Question 1

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO2H (a weak acid) requires what volume of 0.2 M sodium hydroxide?

Accepted Answer

A)  50 ml 
B)  25 ml 
C)  less than 25 ml as formic acid is a weak acid 
D)  100 ml 
E)  between 25 and 50 ml as formic acid is a weak acid 
A)  50 ml 
B)  25 ml 
C)  less than 25 ml as formic acid is a weak acid 
D)  100 ml 
E)  between 25 and 50 ml as formic acid is a weak acid

Question 2

Calculate the concentrations of species involved in complex-ion formation.

Accepted Answer

Electron-donating ligands are

Question 3

Write the equilibrium constant expression and determine the solubility constant for CuS dissolving in an ammonia solution. (CuS, Ksp = 8 x10-37) (Cu(NH3)4+2, Kf = 1.1 x 1013)

Accepted Answer

K = K_spK_f = 8

Question 4

A real world application of solubility products is found in softening "hard water" by removing calcium and magnesium ions present as the sulphate and carbonate salts. We can decrease the amount of Ca2+ in solution by addition of sodium carbonate, a strong electrolyte:Na2CO3 (s)$\rightarrow$2 Na+ (aq) + CO32- (aq)By increasing the concentration of carbonate, we tend to drive the solubility equilibrium toward the reactant:CaCO3 (s)   Ca2+ (aq) + CO32- (aq) Ksp = 4.7 x 10-9If the initial [Ca2+] = 5.0 x 10-3 M, what percent of the [Ca2+] will be removed if the carbonate concentration is maintained at 1.0 x 10-3 M?

Accepted Answer

The answer of A real world application of solubility products...

Question 5

Calculate an acid or a base concentration from titration data.

Accepted Answer

At the stoichiometric point, j

Question 6

What is the concentration of [PbCl3]-prepared from a solution of 0.5 M CaCl2 and solid PbCl2?Pb2+ + 3Cl- ? [PbCl3]- Kf = 2.4 x 101pKsp(PbCl2) = 4.77

Accepted Answer

Multi-step problem. Must use c

Question 7

100 ml of aqueous solution is 0.2 M in both Mg2+ and Pb2+ ions. You wish to separate the two metal ions by adding oxalate, C2O42-. What is the mass of PbC2O4 precipitated before Mg2+ begins to precipitate?Ksp (MgC2O4) = 8.5 x 10-5 Ksp (PbC2O4) = 2.7 x 10-11

Accepted Answer

Pb²⁺concentration drops from 0.2

Question 8

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO2H (a weak acid) requires what volume of 0.2 M methylamine, CH3NH2 (a weak base)?

Accepted Answer

A)  50 ml 
B)  25 ml 
C)  impossible to determine unless Ka for formic acid is known 
D)  impossible to determine unless Kb for methalamine is known 
E)  impossible to determine unless both Ka for formic acid and Kb for methylamine are known 
A)  50 ml 
B)  25 ml 
C)  impossible to determine unless Ka for formic acid is known 
D)  impossible to determine unless Kb for methalamine is known 
E)  impossible to determine unless both Ka for formic acid and Kb for methylamine are known

Question 9

How would you make a buffer of pH = 3.75 from the following solutions with a total volume of 450 ml? (Ka = 1.77 x10-4 for Formic Acid, HCO2H); 0.100M NaHCOO; 0.100 M HClO4; 0.100 M NaOH, 0.100 M NH3

Accepted Answer

take 300 ml of NaHCO

Question 10

What is the molar concentration of barium in a 0.01 M ammonium sulphate solution saturated with Ba(NO3)2?

Accepted Answer

Question 11

Which of the following solutions is a buffer?
I. 50 mL of 0.1 M acetic acid mixed with 25 mL of 0.05 M NaOH
II. 100 mL of 0.1 M acetic acid mixed with 25 mL of 0.5 M NaOH
III. 50 mL of 0.1 M acetic acid mixed with 25 mL of 0.05 M sodium acetate
IV. 50 mL of 0.1 M acetic acid mixed with 25 mL of 0.2 M HCl
V. 50 mL of 0.1 M sodium acetate mixed with 25 mL of 0.05 M NaOH

Accepted Answer

A)  I and III 
B)  III only 
C)  I, II and V 
D)  III, IV and V 
E)  II, IV and V 
A)  I and III 
B)  III only 
C)  I, II and V 
D)  III, IV and V 
E)  II, IV and V

Question 12

What are the major species present when 10 ml of 0.1 M NaOH are added to 40 ml of 0.0.05 M CH3COOH?

