Consider the reaction Cu2+(aq)+ 4 NH3(aq) Cu(NH3)42+(aq) Kf = 2.1 × 1013 If the Ksp for Cu(OH)2 is 2.2 × 10-20,what is the value of the equilibrium constant,K,for the reaction below? Cu(NH3)42+(aq)+ 2 OH-(aq) Cu(OH)2(s)+ 4 NH3(aq)

A) 1.0 × 10-33 B) 4.6 × 10-7 C) 2.1 × 1013 D) 2.2 × 106 E) 9.5 × 1032 A) 1.0 × 10-33 B) 4.6 × 10-7 C) 2.1 × 1013 D) 2.2 × 106 E) 9.5 × 1032

An impure sample of sodium carbonate,Na2CO3,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na2CO3(aq) CO2(g)+ H2O( )+ 2 NaCl(aq) What is the percent of Na2CO3 in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na2CO3 is 106.0 g/mol.

A) 0.295% B) 15.7% C) 25.5% D) 51.1% E) 67.9% A) 0.295% B) 15.7% C) 25.5% D) 51.1% E) 67.9%

What is the pH of a saturated solution of Fe(OH)2? (Ksp = 8.0 × 10-16 and Kw = 1.01 × 10-14)

A) 4.93 B) 8.77 C) 5.23 D) 9.07 E) 7.00 A) 4.93 B) 8.77 C) 5.23 D) 9.07 E) 7.00

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

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 pH of a solution made by combining 134 mL of 0.26 M NaC2H3O2 with 211 mL of 0.31 M HC2H3O2? The Ka of acetic acid is 1.75 × 10-5.

A) 4.47 B) 5.04 C) 5.52 D) 4.42 E) 4.97 A) 4.47 B) 5.04 C) 5.52 D) 4.42 E) 4.97

In which of the following solutions would silver(I)phosphate,Ag3PO4,be least soluble?

A) 0.10 M Na3PO4 B) 0.10 M AgNO3 C) 0.10 M Na2HPO4 D) 0.10 M HNO3 E) 0.10 M NaH2PO4 A) 0.10 M Na3PO4 B) 0.10 M AgNO3 C) 0.10 M Na2HPO4 D) 0.10 M HNO3 E) 0.10 M NaH2PO4

Given the following reactions, AgBr(s) Ag+(aq)+ Br-(aq) Ksp = 5.4 × 10-13 Ag+(aq)+ 2 CN-(aq) Ag(CN)2-(aq) Kf = 1.2 × 1021 Determine the equilibrium constant for the reaction below. AgBr(s)+ 2 CN-(aq) Ag(CN)2-(aq)+ Br-(aq)

A) 4.5 × 10-34 B) 1.5 × 10-9 C) 6.5 × 108 D) 1.2 × 1021 E) 2.2 × 1033 A) 4.5 × 10-34 B) 1.5 × 10-9 C) 6.5 × 108 D) 1.2 × 1021 E) 2.2 × 1033

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

Consider the reaction Cu²⁺(aq)+ 4 NH₃(aq) Cu(NH₃)₄²⁺(aq) K_f = 2.1 × 10¹³ If the K_sp for Cu(OH)₂ is 2.2 × 10^-20,what is the value of the equilibrium constant,K,for the reaction below? Cu(NH₃)₄²⁺(aq)+ 2 OH^-(aq) Cu(OH)₂(s)+ 4 NH₃(aq)

(Multiple Choice)

4.9/5

(43)

Question 41

A solution containing 10.mmol of CO₃²⁻and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

(Multiple Choice)

5.0/5

(40)

Question 42

An impure sample of sodium carbonate,Na₂CO₃,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na₂CO₃(aq) CO₂(g)+ H₂O( )+ 2 NaCl(aq) What is the percent of Na₂CO₃ in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na₂CO₃ is 106.0 g/mol.

(Multiple Choice)

4.8/5

(39)

Question 43

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

(Multiple Choice)

4.8/5

(29)

Question 44

To make a buffer with a pH of 8.00,you should use a weak acid with a K_a close to _______.

