You are given 5.00 mL of an H2SO4 solution of unknown concentration. You divide the 5.00-mL sample into five 1.00-mL samples and titrate each separately with 0.1000 M NaOH. In each titration, the H2SO4 is completely neutralized. The average volume of NaOH solution used to reach the endpoint is 15.3 mL. What was the concentration of H2SO4 in the 5.00-mL sample?

A) 0.306 M B) 0.765 M C) 3.06 M D) 1.53 × 10-3 M E) 1.53 M A) 0.306 M B) 0.765 M C) 3.06 M D) 1.53 × 10-3 M E) 1.53 M

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 the [H+] after 50.00 mL of 1.00 M NaOH has been added.

A) 2.00 × 10-6 M B) 1.41 × 10-10 M C) 1.49 × 10-2 M D) 3.87 × 10-2 M E) none of these A) 2.00 × 10-6 M B) 1.41 × 10-10 M C) 1.49 × 10-2 M D) 3.87 × 10-2 M E) none of these

Which of the following solutions will be the best buffer at a pH of 9.26? (Ka for HC2H3O2 is 1.8 × 10-5; Kb for NH3 is 1.8 × 10-5.)

A) 0.20M NH3 and 0.20M NH4Cl B) 5.0M HC2H3O2 and 5.0M NH4Cl C) 0.20M HC2H3O2 and 0.20M NaC2H3O2 D) 5.0M NH3 and 5.0M NH4Cl E) 5.0M HC2H3O2 and 5.0M NH3 A) 0.20M NH3 and 0.20M NH4Cl B) 5.0M HC2H3O2 and 5.0M NH4Cl C) 0.20M HC2H3O2 and 0.20M NaC2H3O2 D) 5.0M NH3 and 5.0M NH4Cl E) 5.0M HC2H3O2 and 5.0M NH3

The solubility, in moles per liter, of Ag2CrO4 is 1.3 × 10-4 M at 25°C. Calculate Ksp for this compound.

A) 2.3 × 10-13 B) 6.1 × 10-9 C) 8.8 × 10-12 D) 4.7 × 10-13 E) 8.8 × 10-3 A) 2.3 × 10-13 B) 6.1 × 10-9 C) 8.8 × 10-12 D) 4.7 × 10-13 E) 8.8 × 10-3

If 30 mL of 5.0 × 10-4 M Ca(NO3)2 is added to 70 mL of 2.0 × 10-4 M NaF, will a precipitate form? (Ksp of CaF2 = 4.0 × 10-11)

A) No, because the ion product is less than Ksp. B) No, because the ion product is greater than Ksp. C) Not enough information is given. D) Yes, because the ion product is less than Ksp. E) Yes, because the ion product is greater than Ksp. A) No, because the ion product is less than Ksp. B) No, because the ion product is greater than Ksp. C) Not enough information is given. D) Yes, because the ion product is less than Ksp. E) Yes, because the ion product is greater than Ksp.

A 100.-mL sample of 0.10 M HCl is mixed with 50. mL of 0.10 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 × 10-5)

A) 7.85 B) 1.30 C) 3.87 D) 1.48 E) 12.52 A) 7.85 B) 1.30 C) 3.87 D) 1.48 E) 12.52

Calculate the concentration of chromate ion, CrO42-, in a saturated solution of CaCrO4 (Ksp = 7.1 × 10-4).

A) 5.0 × 10-7 M B) 3.5 × 10-2 M C) 0.027 M D) 3.5 × 10-4 M E) 7.1 × 10-4 M A) 5.0 × 10-7 M B) 3.5 × 10-2 M C) 0.027 M D) 3.5 × 10-4 M E) 7.1 × 10-4 M

Exam 8: Applications of Aqueous Equilibria

What combination of substances will give a buffered solution that has a pH of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K_b for NH₃ = 1.8 × 10^-5; K_b for C₅H₅N = 1.7 × 10^-9)

(Multiple Choice)

4.8/5

(41)

Question 161

You are given 5.00 mL of an H₂SO₄ solution of unknown concentration. You divide the 5.00-mL sample into five 1.00-mL samples and titrate each separately with 0.1000 M NaOH. In each titration, the H₂SO₄ is completely neutralized. The average volume of NaOH solution used to reach the endpoint is 15.3 mL. What was the concentration of H₂SO₄ in the 5.00-mL sample?

(Multiple Choice)

4.9/5

(37)

Question 162

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 the [H⁺] after 50.00 mL of 1.00 M NaOH has been added.