Accepted Answer

A)  Na+, OH-, H2O and CH3COOH 
B)  CH3COOH and CH3COO- 
C)  H2O, Na+ and CH3COO- 
D)  NaOH, CH3COOH and H2O 
E)  Na+, H2O, CH3COOH, CH3COO- 
A)  Na+, OH-, H2O and CH3COOH 
B)  CH3COOH and CH3COO- 
C)  H2O, Na+ and CH3COO- 
D)  NaOH, CH3COOH and H2O 
E)  Na+, H2O, CH3COOH, CH3COO-

Question 13

A solution is prepared by adding 0.14 mole Na2HPO4 and 8.2 grams of NaH2PO4 to sufficient water to prepare 1.00 L of solution. What is the pH of the solution? What is the pH of the solution after 0.041 moles HCl are added?If needed, use the following equation: pH = pKa + log(A-/HA)

Accepted Answer

Question 14

At 100°C, 2.1 x 10-2 g of AgCl dissolves in 1.00 L of water. What is the Ksp of AgCl at 100°C?

Accepted Answer

Question 15

A qualitative sketch of the titration curve for acetylsalicylic acid is shown at right.Given the indicators listed, which one would be suitable for titrations of acetylsalicylic acid?

Accepted Answer

phenol red

Question 16

Sodium carbonate, also called soda ash, is often analyzed by titration with strong acid. Initial concentrations of the carbonate ions are about 0.1 M. What indicator(s) would be suitable for detecting the stoichiometric point in this titration? (for H2CO3: pKa1 = 3.75 pKa2 = 10.33)

Accepted Answer

A)  I only 
B)  I and II 
C)  III only 
D)  IV only 
E)  I and V 
A)  I only 
B)  I and II 
C)  III only 
D)  IV only 
E)  I and V

Question 17

In which solution will copper nitrate (Cu(NO3)2) be the least soluble?

Accepted Answer

A)  0.1 M NaNO3 
B)  0.1 M NH3 
C)  pure water 
D)  0.1 M CuCl2 
E)  0.1 M NaOH 
A)  0.1 M NaNO3 
B)  0.1 M NH3 
C)  pure water 
D)  0.1 M CuCl2 
E)  0.1 M NaOH

Question 18

At what pH will an 0.0010 M of iron (III) nitrate (Ksp (Fe(OH)3)= 4.0 x 10-38) begin to precipitate?

Accepted Answer

A)  2.55 
B)  4.22 
C)  5.55 
D)  7.41 
E)  9.03 
A)  2.55 
B)  4.22 
C)  5.55 
D)  7.41 
E)  9.03

Question 19

In which of the following titrations will the pH be greater than 7 at the equivalence point?

Accepted Answer

A)  perchloric acid titrated with lithium hydroxide 
B)  acetic acid titrated with sodium hydroxide 
C)  sodium hydroxide titrated with hydrochloric acid 
D)  ammonium bromide titrated with perchloric acid 
E)  perchloric acid titrated with methyl amine 
A)  perchloric acid titrated with lithium hydroxide 
B)  acetic acid titrated with sodium hydroxide 
C)  sodium hydroxide titrated with hydrochloric acid 
D)  ammonium bromide titrated with perchloric acid 
E)  perchloric acid titrated with methyl amine

Question 20

Which of the following mixtures would make a buffer of pH = 4.74? (pKa of acetic acid is 4.74)

Accepted Answer

A)  100 mL of 0.10 M HCl and 100 mL of 0.10 M NaC2H3O2 
B)  100 mL of 0.10 M HCl and 100 mL of 0.10 M HC2H3O2 
C)  50 mL of 0.10 M HC2H3O2 and 100 mL of 0.10 M NaC2H3O2 
D)  100 mL of 0.10 M NaOH and 100 mL of 0.10 M NaC2H3O2 
E)  50 mL of 0.10 M NaOH and 100 mL of 0.10 M HC2H3O2 
A)  100 mL of 0.10 M HCl and 100 mL of 0.10 M NaC2H3O2 
B)  100 mL of 0.10 M HCl and 100 mL of 0.10 M HC2H3O2 
C)  50 mL of 0.10 M HC2H3O2 and 100 mL of 0.10 M NaC2H3O2 
D)  100 mL of 0.10 M NaOH and 100 mL of 0.10 M NaC2H3O2 
E)  50 mL of 0.10 M NaOH and 100 mL of 0.10 M HC2H3O2

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO₂H (a weak acid) requires what volume of 0.2 M sodium hydroxide?

