Consider a solution consisting of the following two buffer systems: H2CO3 HCO3- + H+ pKa = 6.4 H2PO4- HPO42- + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

A) [H2CO3] > [HCO3-] and [H2PO4-] > [HPO42-] B) [HCO3-] > [H2CO3] and [HPO42-] > [H2PO4-] C) [H2CO3] > [HCO3-] and [HPO42-] > [H2PO4-] D) [H2CO3] = [HCO3-] and [HPO42-] > [H2PO4-] E) [H2CO3] = [HCO3-] and [H2PO4-] > [HPO42-] A) [H2CO3] > [HCO3-] and [H2PO4-] > [HPO42-] B) [HCO3-] > [H2CO3] and [HPO42-] > [H2PO4-] C) [H2CO3] > [HCO3-] and [HPO42-] > [H2PO4-] D) [H2CO3] = [HCO3-] and [HPO42-] > [H2PO4-] E) [H2CO3] = [HCO3-] and [H2PO4-] > [HPO42-]

Calculate the molar concentration of uncomplexed Zn2+ in a solution that contains 0.20 mol of Zn(NH3)42+ per liter. The overall Kf for Zn(NH3)42+ is 3.8 × 109.

A) 6.7 × 10-4 M B) 2.9 × 10-3 M C) 2.0 × 10-13 M D) 8.8 × 10-3 M E) none of these A) 6.7 × 10-4 M B) 2.9 × 10-3 M C) 2.0 × 10-13 M D) 8.8 × 10-3 M E) none of these

How many moles of Fe(OH)2 [Ksp = 1.8 × 10-15] will dissolve in 1 L of water buffered at pH = 12.00?

A) 1.8 × 10-11 mol B) 1.8 × 10-9 mol C) 5.0 × 10-12 mol D) 8.0 × 10-6 mol E) 4.0 × 10-8 mol A) 1.8 × 10-11 mol B) 1.8 × 10-9 mol C) 5.0 × 10-12 mol D) 8.0 × 10-6 mol E) 4.0 × 10-8 mol

The concentration of Al3+ in a saturated solution of Al(OH)3 at 25°C is 5.2 × 10-9 M. Calculate the Ksp for Al(OH)3.

A) 7.3 × 10-34 B) 2.9 × 10-33 C) 2.0 × 10-32 D) 5.6 × 10-25 E) none of these A) 7.3 × 10-34 B) 2.9 × 10-33 C) 2.0 × 10-32 D) 5.6 × 10-25 E) none of these

Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: The concentration of Ag+ at equilibrium is

A) 2.0 M. B) 4.5 × 10-9 M. C) 1.2 × 10-8 M. D) 1.6 M. E) none of these A) 2.0 M. B) 4.5 × 10-9 M. C) 1.2 × 10-8 M. D) 1.6 M. E) none of these

A titration of 100.0 mL of 1.00 M malonic acid (HS1U1B12S1U1B0A) was done with 1.00 M NaOH. For malonic acid, KS1U1B1a1S1U1B0 = 1.49 × 10S1U1P1-2S1S1P0, KS1U1B1a2S1U1B0 = 2.03 × 10S1U1P1-6S1S1P0. -Calculate [H+] after 150.0 mL of 1.00 M NaOH has been added.

A) 2.03 × 10-6 M B) 1.41 × 10-10 M C) 1.49 × 10-2 M D) 1.00 × 10-7 M E) none of these A) 2.03 × 10-6 M B) 1.41 × 10-10 M C) 1.49 × 10-2 M D) 1.00 × 10-7 M E) none of these

In a solution prepared by adding excess PbI2(s) [Ksp = 1.4 × 10-8] to water, [I-] at equilibrium is

A) 2.4 × 10-3 mol/L. B) 1.5 × 10-3 mol/L. C) 8.4 × 10-5 mol/L. D) 3.0 × 10-3 mol/L. E) 1.2 × 10-3 mol/L. A) 2.4 × 10-3 mol/L. B) 1.5 × 10-3 mol/L. C) 8.4 × 10-5 mol/L. D) 3.0 × 10-3 mol/L. E) 1.2 × 10-3 mol/L.

