name for iron(II) carbonate?

(Multiple Choice)

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Question 68

All of the following statements concerning acid-base buffers are true EXCEPT

(Multiple Choice)

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Question 69

What is the concentration of Cd²⁺(aq) in a mixture of 0.014 mol Cd(NO₃)₂ and 1.0 mol NH₃ diluted to 1.00 L? For Cd(NH₃)₄²⁺, K_f = 1.0 × 10⁷.

(Multiple Choice)

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Question 70

When a weak base is titrated with a strong acid, the pH at the equivalence point is _____.

(Multiple Choice)

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Question 71

The concentration of Pb²⁺ in an aqueous solution is 5.5 × 10^-3 M. What concentration of SO₄^2- is required to begin precipitating PbSO₄? The K_sp of PbSO₄ is 2.5 × 10^-8.

(Multiple Choice)

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Question 72

How many moles of solid NaF would have to be added to 1.0 L of 2.16 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change. (K_a for HF = 7.2 × 10^-4)

(Multiple Choice)

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Question 73

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 74

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 75

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25 °C. What mass of BaSO₄ will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

(Multiple Choice)

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Question 76

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 77

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 78

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 79

The solubility of strontium carbonate (SrCO₃) in water at 25°C is $4.5 \times 10 ^ { - 3 }$ g/L. What is the K_sp of this sparingly soluble salt?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 87

Exam 18: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Calculate the molar concentration of uncomplexed Zn2+(aq) in a solution that contains 0.17 M Zn(NH3)42+ and 0.3775 M NH3 at equilibrium. Kf for Zn(NH3)42+ is 2.9×1092.9 \times 10 ^ { 9 }2.9×109 .

What is the pH of the buffer that results when 12.0 g of NaH2PO4 and 8.00 g of Na2HPO4 are diluted with water to a volume of 0.50 L? (Ka of H2PO4- = 6.2 × 10-8, the molar masses of NaH2PO4 and Na2HPO4 are 120.0 g/mol and 142.0 mol, respectively)

What mass of sodium hydroxide must be added to 65.0 mL of 0.926 M acetic acid in order to create a buffer with a pH of 4.83? Ka for acetic acid is 1.8 × 10-5.

The Ksp of Ca(OH)2 is 5.5 × 10-5 at 25 °C. What is the concentration of OH-(aq) in a saturated solution of Ca(OH)2(aq)?

What is the molar solubility of Mn(OH)2(s) in a solution that is buffered at pH 8.00 at 25 °C? The Ksp of Mn(OH)2 is 1.9 × 10-13 at 25 °C.

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?

If 25 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC2H3O2, what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 × 10-5 at 25°C.

Which of the following is the common name for iron(II) carbonate?

All of the following statements concerning acid-base buffers are true EXCEPT

What is the concentration of Cd2+(aq) in a mixture of 0.014 mol Cd(NO3)2 and 1.0 mol NH3 diluted to 1.00 L? For Cd(NH3)42+, Kf = 1.0 × 107.​

When a weak base is titrated with a strong acid, the pH at the equivalence point is _____.

The concentration of Pb2+ in an aqueous solution is 5.5 × 10-3 M. What concentration of SO42- is required to begin precipitating PbSO4? The Ksp of PbSO4 is 2.5 × 10-8.

How many moles of solid NaF would have to be added to 1.0 L of 2.16 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change. (Ka for HF = 7.2 × 10-4)

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.

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 Ksp of BaSO4 is 1.1 × 10-10 at 25 °C. What mass of BaSO4 will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

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 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)

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)

The solubility of strontium carbonate (SrCO3) in water at 25°C is 4.5×10−34.5 \times 10 ^ { - 3 }4.5×10−3 g/L. What is the Ksp of this sparingly soluble salt?

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

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Calculate the molar concentration of uncomplexed Zn²⁺(aq) in a solution that contains 0.17 M Zn(NH₃)₄²⁺ and 0.3775 M NH₃ at equilibrium. K_f for Zn(NH₃)₄²⁺ is $2.9 \times 10 ^ { 9 }$ .

What is the pH of the buffer that results when 12.0 g of NaH₂PO₄ and 8.00 g of Na₂HPO₄ are diluted with water to a volume of 0.50 L? (K_a of H₂PO₄^- = 6.2 × 10^-8, the molar masses of NaH₂PO₄ and Na₂HPO₄ are 120.0 g/mol and 142.0 mol, respectively)

What mass of sodium hydroxide must be added to 65.0 mL of 0.926 M acetic acid in order to create a buffer with a pH of 4.83? K_a for acetic acid is 1.8 × 10^-5.

The K_sp of Ca(OH)₂ is 5.5 × 10^-5 at 25 °C. What is the concentration of OH^-(aq) in a saturated solution of Ca(OH)₂(aq)?

What is the molar solubility of Mn(OH)₂(s) in a solution that is buffered at pH 8.00 at 25 °C? The K_sp of Mn(OH)₂ is 1.9 × 10^-13 at 25 °C.

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?

If 25 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC₂H₃O₂, what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5 at 25°C.

What is the concentration of Cd²⁺(aq) in a mixture of 0.014 mol Cd(NO₃)₂ and 1.0 mol NH₃ diluted to 1.00 L? For Cd(NH₃)₄²⁺, K_f = 1.0 × 10⁷.

The concentration of Pb²⁺ in an aqueous solution is 5.5 × 10^-3 M. What concentration of SO₄^2- is required to begin precipitating PbSO₄? The K_sp of PbSO₄ is 2.5 × 10^-8.

How many moles of solid NaF would have to be added to 1.0 L of 2.16 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change. (K_a for HF = 7.2 × 10^-4)

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.

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25 °C. What mass of BaSO₄ will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

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 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)

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)

The solubility of strontium carbonate (SrCO₃) in water at 25°C is $4.5 \times 10 ^ { - 3 }$ g/L. What is the K_sp of this sparingly soluble salt?