(Multiple Choice)

4.8/5

(42)

Question 163

Which of the following solutions will be the best buffer at a pH of 9.26? (K_a for HC₂H₃O₂ is 1.8 × 10^-5; K_b for NH₃ is 1.8 × 10^-5.)

(Multiple Choice)

4.9/5

(35)

Question 164

Given the following K_sp values which statement about solubility, in moles per liter, in water is correct?

(Multiple Choice)

4.8/5

(39)

Question 165

A 73.5-mL sample of 0.18 M HNO₂ (K_a = 4.0 × 10^-4) is titrated with 0.12 M NaOH. What is the pH after 25.2 mL of NaOH has been added?

(Multiple Choice)

4.9/5

(42)

Question 166

The Ag⁺ ion reacts with NH₃ to form the following complex ions: AgCl (K_sp = 1.6 × 10^-10) is dissolved to its solubility limit in 10.0 M NH₃. Calculate the equilibrium concentrations of Ag⁺, Cl^-, Ag(NH₃)₂⁺, and NH₃.

(Essay)

4.9/5

(28)

Question 167

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

(Multiple Choice)

4.9/5

(36)

Question 168

The salt AgCl is ________ soluble in strong acid solution than in water.

(Multiple Choice)

4.9/5

(36)

Question 169

The solubility, in moles per liter, of Ag₂CrO₄ is 1.3 × 10^-4 M at 25°C. Calculate K_sp for this compound.

(Multiple Choice)

4.8/5

(42)

Question 170

Which of the following statements is/are true of ligands? 1) A ligand is a molecule or an ion having a lone pair of electrons that can be donated to the metal ion to form a covalent bond.2. A complex ion is a charged species consisting of a metal ion surrounded by ligands. 3) The number of ligands attached to a metal ion is called the coordination number.

(Multiple Choice)

4.7/5

(41)

Question 171

What is the molar solubility of AgCl (K_sp = 1.6 × 10^-10) in 0.0020 M sodium chloride at 25°C?

(Multiple Choice)

4.8/5

(35)

Question 172

Consider a solution of 2.0 M HCN and 1.0 M NaCN (K_a for HCN = 6.2 × 10^-10). Which of the following statements is true?

(Multiple Choice)

4.9/5

(36)

Question 173

If 30 mL of 5.0 × 10^-4 M Ca(NO₃)₂ is added to 70 mL of 2.0 × 10^-4 M NaF, will a precipitate form? (K_sp of CaF₂ = 4.0 × 10^-11)

(Multiple Choice)

4.8/5

(35)

Question 174

A 100.-mL sample of 0.10 M HCl is mixed with 50. mL of 0.10 M NH₃. What is the resulting pH? (K_b for NH₃ = 1.8 × 10^-5)

(Multiple Choice)

4.7/5

(34)

Question 175

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 K_a1 for H₂A.

(Multiple Choice)

4.8/5

(35)

Question 176

Calculate the concentration of chromate ion, CrO₄^2-, in a saturated solution of CaCrO₄ (K_sp = 7.1 × 10^-4).

(Multiple Choice)

4.8/5

(39)

Question 177

Showing 161 - 177 of 177

What combination of substances will give a buffered solution that has a pH of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K_b for NH₃ = 1.8 × 10^-5; K_b for C₅H₅N = 1.7 × 10^-9)

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 the [H⁺] after 50.00 mL of 1.00 M NaOH has been added.

Which of the following solutions will be the best buffer at a pH of 9.26? (K_a for HC₂H₃O₂ is 1.8 × 10^-5; K_b for NH₃ is 1.8 × 10^-5.)

Given the following K_sp values which statement about solubility, in moles per liter, in water is correct?

A 73.5-mL sample of 0.18 M HNO₂ (K_a = 4.0 × 10^-4) is titrated with 0.12 M NaOH. What is the pH after 25.2 mL of NaOH has been added?

The Ag⁺ ion reacts with NH₃ to form the following complex ions: AgCl (K_sp = 1.6 × 10^-10) is dissolved to its solubility limit in 10.0 M NH₃. Calculate the equilibrium concentrations of Ag⁺, Cl^-, Ag(NH₃)₂⁺, and NH₃.

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

The salt AgCl is ________ soluble in strong acid solution than in water.

The solubility, in moles per liter, of Ag₂CrO₄ is 1.3 × 10^-4 M at 25°C. Calculate K_sp for this compound.

What is the molar solubility of AgCl (K_sp = 1.6 × 10^-10) in 0.0020 M sodium chloride at 25°C?

