Question 1

Explain how to decide on a specific indicator for a given titration.

Accepted Answer

See Sectio

Question 2

Calculate the molar solubility of BaCO3 (Ksp = 1.6 × 10-9) in a 0.42M BaCl2 solution.

Accepted Answer

A)  6.2 × 10-4 M 
B)  2.6 × 10-5 M 
C)  6.7 × 10-10 M 
D)  4.0 × 10-5 M 
E)  3.8 × 10-9 M 
A)  6.2 × 10-4 M 
B)  2.6 × 10-5 M 
C)  6.7 × 10-10 M 
D)  4.0 × 10-5 M 
E)  3.8 × 10-9 M

Question 3

Derive the equation describing the relationship between the pH at the first equivalence point and the Ka values of the diprotic weak acid being titrated with NaOH.

Accepted Answer

See Sectio

Question 4

An indicator HIn has Ka = 1 × 10-8. At pH = 6.0, what is the ratio HIn/In-?

Accepted Answer

A)  1/100 
B)  10/1 
C)  1/1 
D)  100/1 
E)  none of these 
A)  1/100 
B)  10/1 
C)  1/1 
D)  100/1 
E)  none of these

Question 5

​Which of the following statements is/are true of titrations?
1) The stoichiometric or equivalence point in a titration is usually signaled by the color change of an indicator.2. The pH at the equivalence point of a titration of a weak acid with a strong base is always greater than 7.3. The pH at the equivalence point of a titration of a strong acid with a strong base is equal to 7.

Accepted Answer

A)  1 only​ 
B)  3 only 
C)  1, 2, and 3 
D)  2 and 3 
E)  2 only 
A)  1 only​ 
B)  3 only 
C)  1, 2, and 3 
D)  2 and 3 
E)  2 only

Question 6

Calculate [H+] in a solution that is 0.30M in NaF and 0.46 M in HF. (Ka = 7.2 × 10-4)

Accepted Answer

A)  1.2 × 10-4 M 
B)  5.7 × 10-3 M 
C)  231.5 × 10-2 M 
D)  4.7 × 10-4 M 
E)  0.46 M 
A)  1.2 × 10-4 M 
B)  5.7 × 10-3 M 
C)  231.5 × 10-2 M 
D)  4.7 × 10-4 M 
E)  0.46 M

Question 7

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 × 10S1U1P1-3S1S1P0 M CuNOS1U1B13S1U1B0. Cu(I) forms complex ions with cyanide as follows:   Calculate the following concentrations at equilibrium:
-[Cu(CN)32-]

Accepted Answer

A)  3.33 M 
B)  1.67 M 
C)  2.0 × 10-3 M 
D)  1.0 × 10-3 M 
E)  none of these 
A)  3.33 M 
B)  1.67 M 
C)  2.0 × 10-3 M 
D)  1.0 × 10-3 M 
E)  none of these

Question 8

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(NH3)2+ at equilibrium is

Accepted Answer

A)  0.20 M. 
B)  2.0 M. 
C)  0.40 M. 
D)  1.0 × 10-3 M. 
E)  none of these 
A)  0.20 M. 
B)  2.0 M. 
C)  0.40 M. 
D)  1.0 × 10-3 M. 
E)  none of these

Question 9

12.4​ mL of 0.25 M HCl is added to a 120.0-mL sample of 0.220 M HNO2 (Ka for HNO2 = 4.0 × 10-4). What is the equilibrium concentration of NO2- ions?

Accepted Answer

A)  ​3.4 × 10-3 M 
B)  ​2.3 × 10-2 M 
C)  ​3.9 × 10-3 M 
D)  ​4.7 × 10-4 M 
E)  ​9.4 × 10-3 M 
A)  ​3.4 × 10-3 M 
B)  ​2.3 × 10-2 M 
C)  ​3.9 × 10-3 M 
D)  ​4.7 × 10-4 M 
E)  ​9.4 × 10-3 M

Question 10

The pH at the equivalence point of a titration of a weak acid with a strong base is

Accepted Answer

A)  More data are needed to answer this question. 
B)  equal to 7.00. 
C)  greater than 7.00. 
D)  less than 7.00. 
A)  More data are needed to answer this question. 
B)  equal to 7.00. 
C)  greater than 7.00. 
D)  less than 7.00.

Question 11

A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. Assuming tartaric acid is diprotic, what is the molarity of the acid?

Accepted Answer

A) 10. 
B)  1.0 
C)  2.0 
D)  4.0 
E)  impossible to determine 
A) 10. 
B)  1.0 
C)  2.0 
D)  4.0 
E)  impossible to determine

Question 12

For the compound MX, Ksp is 2.00 × 10-11. The anion X- forms the weak acid HX (Ka = 1.8 × 10-5). Calculate the solubility of MX in 10.00 M strong acid.

Accepted Answer

Question 13

Consider the titration of 200.0 mL of a 0.100 M solution of the weak acid H2A with 0.200 M NaOH. The first equivalence point is reached after 100.0 mL of 0.200 M NaOH has been added, and the pH is 6.27. The pH after 65.0 mL of 0.200 M NaOH has been added, the pH is 4.95.Calculate the value of Ka2 for H2A.