A 100.0-mL sample of 0.2 M (CH3)3N (Kb = 5.3 × 10-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

A) 5.4 B) 7.0 C) 10.3 D) 3.1 E) 9.9 A) 5.4 B) 7.0 C) 10.3 D) 3.1 E) 9.9

What is the solubility of Mg(OH)2 (Ksp = 8.9 × 10-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

A) 8.9 × 10-1 mol B) 8.9 × 10-4 mol C) 8.9 × 109 mol D) 8.9 × 10-7 mol E) none of these A) 8.9 × 10-1 mol B) 8.9 × 10-4 mol C) 8.9 × 109 mol D) 8.9 × 10-7 mol E) none of these

Chromate ion is added to a saturated solution of Ag2CrO4 to reach 0.10 M CrO42-. Calculate the final concentration of silver ion at equilibrium (Ksp for Ag2CrO4 is 9.0 × 10-12).

A) 9.5 × 10-6 M B) 1.7 × 10-6 M C) 5.5 × 10-11 M D) 6.6 × 10-6 M E) 1.1 × 10-13 M A) 9.5 × 10-6 M B) 1.7 × 10-6 M C) 5.5 × 10-11 M D) 6.6 × 10-6 M E) 1.1 × 10-13 M

Exam 8: Applications of Aqueous Equilibria

Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + H⁺ pK_a = 6.4 H₂PO₄^- HPO₄^2- + H⁺ pK_a = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

(Multiple Choice)

5.0/5

(36)

Question 41

Calculate the molar concentration of uncomplexed Zn²⁺ in a solution that contains 0.20 mol of Zn(NH₃)₄²⁺ per liter. The overall K_f for Zn(NH₃)₄²⁺ is 3.8 × 10⁹.

(Multiple Choice)

5.0/5

(33)

Question 42

How many moles of Fe(OH)₂ [K_sp = 1.8 × 10^-15] will dissolve in 1 L of water buffered at pH = 12.00?

(Multiple Choice)

4.8/5

(31)

Question 43

The concentration of Al³⁺ in a saturated solution of Al(OH)₃ at 25°C is 5.2 × 10^-9 M. Calculate the K_sp for Al(OH)₃.

(Multiple Choice)

4.8/5

(34)

Question 44

What is the pH of this solution?

(Multiple Choice)

4.9/5

(23)

Question 45

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, K_a = 6.2 × 10^-10.50.0 mL of 0.10 M HNO₃ 60.0 mL of 0.20 M Ba(OH)₂ 95.0 mL of 0.20 M HClO₄195.0 mL of 1.0 × 10^-4 M HCN

(Short Answer)

4.8/5

(30)

Question 46

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 220.0 mL of 0.200 M NaOH is added

(Multiple Choice)

4.8/5

(38)

Question 47

Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2 × 10^-10), 1.00 M NaOH and 1.50 M NaCN.

(Multiple Choice)

4.8/5

(36)

Question 48

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃^2-: The concentration of Cu⁺ at equilibrium is

(Multiple Choice)

4.8/5

(36)

Question 49

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃. Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: The concentration of Ag⁺ at equilibrium is

(Multiple Choice)

4.9/5

(49)

Question 50

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49 × 10^-2, K_a2 = 2.03 × 10^-6. -Calculate [H⁺] after 150.0 mL of 1.00 M NaOH has been added.

(Multiple Choice)

4.9/5

(39)

Question 51

In a solution prepared by adding excess PbI₂(s) [K_sp = 1.4 × 10^-8] to water, [I^-] at equilibrium is

(Multiple Choice)

4.9/5

(31)

Question 52

A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3 × 10^-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

(Multiple Choice)

4.7/5

(42)

Question 53

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of K_a for the acid HA.

(Multiple Choice)

4.9/5

(29)

Question 54

What is the solubility of Mg(OH)₂ (K_sp = 8.9 × 10^-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

(Multiple Choice)

4.8/5

(29)

Question 55

Calculate the pH of a solution made by mixing 46.0 mL of 0.350 M NaA (K_a for HA = 1.0 × 10^-9) with 26.0 mL of 0.190 M HCl.

(Multiple Choice)

4.8/5

(37)

Question 56

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃^2-: What is the concentration of CN^- at equilibrium?

(Multiple Choice)

4.8/5

(27)

Question 57

Chromate ion is added to a saturated solution of Ag₂CrO₄ to reach 0.10 M CrO₄^2-. Calculate the final concentration of silver ion at equilibrium (K_sp for Ag₂CrO₄ is 9.0 × 10^-12).

