How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq)to make a buffer with a pH of 9.00? (pKa of NH4+ = 9.25)

A) 0.36 mol B) 0.44 mol C) 0.56 mol D) 0.64 mol E) 1.8 mol A) 0.36 mol B) 0.44 mol C) 0.56 mol D) 0.64 mol E) 1.8 mol D

Given the two equilibria below, Ag(NH3)2+(aq) Ag+(aq)+ 2NH3(aq); Kd = 5.9 × 10-8 AgCN(s) Ag+(aq)+ CN−(aq); Ksp = what is K for the following equilibrium? AgCN(s)+ 2NH3(aq) Ag(NH3)2+(aq)+ CN-(aq)

A) B) C) D) E) A) B) C) D) E) A

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

Consider the titration of 300.0 mL of 0.414 M NH3 (Kb = 1.8 ×10-5)with 0.500 M HNO3.After 150.0 mL HNO3 has been added,what is the pH of the solution?

A) 4.93 B) 9.07 C) 6.07 D) 11.07 E) 7.00 A) 4.93 B) 9.07 C) 6.07 D) 11.07 E) 7.00

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 molar solubility of solid iron(III)hydroxide,Fe(OH)3,in a solution that is buffered to a pH of 2.50 at 25 °C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25 °C.

A) 6.9 × 10-28 mol/L B) 2.0 × 10-26 mol/L C) 1.3 × 10-13 mol/L D) 2.0 × 10-3 mol/L E) 5.0 × 102 mol/L A) 6.9 × 10-28 mol/L B) 2.0 × 10-26 mol/L C) 1.3 × 10-13 mol/L D) 2.0 × 10-3 mol/L E) 5.0 × 102 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 minimum concentration of Cd2+ required to begin precipitating Cd(OH)2(s)in a solution buffered at pH 10.83? The Ksp of Cd(OH)2 is 5.3 × 10-15 and Kw = 1.01 × 10-14.

A) 3.4 × 10-4 M B) 3.6 × 10-4 M C) 7.8 × 10-12 M D) 1.2 × 10-8 M E) 4.5 × 10-17 M A) 3.4 × 10-4 M B) 3.6 × 10-4 M C) 7.8 × 10-12 M D) 1.2 × 10-8 M E) 4.5 × 10-17 M

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

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How many moles of HCl must be added to 1.0 L of 1.0 M NH₃(aq)to make a buffer with a pH of 9.00? (pK_a of NH₄⁺ = 9.25)

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Question 1

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Which of the following mathematical expressions is the Henderson-Hasselbalch equation?

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Question 2

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Given the two equilibria below, Ag(NH₃)₂⁺(aq) Ag⁺(aq)+ 2NH₃(aq); K_d = 5.9 × 10^-8 AgCN(s) Ag⁺(aq)+ CN−(aq); K_sp = what is K for the following equilibrium? AgCN(s)+ 2NH₃(aq) Ag(NH₃)₂⁺(aq)+ CN^-(aq)

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Question 3

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

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Question 4

What is the pH of a solution that is 0.044 M in HA and also 0.0044 M in NaA? (K_a = 4.7 × 10^-6)

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Question 5

If the ratio of acid to base in a buffer is increased by a factor of 10,the buffer pH decreases by ________.

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Question 6

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 7

Consider the titration of 300.0 mL of 0.414 M NH₃ (K_b = 1.8 ×10^-5)with 0.500 M HNO₃.After 150.0 mL HNO₃ has been added,what is the pH of the solution?

(Multiple Choice)

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Question 8

What is the value of the dissociation constant,K_dissociation,for the complex ion Zn(NH₃)₄²⁺? (K_f = 2.9 × 10⁹)

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Question 9

A 50.0 mL sample of 0.155 M HNO₂(aq)is titrated with 0.100 M NaOH(aq).What is the pH of a solution after the addition of 25.0 mL of NaOH? (K_a of HNO₂ = 4.5 × 10^-4)

(Multiple Choice)

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Question 10

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 11

What is the molar solubility of solid iron(III)hydroxide,Fe(OH)₃,in a solution that is buffered to a pH of 2.50 at 25 °C? The K_sp of Fe(OH)₃ is 6.3 × 10^-38 at 25 °C.

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Question 12

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)?

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Question 13

What color change is exhibited by phenolphthalein during a titration of aqueous acetic acid with aqueous sodium hydroxide?

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Question 14

The solubility of strontium carbonate (SrCO₃)in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

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Question 15

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 16

Given the following equilibrium constants, Zn4IO₃)₂ K_sp = Zn(NH₃)₄²⁺ K_f = determine K for the dissolution of the sparingly soluble salt Zn(IO₃)₂ in aqueous ammonia (shown below). Zn(IO₃)₂(s)+ 4NH₃(aq)⇌ Zn(NH₃)₄²⁺(aq)+ 2IO₃^-(aq)

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Question 17

Which acid-base combination is depicted by this titration curve? The dot on the curve is located at the titrant volume where the titration solution pH equals 7.

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Question 18

What is the minimum concentration of Cd²⁺ required to begin precipitating Cd(OH)₂(s)in a solution buffered at pH 10.83? The K_sp of Cd(OH)₂ is 5.3 × 10^-15 and K_w = 1.01 × 10^-14.