Accepted Answer

A)  5.37 × 10-7 
B)  2.10 × 10-5 
C)  1.12 × 10-5 
D)  1.40 × 10-8 
E)  none of these 
A)  5.37 × 10-7 
B)  2.10 × 10-5 
C)  1.12 × 10-5 
D)  1.40 × 10-8 
E)  none of these

Question 14

How many mmoles of HCl must be added to 155.0 mL of a 0.28 M solution of methylamine (pKb = 3.36) to give a buffer having a pH of 11.42?

Accepted Answer

A)  19 mmol 
B)  0.17 mmol 
C)  6.2 mmol 
D)  3.7 mmol 
E)  0.61 mmol 
A)  19 mmol 
B)  0.17 mmol 
C)  6.2 mmol 
D)  3.7 mmol 
E)  0.61 mmol

Question 15

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

Accepted Answer

A)  greater than 
B)  cannot be determined 
C)  less than 
D)  about the same as 
A)  greater than 
B)  cannot be determined 
C)  less than 
D)  about the same as

Question 16

A 5.95-g sample of an acid, H2X, requires 45.0 mL of a 0.500 M NaOH solution for complete reaction (removing both protons). What is the molar mass of the acid expressed in grams per mol?

Accepted Answer

A)  529 
B)  264 
C)  178 
D)  132 
E)  none of these 
A)  529 
B)  264 
C)  178 
D)  132 
E)  none of these

Question 17

How many moles of Ca(NO3)2 must be added to 1.0 L of a 0.10 M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 × 10-11.

Accepted Answer

A)  4.0 × 10-9 mol 
B)  4.0 × 10-10 mol 
C)  4.5 × 10-7 mol 
D)  4.0 × 10-12 mol 
E)  4.0 × 10-13 mol 
A)  4.0 × 10-9 mol 
B)  4.0 × 10-10 mol 
C)  4.5 × 10-7 mol 
D)  4.0 × 10-12 mol 
E)  4.0 × 10-13 mol

Question 18

A certain indicator HIn has a pKa of 9.00, and a color change becomes visible when 7.00% of it is In-. At what pH is this color change visible?

Accepted Answer

A)  6.15 
B)  7.88 
C)  10.2 
D)  3.85 
E)  none of these 
A)  6.15 
B)  7.88 
C)  10.2 
D)  3.85 
E)  none of these

Question 19

You have a solution of 0.10 M Cl- and   . You add 0.10 M silver nitrate dropwise into the solution. Ksp for Ag2CrO4 is 9.0 × 10-12 and for AgCl is1.6 × 10-10. Which of the following will precipitate first?

Accepted Answer

A)  silver nitrate 
B)  silver chromate 
C)  cannot be determined from the information given 
D)  silver chloride 
E)  none of these 
A)  silver nitrate 
B)  silver chromate 
C)  cannot be determined from the information given 
D)  silver chloride 
E)  none of these

Question 20

A solution containing 10. mmol of CO32- and 5.0 mmol of HCO3- is titrated with
1)0 M HCl.What volume of HCl must be added to reach the first equivalence point?

Accepted Answer

A)  5.0 mL 
B)  15 mL 
C) 10. mL 
D)  25 mL 
E) 20. mL 
A)  5.0 mL 
B)  15 mL 
C) 10. mL 
D)  25 mL 
E) 20. mL

Explain how to decide on a specific indicator for a given titration.

Calculate the molar solubility of BaCO₃ (K_sp = 1.6 × 10^-9) in a 0.42M BaCl₂ solution.

Derive the equation describing the relationship between the pH at the first equivalence point and the K_a values of the diprotic weak acid being titrated with NaOH.

An indicator HIn has K_a = 1 × 10^-8. At pH = 6.0, what is the ratio HIn/In^-?

Calculate [H⁺] in a solution that is 0.30M in NaF and 0.46 M in HF. (K_a = 7.2 × 10^-4)

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 × 10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)₃^2-]

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(NH₃)₂⁺ at equilibrium is

12.4 mL of 0.25 M HCl is added to a 120.0-mL sample of 0.220 M HNO₂ (K_a for HNO₂ = 4.0 × 10^-4). What is the equilibrium concentration of NO₂- ions?

The pH at the equivalence point of a titration of a weak acid with a strong base is

A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. Assuming tartaric acid is diprotic, what is the molarity of the acid?

For the compound MX, K_sp is 2.00 × 10^-11. The anion X^- forms the weak acid HX (K_a= 1.8 × 10^-5). Calculate the solubility of MX in 10.00 M strong acid.

How many mmoles of HCl must be added to 155.0 mL of a 0.28 M solution of methylamine (pK_b = 3.36) to give a buffer having a pH of 11.42?

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

A 5.95-g sample of an acid, H₂X, requires 45.0 mL of a 0.500 M NaOH solution for complete reaction (removing both protons). What is the molar mass of the acid expressed in grams per mol?

How many moles of Ca(NO₃)₂ must be added to 1.0 L of a 0.10 M HF solution to begin precipitation of CaF₂(s)? For CaF₂, K_sp = 4.0 × 10^-11.