(Short Answer)

4.9/5

(45)

Question 45

What is the pH of a saturated solution of Fe(OH)₂? (K_sp = 8.0 × 10^-16 and K_w = 1.01 × 10^-14)

(Multiple Choice)

4.9/5

(45)

Question 46

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)

4.8/5

(32)

Question 47

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)

4.9/5

(31)

Question 48

What is the pH of a solution made by combining 134 mL of 0.26 M NaC₂H₃O₂ with 211 mL of 0.31 M HC₂H₃O₂? The K_a of acetic acid is 1.75 × 10^-5.

(Multiple Choice)

4.8/5

(30)

Question 49

A solution containing 10.mmol of CO₃²⁻ and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

(Multiple Choice)

4.9/5

(37)

Question 50

A buffer is composed of 0.400 mol H₂PO₄^- and 0.400 mol HPO₄^2- diluted with water to a volume of 1.00 L.The pH of the buffer is 7.210.How many moles of HCl must be added to decrease the pH to 6.210?

(Multiple Choice)

4.8/5

(41)

Question 51

For a monoprotic acid titration,the _____ in a titration is the point where number of moles of a strong base added equals the number of moles of an acid initially present.

(Short Answer)

4.8/5

(33)

Question 52

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq).What is the pH after the addition of 32.0 mL of HCl(aq)? (K_b of C₆H₅CO₂^- = 1.6 × 10^-10)

(Multiple Choice)

4.8/5

(35)

Question 53

Titration of 0.1615 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 21.84 mL of 0.1231 M NaOH to reach the endpoint.What is the molar mass of the acid?

(Multiple Choice)

4.9/5

(41)

Question 54

In which of the following solutions would silver(I)phosphate,Ag₃PO₄,be least soluble?

(Multiple Choice)

4.9/5

(36)

Question 55

The pH of a solution at the equivalence point in a monoprotic strong acid-−strong base reaction is always 7.0 at 25 °C.

(True/False)

4.7/5

(37)

Question 56

When mixed in appropriate amounts,each of the following mixtures can produce an effective buffer solution except _____.

(Multiple Choice)

4.9/5

(33)

Question 57

If the ratio of acid to base in a buffer increases by a factor of 10,the pH of the buffer

(Multiple Choice)

4.9/5

(38)

Question 58

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,and K_a3 = 3.6 × 10^-13)

(Multiple Choice)

4.7/5

(42)

Question 59

Given the following reactions, AgBr(s) Ag⁺(aq)+ Br^-(aq) K_sp = 5.4 × 10^-13 Ag⁺(aq)+ 2 CN^-(aq) Ag(CN)₂^-(aq) K_f = 1.2 × 10²¹ Determine the equilibrium constant for the reaction below. AgBr(s)+ 2 CN^-(aq) Ag(CN)₂^-(aq)+ Br^-(aq)

(Multiple Choice)

4.9/5

(44)

Question 60

Showing 41 - 60 of 86

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

Consider the reaction Cu2+(aq)+ 4 NH3(aq) Cu(NH3)42+(aq) Kf = 2.1 × 1013 If the Ksp for Cu(OH)2 is 2.2 × 10-20,what is the value of the equilibrium constant,K,for the reaction below? Cu(NH3)42+(aq)+ 2 OH-(aq) Cu(OH)2(s)+ 4 NH3(aq)

A solution containing 10.mmol of CO32−and 5.0 mmol of HCO3−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

An impure sample of sodium carbonate,Na2CO3,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na2CO3(aq) CO2(g)+ H2O( )+ 2 NaCl(aq) What is the percent of Na2CO3 in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na2CO3 is 106.0 g/mol.

A 25.00-mL sample of propionic acid,HC3H5O2,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

To make a buffer with a pH of 8.00,you should use a weak acid with a Ka close to _______.

