Identify the Lewis base in the following reaction: SO2 (g) +H2 O(l) $\rightarrow$ H2 SO3 (aq)

A) SO2 B) H2O C) H2SO3 D) None of these is a base. E) All of these are bases. A) SO2 B) H2O C) H2SO3 D) None of these is a base. E) All of these are bases.

The solubility product for Ag3PO4 is written as _______ , where s is the molar solubility.

A) Ksp = s2 B) Ksp =4S3 C) Ksp = 27s4 D) Ksp = 3S3 E) Ksp =3s4 A) Ksp = s2 B) Ksp =4S3 C) Ksp = 27s4 D) Ksp = 3S3 E) Ksp =3s4

Identify the Lewis base in the following reaction: PH3 (aq) +H+(aq) $\rightarrow$ PH4+ (aq)

A) PH4+ B) H+ C) PH3 D) None of these is a base. E) All of these are bases. A) PH4+ B) H+ C) PH3 D) None of these is a base. E) All of these are bases.

Exam 16: Additional Aqueous Equilibria Chemistry and the Oceans

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When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates.This phenomenon is called

(Multiple Choice)

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Question 41

A Lewis acid is any species capable of _______ an electron pair.

(Multiple Choice)

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Question 42

What are the characteristics of a pH indicator? I.It is usually a conjugate acid-base pair. II)It has different characteristic colors in protonated and unprotonated forms. III)It changes color when the pH is near its pK_a.

(Multiple Choice)

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Question 43

Identify the Lewis base in the following reaction: SO₂ (g) +H₂ O(l) $\rightarrow$ H₂ SO₃ (aq)

(Multiple Choice)

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Question 44

Acid-base indicators change color

(Multiple Choice)

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Question 45

A 200.0 mL solution of 0.40 M ammonium chloride was titrated with 0.80M sodium hydroxide.What was the pH of the solution after 50.0 mL of the NaOH solution were added? The K_b of ammonia is 1.76 *10^-5.

(Multiple Choice)

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Question 46

K_sp for lead(II) hydroxide is 1.4*10^-20 at 25°C.What is the molar solubility of (PbOH)₂ in A) pure water and B) a buffer solution with a pH= 11.50?

(Essay)

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Question 47

Which solution below would be the best choice for preparing a buffer with a pH=8.0?

(Multiple Choice)

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Question 48

What is the equilibrium concentration of Cu⁺(aq) in a solution that is initially 0.0200 M solution in CuNO₃ and 0.450 M HCl(aq)? Cu⁺(aq) + 3 Cl^-(aq) fi CuCl ²^-(aq) K_f * 5.0 *10⁵

(Multiple Choice)

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Question 49

Research with biochemical systems commonly requires buffers because

(Multiple Choice)

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Question 50

The Yucca Mountain repository in Nevada, which is intended for the long-term storage of nuclear waste, has long been mired in controversy.One ongoing concern is whether the stainless-steel alloy containers could be corroded by salts such as calcium fluoride.If the calcium ion concentration in water inside Yucca Mountain is 1.2510^-3 M, what is the maximum possible concentration of fluoride ion in this water? Assume calcium fluoride K_sp = 2.2 10^-10 at the temperatures inside the nuclear waste depository.

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Question 51

What is the pH of a solution prepared by dissolving 4.50 g sodium dihydrogen borate (83.82g/mol) in 650 mL of a 0.0725 M boric acid? The K_a of boric acid is 5.4 *10^-10.Ignore any volume change.

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Question 52

Glycolic acid, which is a monoprotic acid and a constituent in sugarcane, has a pK_a of 3.9.A 25.0 mL solution of glycolic acid is titrated to the equivalence point with 35.8 mL of 0.020 M sodium hydroxide solution.What is the pH of the resulting solution at the equivalence point?

(Short Answer)

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Question 53

Suppose a 1.0 L solution containing 0.20 moles of morphine is titrated with 0.40 M HCl.The pH at the equivalence point is 4.543.What is the K_b of morphine?

(Multiple Choice)

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Question 54

Which of the following species is a Lewis base?

(Multiple Choice)

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Question 55

The solubility product for Ag₃PO₄ is written as _______ , where s is the molar solubility.

(Multiple Choice)

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Question 56

At what point in the following titration curve for a weak acid being titrated with a strong base is the pH equal to the pK_a of the acid? The x-axis scale goes from 0.0 mL to 20.0 mL.The sharp rise is at 10.0 mL.

(Multiple Choice)

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Question 57

Identify the Lewis base in the following reaction: PH₃ (aq) +H⁺(aq) $\rightarrow$ PH₄⁺ (aq)

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Question 58

A 25.00 mL sample of a phosphoric acid solution was titrated to completion with 37.04 mL of 0.1107 M sodium hydroxide.What was the concentration of the phosphoric acid?

(Multiple Choice)

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Question 59

Bromocresol green is yellow in its acidic form and blue in its basic form.When is it green?