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Question 19

How many moles of solid NaF would have to be added to 1.0 L of 1.85 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)

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Question 20

Showing 1 - 20 of 86

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

How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq)to make a buffer with a pH of 9.00? (pKa of NH4+ = 9.25)

Which of the following mathematical expressions is the Henderson-Hasselbalch equation?

Given the two equilibria below, Ag(NH3)2+(aq) Ag+(aq)+ 2NH3(aq); Kd = 5.9 × 10-8 AgCN(s) Ag+(aq)+ CN−(aq); Ksp = what is K for the following equilibrium? AgCN(s)+ 2NH3(aq) Ag(NH3)2+(aq)+ CN-(aq)

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

What is the pH of a solution that is 0.044 M in HA and also 0.0044 M in NaA? (Ka = 4.7 × 10-6)

If the ratio of acid to base in a buffer is increased by a factor of 10,the buffer pH decreases by ________.

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.

Consider the titration of 300.0 mL of 0.414 M NH3 (Kb = 1.8 ×10-5)with 0.500 M HNO3.After 150.0 mL HNO3 has been added,what is the pH of the solution?

What is the value of the dissociation constant,Kdissociation,for the complex ion Zn(NH3)42+? (Kf = 2.9 × 109)

A 50.0 mL sample of 0.155 M HNO2(aq)is titrated with 0.100 M NaOH(aq).What is the pH of a solution after the addition of 25.0 mL of NaOH? (Ka of HNO2 = 4.5 × 10-4)

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 molar solubility of solid iron(III)hydroxide,Fe(OH)3,in a solution that is buffered to a pH of 2.50 at 25 °C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25 °C.

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 color change is exhibited by phenolphthalein during a titration of aqueous acetic acid with aqueous sodium hydroxide?

The solubility of strontium carbonate (SrCO3)in water at 25°C is g/L.What is the Ksp of this sparingly soluble salt?

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.

​Given the following equilibrium constants, Zn4IO3)2 Ksp = Zn(NH3)42+ Kf = determine K for the dissolution of the sparingly soluble salt Zn(IO3)2 in aqueous ammonia (shown below). Zn(IO3)2(s)+ 4NH3(aq)⇌ Zn(NH3)42+(aq)+ 2IO3-(aq)

Which acid-base combination is depicted by this titration curve? The dot on the curve is located at the titrant volume where the titration solution pH equals 7.

What is the minimum concentration of Cd2+ required to begin precipitating Cd(OH)2(s)in a solution buffered at pH 10.83? The Ksp of Cd(OH)2 is 5.3 × 10-15 and Kw = 1.01 × 10-14.

How many moles of solid NaF would have to be added to 1.0 L of 1.85 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(Ka for HF = 7.2 × 10-4)

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How many moles of HCl must be added to 1.0 L of 1.0 M NH₃(aq)to make a buffer with a pH of 9.00? (pK_a of NH₄⁺ = 9.25)

Given the two equilibria below, Ag(NH₃)₂⁺(aq) Ag⁺(aq)+ 2NH₃(aq); K_d = 5.9 × 10^-8 AgCN(s) Ag⁺(aq)+ CN−(aq); K_sp = what is K for the following equilibrium? AgCN(s)+ 2NH₃(aq) Ag(NH₃)₂⁺(aq)+ CN^-(aq)

What is the pH of a solution that is 0.044 M in HA and also 0.0044 M in NaA? (K_a = 4.7 × 10^-6)

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.

Consider the titration of 300.0 mL of 0.414 M NH₃ (K_b = 1.8 ×10^-5)with 0.500 M HNO₃.After 150.0 mL HNO₃ has been added,what is the pH of the solution?

What is the value of the dissociation constant,K_dissociation,for the complex ion Zn(NH₃)₄²⁺? (K_f = 2.9 × 10⁹)

A 50.0 mL sample of 0.155 M HNO₂(aq)is titrated with 0.100 M NaOH(aq).What is the pH of a solution after the addition of 25.0 mL of NaOH? (K_a of HNO₂ = 4.5 × 10^-4)

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 molar solubility of solid iron(III)hydroxide,Fe(OH)₃,in a solution that is buffered to a pH of 2.50 at 25 °C? The K_sp of Fe(OH)₃ is 6.3 × 10^-38 at 25 °C.

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)?

The solubility of strontium carbonate (SrCO₃)in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

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.

Given the following equilibrium constants, Zn4IO₃)₂ K_sp = Zn(NH₃)₄²⁺ K_f = determine K for the dissolution of the sparingly soluble salt Zn(IO₃)₂ in aqueous ammonia (shown below). Zn(IO₃)₂(s)+ 4NH₃(aq)⇌ Zn(NH₃)₄²⁺(aq)+ 2IO₃^-(aq)

What is the minimum concentration of Cd²⁺ required to begin precipitating Cd(OH)₂(s)in a solution buffered at pH 10.83? The K_sp of Cd(OH)₂ is 5.3 × 10^-15 and K_w = 1.01 × 10^-14.

How many moles of solid NaF would have to be added to 1.0 L of 1.85 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)