(Multiple Choice)

4.8/5

(41)

Question 58

A student uses 16.60 mL of 0.100 M NaOH to titrate a 0.2000-g sample of an unknown acid. Which of the following acids is the unknown most likely to be? Assume that only the hydrogens bonded to oxygen are titrated by the sodium hydroxide and that, because of experimental error, the student's value may not be identical to the theoretical value.

(Multiple Choice)

4.9/5

(43)

Question 59

The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: Consider an experiment in which 1.0 × 10^-3 mol of M(NO₃)₂ is added to 1.0 L of 15.0 M NH₃. Calculate the equilibrium concentrations of M²⁺, M(NH₃)₂²⁺, and M(NH₃)₃²⁺

(Essay)

4.9/5

(39)

Question 60

Showing 41 - 60 of 177

Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + H⁺ pK_a = 6.4 H₂PO₄^- HPO₄^2- + H⁺ pK_a = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

Calculate the molar concentration of uncomplexed Zn²⁺ in a solution that contains 0.20 mol of Zn(NH₃)₄²⁺ per liter. The overall K_f for Zn(NH₃)₄²⁺ is 3.8 × 10⁹.

How many moles of Fe(OH)₂ [K_sp = 1.8 × 10^-15] will dissolve in 1 L of water buffered at pH = 12.00?

The concentration of Al³⁺ in a saturated solution of Al(OH)₃ at 25°C is 5.2 × 10^-9 M. Calculate the K_sp for Al(OH)₃.

What is the pH of this solution?

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, K_a = 6.2 × 10^-10.50.0 mL of 0.10 M HNO₃ 60.0 mL of 0.20 M Ba(OH)₂ 95.0 mL of 0.20 M HClO₄195.0 mL of 1.0 × 10^-4 M HCN

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 220.0 mL of 0.200 M NaOH is added

Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2 × 10^-10), 1.00 M NaOH and 1.50 M NaCN.

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃^2-: The concentration of Cu⁺ at equilibrium is

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃. Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: The concentration of Ag⁺ at equilibrium is

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49 × 10^-2, K_a2 = 2.03 × 10^-6. -Calculate [H⁺] after 150.0 mL of 1.00 M NaOH has been added.

In a solution prepared by adding excess PbI₂(s) [K_sp = 1.4 × 10^-8] to water, [I^-] at equilibrium is

A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3 × 10^-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of K_a for the acid HA.

What is the solubility of Mg(OH)₂ (K_sp = 8.9 × 10^-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Calculate the pH of a solution made by mixing 46.0 mL of 0.350 M NaA (K_a for HA = 1.0 × 10^-9) with 26.0 mL of 0.190 M HCl.

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃^2-: What is the concentration of CN^- at equilibrium?

Chromate ion is added to a saturated solution of Ag₂CrO₄ to reach 0.10 M CrO₄^2-. Calculate the final concentration of silver ion at equilibrium (K_sp for Ag₂CrO₄ is 9.0 × 10^-12).

The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: Consider an experiment in which 1.0 × 10^-3 mol of M(NO₃)₂ is added to 1.0 L of 15.0 M NH₃. Calculate the equilibrium concentrations of M²⁺, M(NH₃)₂²⁺, and M(NH₃)₃²⁺

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Exam 8: Applications of Aqueous Equilibria

Consider a solution consisting of the following two buffer systems: H2CO3 HCO3- + H+ pKa = 6.4 H2PO4- HPO42- + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

Calculate the molar concentration of uncomplexed Zn2+ in a solution that contains 0.20 mol of Zn(NH3)42+ per liter. The overall Kf for Zn(NH3)42+ is 3.8 × 109.

How many moles of Fe(OH)2 [Ksp = 1.8 × 10-15] will dissolve in 1 L of water buffered at pH = 12.00?

The concentration of Al3+ in a saturated solution of Al(OH)3 at 25°C is 5.2 × 10-9 M. Calculate the Ksp for Al(OH)3.

What is the pH of this solution?

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, Ka = 6.2 × 10-10.50.0 mL of 0.10 M HNO3 60.0 mL of 0.20 M Ba(OH)2 95.0 mL of 0.20 M HClO4 195.0 mL of 1.0 × 10-4 M HCN

A 200.0-mL sample of the weak acid H3A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 220.0 mL of 0.200 M NaOH is added

Calculate the pH of a solution that contains 3.25 M HCN (Ka = 6.2 × 10-10), 1.00 M NaOH and 1.50 M NaCN.