Calculate the concentrations of species involved in complex-ion formation.

Write the equilibrium constant expression and determine the solubility constant for CuS dissolving in an ammonia solution. (CuS, K_sp = 8 x10^-37) (Cu(NH₃)₄⁺², K_f = 1.1 x 10¹³)

Calculate an acid or a base concentration from titration data.

What is the concentration of [PbCl₃]^-prepared from a solution of 0.5 M CaCl₂ and solid PbCl₂?Pb²⁺ + 3Cl^- ? [PbCl₃]^- K_f = 2.4 x 10¹pK_sp(PbCl₂) = 4.77

100 ml of aqueous solution is 0.2 M in both Mg²⁺ and Pb²⁺ ions. You wish to separate the two metal ions by adding oxalate, C₂O₄^2-. What is the mass of PbC₂O₄ precipitated before Mg²⁺begins to precipitate?K_sp (MgC₂O₄) = 8.5 x 10^-5 K_sp (PbC₂O₄) = 2.7 x 10^-11

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO₂H (a weak acid) requires what volume of 0.2 M methylamine, CH₃NH₂ (a weak base)?

How would you make a buffer of pH = 3.75 from the following solutions with a total volume of 450 ml? (K_a = 1.77 x10^-4 for Formic Acid, HCO₂H); 0.100M NaHCOO; 0.100 M HClO₄; 0.100 M NaOH, 0.100 M NH₃

What is the molar concentration of barium in a 0.01 M ammonium sulphate solution saturated with Ba(NO₃)₂?

What are the major species present when 10 ml of 0.1 M NaOH are added to 40 ml of 0.0.05 M CH₃COOH?

A solution is prepared by adding 0.14 mole Na₂HPO₄ and 8.2 grams of NaH₂PO₄ to sufficient water to prepare 1.00 L of solution. What is the pH of the solution? What is the pH of the solution after 0.041 moles HCl are added?If needed, use the following equation: pH = pK_a + log(A^-/HA)

At 100°C, 2.1 x 10^-2 g of AgCl dissolves in 1.00 L of water. What is the K_sp of AgCl at 100°C?

A qualitative sketch of the titration curve for acetylsalicylic acid is shown at right.Given the indicators listed, which one would be suitable for titrations of acetylsalicylic acid?

Sodium carbonate, also called soda ash, is often analyzed by titration with strong acid. Initial concentrations of the carbonate ions are about 0.1 M. What indicator(s) would be suitable for detecting the stoichiometric point in this titration? (for H₂CO₃: pK_a1 = 3.75 pK_a2 = 10.33)

In which solution will copper nitrate (Cu(NO₃)₂) be the least soluble?

At what pH will an 0.0010 M of iron (III) nitrate (K_sp (Fe(OH)₃)= 4.0 x 10^-38) begin to precipitate?

In which of the following titrations will the pH be greater than 7 at the equivalence point?

Which of the following mixtures would make a buffer of pH = 4.74? (pK_a of acetic acid is 4.74)

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Electron Transfer Reactions

Macromolecules

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The Main Group Elements

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Exam 16: Applications of Aqueous Equilibria

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO2H (a weak acid) requires what volume of 0.2 M sodium hydroxide?

Calculate the concentrations of species involved in complex-ion formation.

Write the equilibrium constant expression and determine the solubility constant for CuS dissolving in an ammonia solution. (CuS, Ksp = 8 x10-37) (Cu(NH3)4+2, Kf = 1.1 x 1013)

Calculate an acid or a base concentration from titration data.

What is the concentration of [PbCl3]-prepared from a solution of 0.5 M CaCl2 and solid PbCl2?Pb2+ + 3Cl- ? [PbCl3]- Kf = 2.4 x 101pKsp(PbCl2) = 4.77

100 ml of aqueous solution is 0.2 M in both Mg2+ and Pb2+ ions. You wish to separate the two metal ions by adding oxalate, C2O42-. What is the mass of PbC2O4 precipitated before Mg2+ begins to precipitate?Ksp (MgC2O4) = 8.5 x 10-5 Ksp (PbC2O4) = 2.7 x 10-11

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO2H (a weak acid) requires what volume of 0.2 M methylamine, CH3NH2 (a weak base)?