A certain indicator HIn has a pK_a of 9.00, and a color change becomes visible when 7.00% of it is In^-. At what pH is this color change visible?

You have a solution of 0.10 M Cl^- and . You add 0.10 M silver nitrate dropwise into the solution. K_sp for Ag₂CrO₄ is 9.0 × 10^-12 and for AgCl is1.6 × 10^-10. Which of the following will precipitate first?

A solution containing 10. mmol of CO₃^2- and 5.0 mmol of HCO₃^- is titrated with 1)0 M HCl.What volume of HCl must be added to reach the first equivalence point?

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

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Exam 8: Applications of Aqueous Equilibria

Explain how to decide on a specific indicator for a given titration.

Calculate the molar solubility of BaCO3 (Ksp = 1.6 × 10-9) in a 0.42M BaCl2 solution.

Derive the equation describing the relationship between the pH at the first equivalence point and the Ka values of the diprotic weak acid being titrated with NaOH.

An indicator HIn has Ka = 1 × 10-8. At pH = 6.0, what is the ratio HIn/In-?

Calculate [H+] in a solution that is 0.30M in NaF and 0.46 M in HF. (Ka = 7.2 × 10-4)

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 × 10-3 M CuNO3. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)32-]

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(NH3)2+ at equilibrium is

12.4​ mL of 0.25 M HCl is added to a 120.0-mL sample of 0.220 M HNO2 (Ka for HNO2 = 4.0 × 10-4). What is the equilibrium concentration of NO2- ions?

The pH at the equivalence point of a titration of a weak acid with a strong base is

A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. Assuming tartaric acid is diprotic, what is the molarity of the acid?

For the compound MX, Ksp is 2.00 × 10-11. The anion X- forms the weak acid HX (Ka = 1.8 × 10-5). Calculate the solubility of MX in 10.00 M strong acid.

How many mmoles of HCl must be added to 155.0 mL of a 0.28 M solution of methylamine (pKb = 3.36) to give a buffer having a pH of 11.42?

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

A 5.95-g sample of an acid, H2X, requires 45.0 mL of a 0.500 M NaOH solution for complete reaction (removing both protons). What is the molar mass of the acid expressed in grams per mol?

How many moles of Ca(NO3)2 must be added to 1.0 L of a 0.10 M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 × 10-11.

A certain indicator HIn has a pKa of 9.00, and a color change becomes visible when 7.00% of it is In-. At what pH is this color change visible?

You have a solution of 0.10 M Cl- and . You add 0.10 M silver nitrate dropwise into the solution. Ksp for Ag2CrO4 is 9.0 × 10-12 and for AgCl is1.6 × 10-10. Which of the following will precipitate first?

A solution containing 10. mmol of CO32- and 5.0 mmol of HCO3- is titrated with 1)0 M HCl.What volume of HCl must be added to reach the first equivalence point?

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

Calculate the molar solubility of BaCO₃ (K_sp = 1.6 × 10^-9) in a 0.42M BaCl₂ solution.

Derive the equation describing the relationship between the pH at the first equivalence point and the K_a values of the diprotic weak acid being titrated with NaOH.

An indicator HIn has K_a = 1 × 10^-8. At pH = 6.0, what is the ratio HIn/In^-?

Calculate [H⁺] in a solution that is 0.30M in NaF and 0.46 M in HF. (K_a = 7.2 × 10^-4)

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 × 10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)₃^2-]

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(NH₃)₂⁺ at equilibrium is

12.4 mL of 0.25 M HCl is added to a 120.0-mL sample of 0.220 M HNO₂ (K_a for HNO₂ = 4.0 × 10^-4). What is the equilibrium concentration of NO₂- ions?

For the compound MX, K_sp is 2.00 × 10^-11. The anion X^- forms the weak acid HX (K_a= 1.8 × 10^-5). Calculate the solubility of MX in 10.00 M strong acid.

How many mmoles of HCl must be added to 155.0 mL of a 0.28 M solution of methylamine (pK_b = 3.36) to give a buffer having a pH of 11.42?

A 5.95-g sample of an acid, H₂X, requires 45.0 mL of a 0.500 M NaOH solution for complete reaction (removing both protons). What is the molar mass of the acid expressed in grams per mol?

How many moles of Ca(NO₃)₂ must be added to 1.0 L of a 0.10 M HF solution to begin precipitation of CaF₂(s)? For CaF₂, K_sp = 4.0 × 10^-11.

A certain indicator HIn has a pK_a of 9.00, and a color change becomes visible when 7.00% of it is In^-. At what pH is this color change visible?

You have a solution of 0.10 M Cl^- and . You add 0.10 M silver nitrate dropwise into the solution. K_sp for Ag₂CrO₄ is 9.0 × 10^-12 and for AgCl is1.6 × 10^-10. Which of the following will precipitate first?

A solution containing 10. mmol of CO₃^2- and 5.0 mmol of HCO₃^- is titrated with 1)0 M HCl.What volume of HCl must be added to reach the first equivalence point?