Consider a solution of 2.0 M HCN and 1.0 M NaCN (K_a for HCN = 6.2 × 10^-10). Which of the following statements is true?

If 30 mL of 5.0 × 10^-4 M Ca(NO₃)₂ is added to 70 mL of 2.0 × 10^-4 M NaF, will a precipitate form? (K_sp of CaF₂ = 4.0 × 10^-11)

A 100.-mL sample of 0.10 M HCl is mixed with 50. mL of 0.10 M NH₃. What is the resulting pH? (K_b for NH₃ = 1.8 × 10^-5)

Calculate the concentration of chromate ion, CrO₄^2-, in a saturated solution of CaCrO₄ (K_sp = 7.1 × 10^-4).

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

What combination of substances will give a buffered solution that has a pH of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (Kb for NH3 = 1.8 × 10-5; Kb for C5H5N = 1.7 × 10-9)

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 the [H+] after 50.00 mL of 1.00 M NaOH has been added.

Which of the following solutions will be the best buffer at a pH of 9.26? (Ka for HC2H3O2 is 1.8 × 10-5; Kb for NH3 is 1.8 × 10-5.)

Given the following Ksp values which statement about solubility, in moles per liter, in water is correct?

A 73.5-mL sample of 0.18 M HNO2 (Ka = 4.0 × 10-4) is titrated with 0.12 M NaOH. What is the pH after 25.2 mL of NaOH has been added?

The Ag+ ion reacts with NH3 to form the following complex ions: AgCl (Ksp = 1.6 × 10-10) is dissolved to its solubility limit in 10.0 M NH3. Calculate the equilibrium concentrations of Ag+, Cl-, Ag(NH3)2+, and NH3.

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

The salt AgCl is ________ soluble in strong acid solution than in water.

The solubility, in moles per liter, of Ag2CrO4 is 1.3 × 10-4 M at 25°C. Calculate Ksp for this compound.

What is the molar solubility of AgCl (Ksp = 1.6 × 10-10) in 0.0020 M sodium chloride at 25°C?

Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2 × 10-10). Which of the following statements is true?

If 30 mL of 5.0 × 10-4 M Ca(NO3)2 is added to 70 mL of 2.0 × 10-4 M NaF, will a precipitate form? (Ksp of CaF2 = 4.0 × 10-11)

A 100.-mL sample of 0.10 M HCl is mixed with 50. mL of 0.10 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 × 10-5)

Calculate the concentration of chromate ion, CrO42-, in a saturated solution of CaCrO4 (Ksp = 7.1 × 10-4).

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

What combination of substances will give a buffered solution that has a pH of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K_b for NH₃ = 1.8 × 10^-5; K_b for C₅H₅N = 1.7 × 10^-9)

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 the [H⁺] after 50.00 mL of 1.00 M NaOH has been added.

Which of the following solutions will be the best buffer at a pH of 9.26? (K_a for HC₂H₃O₂ is 1.8 × 10^-5; K_b for NH₃ is 1.8 × 10^-5.)

Given the following K_sp values which statement about solubility, in moles per liter, in water is correct?

A 73.5-mL sample of 0.18 M HNO₂ (K_a = 4.0 × 10^-4) is titrated with 0.12 M NaOH. What is the pH after 25.2 mL of NaOH has been added?

The Ag⁺ ion reacts with NH₃ to form the following complex ions: AgCl (K_sp = 1.6 × 10^-10) is dissolved to its solubility limit in 10.0 M NH₃. Calculate the equilibrium concentrations of Ag⁺, Cl^-, Ag(NH₃)₂⁺, and NH₃.

The solubility, in moles per liter, of Ag₂CrO₄ is 1.3 × 10^-4 M at 25°C. Calculate K_sp for this compound.

What is the molar solubility of AgCl (K_sp = 1.6 × 10^-10) in 0.0020 M sodium chloride at 25°C?

Consider a solution of 2.0 M HCN and 1.0 M NaCN (K_a for HCN = 6.2 × 10^-10). Which of the following statements is true?

If 30 mL of 5.0 × 10^-4 M Ca(NO₃)₂ is added to 70 mL of 2.0 × 10^-4 M NaF, will a precipitate form? (K_sp of CaF₂ = 4.0 × 10^-11)

A 100.-mL sample of 0.10 M HCl is mixed with 50. mL of 0.10 M NH₃. What is the resulting pH? (K_b for NH₃ = 1.8 × 10^-5)

Calculate the concentration of chromate ion, CrO₄^2-, in a saturated solution of CaCrO₄ (K_sp = 7.1 × 10^-4).