A 50.0-mL sample of 2.0 × 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN)32-: The concentration of Cu+ at equilibrium is

Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: The concentration of Ag+ at equilibrium is

A titration of 100.0 mL of 1.00 M malonic acid (H2A) was done with 1.00 M NaOH. For malonic acid, Ka1 = 1.49 × 10-2, Ka2 = 2.03 × 10-6. -Calculate [H+] after 150.0 mL of 1.00 M NaOH has been added.

In a solution prepared by adding excess PbI2(s) [Ksp = 1.4 × 10-8] to water, [I-] at equilibrium is

A 100.0-mL sample of 0.2 M (CH3)3N (Kb = 5.3 × 10-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of Ka for the acid HA.

What is the solubility of Mg(OH)2 (Ksp = 8.9 × 10-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Calculate the pH of a solution made by mixing 46.0 mL of 0.350 M NaA (Ka for HA = 1.0 × 10-9) with 26.0 mL of 0.190 M HCl.

A 50.0-mL sample of 2.0 × 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN)32-: What is the concentration of CN- at equilibrium?

Chromate ion is added to a saturated solution of Ag2CrO4 to reach 0.10 M CrO42-. Calculate the final concentration of silver ion at equilibrium (Ksp for Ag2CrO4 is 9.0 × 10-12).

The cation M2+ reacts with NH3 to form a series of complex ions as follows: Consider an experiment in which 1.0 × 10-3 mol of M(NO3)2 is added to 1.0 L of 15.0 M NH3. Calculate the equilibrium concentrations of M2+, M(NH3)22+, and M(NH3)32+

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + H⁺ pK_a = 6.4 H₂PO₄^- HPO₄^2- + H⁺ pK_a = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

Calculate the molar concentration of uncomplexed Zn²⁺ in a solution that contains 0.20 mol of Zn(NH₃)₄²⁺ per liter. The overall K_f for Zn(NH₃)₄²⁺ is 3.8 × 10⁹.

How many moles of Fe(OH)₂ [K_sp = 1.8 × 10^-15] will dissolve in 1 L of water buffered at pH = 12.00?

The concentration of Al³⁺ in a saturated solution of Al(OH)₃ at 25°C is 5.2 × 10^-9 M. Calculate the K_sp for Al(OH)₃.

Calculate the pH of the final solution obtained by mixing the following solutions. For HCN, K_a = 6.2 × 10^-10.50.0 mL of 0.10 M HNO₃ 60.0 mL of 0.20 M Ba(OH)₂ 95.0 mL of 0.20 M HClO₄195.0 mL of 1.0 × 10^-4 M HCN

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 220.0 mL of 0.200 M NaOH is added

Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2 × 10^-10), 1.00 M NaOH and 1.50 M NaCN.

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃^2-: The concentration of Cu⁺ at equilibrium is

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃. Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: The concentration of Ag⁺ at equilibrium is

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49 × 10^-2, K_a2 = 2.03 × 10^-6. -Calculate [H⁺] after 150.0 mL of 1.00 M NaOH has been added.

In a solution prepared by adding excess PbI₂(s) [K_sp = 1.4 × 10^-8] to water, [I^-] at equilibrium is

A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3 × 10^-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of K_a for the acid HA.

What is the solubility of Mg(OH)₂ (K_sp = 8.9 × 10^-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Calculate the pH of a solution made by mixing 46.0 mL of 0.350 M NaA (K_a for HA = 1.0 × 10^-9) with 26.0 mL of 0.190 M HCl.

A 50.0-mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃^2-: What is the concentration of CN^- at equilibrium?

Chromate ion is added to a saturated solution of Ag₂CrO₄ to reach 0.10 M CrO₄^2-. Calculate the final concentration of silver ion at equilibrium (K_sp for Ag₂CrO₄ is 9.0 × 10^-12).

The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: Consider an experiment in which 1.0 × 10^-3 mol of M(NO₃)₂ is added to 1.0 L of 15.0 M NH₃. Calculate the equilibrium concentrations of M²⁺, M(NH₃)₂²⁺, and M(NH₃)₃²⁺