How would you make a buffer of pH = 3.75 from the following solutions with a total volume of 450 ml? (Ka = 1.77 x10-4 for Formic Acid, HCO2H); 0.100M NaHCOO; 0.100 M HClO4; 0.100 M NaOH, 0.100 M NH3

What is the molar concentration of barium in a 0.01 M ammonium sulphate solution saturated with Ba(NO3)2?

What are the major species present when 10 ml of 0.1 M NaOH are added to 40 ml of 0.0.05 M CH3COOH?

A solution is prepared by adding 0.14 mole Na2HPO4 and 8.2 grams of NaH2PO4 to sufficient water to prepare 1.00 L of solution. What is the pH of the solution? What is the pH of the solution after 0.041 moles HCl are added?If needed, use the following equation: pH = pKa + log(A-/HA)

At 100°C, 2.1 x 10-2 g of AgCl dissolves in 1.00 L of water. What is the Ksp of AgCl at 100°C?

A qualitative sketch of the titration curve for acetylsalicylic acid is shown at right.Given the indicators listed, which one would be suitable for titrations of acetylsalicylic acid?

Sodium carbonate, also called soda ash, is often analyzed by titration with strong acid. Initial concentrations of the carbonate ions are about 0.1 M. What indicator(s) would be suitable for detecting the stoichiometric point in this titration? (for H2CO3: pKa1 = 3.75 pKa2 = 10.33)

In which solution will copper nitrate (Cu(NO3)2) be the least soluble?

At what pH will an 0.0010 M of iron (III) nitrate (Ksp (Fe(OH)3)= 4.0 x 10-38) begin to precipitate?

In which of the following titrations will the pH be greater than 7 at the equivalence point?

Which of the following mixtures would make a buffer of pH = 4.74? (pKa of acetic acid is 4.74)

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO₂H (a weak acid) requires what volume of 0.2 M sodium hydroxide?

Write the equilibrium constant expression and determine the solubility constant for CuS dissolving in an ammonia solution. (CuS, K_sp = 8 x10^-37) (Cu(NH₃)₄⁺², K_f = 1.1 x 10¹³)

What is the concentration of [PbCl₃]^-prepared from a solution of 0.5 M CaCl₂ and solid PbCl₂?Pb²⁺ + 3Cl^- ? [PbCl₃]^- K_f = 2.4 x 10¹pK_sp(PbCl₂) = 4.77

100 ml of aqueous solution is 0.2 M in both Mg²⁺ and Pb²⁺ ions. You wish to separate the two metal ions by adding oxalate, C₂O₄^2-. What is the mass of PbC₂O₄ precipitated before Mg²⁺begins to precipitate?K_sp (MgC₂O₄) = 8.5 x 10^-5 K_sp (PbC₂O₄) = 2.7 x 10^-11

The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO₂H (a weak acid) requires what volume of 0.2 M methylamine, CH₃NH₂ (a weak base)?

How would you make a buffer of pH = 3.75 from the following solutions with a total volume of 450 ml? (K_a = 1.77 x10^-4 for Formic Acid, HCO₂H); 0.100M NaHCOO; 0.100 M HClO₄; 0.100 M NaOH, 0.100 M NH₃

What is the molar concentration of barium in a 0.01 M ammonium sulphate solution saturated with Ba(NO₃)₂?

What are the major species present when 10 ml of 0.1 M NaOH are added to 40 ml of 0.0.05 M CH₃COOH?

A solution is prepared by adding 0.14 mole Na₂HPO₄ and 8.2 grams of NaH₂PO₄ to sufficient water to prepare 1.00 L of solution. What is the pH of the solution? What is the pH of the solution after 0.041 moles HCl are added?If needed, use the following equation: pH = pK_a + log(A^-/HA)

At 100°C, 2.1 x 10^-2 g of AgCl dissolves in 1.00 L of water. What is the K_sp of AgCl at 100°C?

Sodium carbonate, also called soda ash, is often analyzed by titration with strong acid. Initial concentrations of the carbonate ions are about 0.1 M. What indicator(s) would be suitable for detecting the stoichiometric point in this titration? (for H₂CO₃: pK_a1 = 3.75 pK_a2 = 10.33)

In which solution will copper nitrate (Cu(NO₃)₂) be the least soluble?

At what pH will an 0.0010 M of iron (III) nitrate (K_sp (Fe(OH)₃)= 4.0 x 10^-38) begin to precipitate?

Which of the following mixtures would make a buffer of pH = 4.74? (pK_a of acetic acid is 4.74)