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Question 60

Showing 41 - 60 of 114

Exam 16: Additional Aqueous Equilibria Chemistry and the Oceans

When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates.This phenomenon is called

A Lewis acid is any species capable of _______ an electron pair.

What are the characteristics of a pH indicator? I.It is usually a conjugate acid-base pair. II)It has different characteristic colors in protonated and unprotonated forms. III)It changes color when the pH is near its pKa.

Identify the Lewis base in the following reaction: SO2 (g) +H2 O(l) →\rightarrow→ H2 SO3 (aq)

Acid-base indicators change color

A 200.0 mL solution of 0.40 M ammonium chloride was titrated with 0.80M sodium hydroxide.What was the pH of the solution after 50.0 mL of the NaOH solution were added? The Kb of ammonia is 1.76 *10-5.

Ksp for lead(II) hydroxide is 1.4*10-20 at 25°C.What is the molar solubility of (PbOH)2 in A) pure water and B) a buffer solution with a pH= 11.50?

Which solution below would be the best choice for preparing a buffer with a pH=8.0?

What is the equilibrium concentration of Cu+(aq) in a solution that is initially 0.0200 M solution in CuNO3 and 0.450 M HCl(aq)? Cu+(aq) + 3 Cl-(aq) fi CuCl 2-(aq) Kf * 5.0 *105

Research with biochemical systems commonly requires buffers because

What is the pH of a solution prepared by dissolving 4.50 g sodium dihydrogen borate (83.82g/mol) in 650 mL of a 0.0725 M boric acid? The Ka of boric acid is 5.4 *10-10.Ignore any volume change.

Glycolic acid, which is a monoprotic acid and a constituent in sugarcane, has a pKa of 3.9.A 25.0 mL solution of glycolic acid is titrated to the equivalence point with 35.8 mL of 0.020 M sodium hydroxide solution.What is the pH of the resulting solution at the equivalence point?

Suppose a 1.0 L solution containing 0.20 moles of morphine is titrated with 0.40 M HCl.The pH at the equivalence point is 4.543.What is the Kb of morphine?

Which of the following species is a Lewis base?

The solubility product for Ag3PO4 is written as _______ , where s is the molar solubility.

At what point in the following titration curve for a weak acid being titrated with a strong base is the pH equal to the pKa of the acid? The x-axis scale goes from 0.0 mL to 20.0 mL.The sharp rise is at 10.0 mL.

Identify the Lewis base in the following reaction: PH3 (aq) +H+(aq) →\rightarrow→ PH4+ (aq)

A 25.00 mL sample of a phosphoric acid solution was titrated to completion with 37.04 mL of 0.1107 M sodium hydroxide.What was the concentration of the phosphoric acid?

Bromocresol green is yellow in its acidic form and blue in its basic form.When is it green?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

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What are the characteristics of a pH indicator? I.It is usually a conjugate acid-base pair. II)It has different characteristic colors in protonated and unprotonated forms. III)It changes color when the pH is near its pK_a.

Identify the Lewis base in the following reaction: SO₂ (g) +H₂ O(l) $\rightarrow$ H₂ SO₃ (aq)

A 200.0 mL solution of 0.40 M ammonium chloride was titrated with 0.80M sodium hydroxide.What was the pH of the solution after 50.0 mL of the NaOH solution were added? The K_b of ammonia is 1.76 *10^-5.

K_sp for lead(II) hydroxide is 1.4*10^-20 at 25°C.What is the molar solubility of (PbOH)₂ in A) pure water and B) a buffer solution with a pH= 11.50?

What is the equilibrium concentration of Cu⁺(aq) in a solution that is initially 0.0200 M solution in CuNO₃ and 0.450 M HCl(aq)? Cu⁺(aq) + 3 Cl^-(aq) fi CuCl ²^-(aq) K_f * 5.0 *10⁵

What is the pH of a solution prepared by dissolving 4.50 g sodium dihydrogen borate (83.82g/mol) in 650 mL of a 0.0725 M boric acid? The K_a of boric acid is 5.4 *10^-10.Ignore any volume change.

Glycolic acid, which is a monoprotic acid and a constituent in sugarcane, has a pK_a of 3.9.A 25.0 mL solution of glycolic acid is titrated to the equivalence point with 35.8 mL of 0.020 M sodium hydroxide solution.What is the pH of the resulting solution at the equivalence point?

Suppose a 1.0 L solution containing 0.20 moles of morphine is titrated with 0.40 M HCl.The pH at the equivalence point is 4.543.What is the K_b of morphine?

The solubility product for Ag₃PO₄ is written as _______ , where s is the molar solubility.

At what point in the following titration curve for a weak acid being titrated with a strong base is the pH equal to the pK_a of the acid? The x-axis scale goes from 0.0 mL to 20.0 mL.The sharp rise is at 10.0 mL.

Identify the Lewis base in the following reaction: PH₃ (aq) +H⁺(aq) $\rightarrow$ PH₄⁺ (aq)