What is the pH of a saturated solution of Fe(OH)2? (Ksp = 8.0 × 10-16 and Kw = 1.01 × 10-14)

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.

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 is the pH of a solution made by combining 134 mL of 0.26 M NaC2H3O2 with 211 mL of 0.31 M HC2H3O2? The Ka of acetic acid is 1.75 × 10-5.

A solution containing 10.mmol of CO32− and 5.0 mmol of HCO3−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

A buffer is composed of 0.400 mol H2PO4- and 0.400 mol HPO42- diluted with water to a volume of 1.00 L.The pH of the buffer is 7.210.How many moles of HCl must be added to decrease the pH to 6.210?

For a monoprotic acid titration,the _____ in a titration is the point where number of moles of a strong base added equals the number of moles of an acid initially present.

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq).What is the pH after the addition of 32.0 mL of HCl(aq)? (Kb of C6H5CO2- = 1.6 × 10-10)

Titration of 0.1615 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 21.84 mL of 0.1231 M NaOH to reach the endpoint.What is the molar mass of the acid?

In which of the following solutions would silver(I)phosphate,Ag3PO4,be least soluble?

The pH of a solution at the equivalence point in a monoprotic strong acid-−strong base reaction is always 7.0 at 25 °C.

When mixed in appropriate amounts,each of the following mixtures can produce an effective buffer solution except _____.

If the ratio of acid to base in a buffer increases by a factor of 10,the pH of the buffer

What is the pH of a buffer that results when 0.50 mole of H3PO4 is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are Ka1 = 7.5 × 10-3,Ka2 = 6.2 × 10-8,and Ka3 = 3.6 × 10-13)

Given the following reactions, AgBr(s) Ag+(aq)+ Br-(aq) Ksp = 5.4 × 10-13 Ag+(aq)+ 2 CN-(aq) Ag(CN)2-(aq) Kf = 1.2 × 1021 Determine the equilibrium constant for the reaction below. AgBr(s)+ 2 CN-(aq) Ag(CN)2-(aq)+ Br-(aq)

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

Filters

Consider the reaction Cu²⁺(aq)+ 4 NH₃(aq) Cu(NH₃)₄²⁺(aq) K_f = 2.1 × 10¹³ If the K_sp for Cu(OH)₂ is 2.2 × 10^-20,what is the value of the equilibrium constant,K,for the reaction below? Cu(NH₃)₄²⁺(aq)+ 2 OH^-(aq) Cu(OH)₂(s)+ 4 NH₃(aq)

A solution containing 10.mmol of CO₃²⁻and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

To make a buffer with a pH of 8.00,you should use a weak acid with a K_a close to _______.

What is the pH of a saturated solution of Fe(OH)₂? (K_sp = 8.0 × 10^-16 and K_w = 1.01 × 10^-14)

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.

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 is the pH of a solution made by combining 134 mL of 0.26 M NaC₂H₃O₂ with 211 mL of 0.31 M HC₂H₃O₂? The K_a of acetic acid is 1.75 × 10^-5.

A solution containing 10.mmol of CO₃²⁻ and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

A buffer is composed of 0.400 mol H₂PO₄^- and 0.400 mol HPO₄^2- diluted with water to a volume of 1.00 L.The pH of the buffer is 7.210.How many moles of HCl must be added to decrease the pH to 6.210?

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq).What is the pH after the addition of 32.0 mL of HCl(aq)? (K_b of C₆H₅CO₂^- = 1.6 × 10^-10)

In which of the following solutions would silver(I)phosphate,Ag₃PO₄,be least soluble?

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,and K_a3 = 3.6 × 10^-13)

Given the following reactions, AgBr(s) Ag⁺(aq)+ Br^-(aq) K_sp = 5.4 × 10^-13 Ag⁺(aq)+ 2 CN^-(aq) Ag(CN)₂^-(aq) K_f = 1.2 × 10²¹ Determine the equilibrium constant for the reaction below. AgBr(s)+ 2 CN^-(aq) Ag(CN)₂^-(aq)+ Br^-(aq)