Exhibit 15-3 Ephedrine (CS1U1B110S1U1B0HS1U1B115S1U1B0ON), a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base : CS1U1B110S1U1B0HS1U1B115S1U1B0ON (aq) + H₂ O HCS1U1B110S1U1B0HS1U1B115S1U1B0ON + (aq) + OH - (aq) Consider a 0.035 M Solution of ephedrine that has a pH of 11.33 to answer the following problem(s). -Refer to Exhibit 15-3. What is the equilibrium concentration of ephedrine, C10H15ON eq , in this 0.035 M solution?

A) 4.7×10 - 12 M B) 2.1×10 - 3 M C) 3.3×10 - 2 M D) 3.7×10 - 2 M E) 4.5×10 - 2 M A) 4.7×10 - 12 M B) 2.1×10 - 3 M C) 3.3×10 - 2 M D) 3.7×10 - 2 M E) 4.5×10 - 2 M

Which solution is most basic, given K b (NH3) = 1.8×10 - 5; K b (CH3NH2) = 3.7×10 - 4; K b (C5H5N) = 1.8×10 - 9?

A) 0.10 M NH3 B) 0.10 M C5H5N C) 0.10 M CH3NH2 D) 0.010 M NH3 E) 0.010 M C5H5N A) 0.10 M NH3 B) 0.10 M C5H5N C) 0.10 M CH3NH2 D) 0.010 M NH3 E) 0.010 M C5H5N

In the acid-base equilibrium PO4 3 - + NH ₄+ HPO3 2 - + NH₃, one conjugate acid-base pair is:

A) PO43 - , NH4+ B) NH4+ , HPO42 - C) HPO42 - , NH3 D) NH4+ , NH3 E) none of these A) PO43 - , NH4+ B) NH4+ , HPO42 - C) HPO42 - , NH3 D) NH4+ , NH3 E) none of these

The hydronium ion concentration, [H3O+], for a certain brand of beer is 3.16×10 - 5 M. What is the pOH of this aqueous solution?

A) pOH = 0.00; there can be no hydroxide ion present when hydronium ion is present. B) pOH = 3.64 C) pOH = 4.50 D) pOH = 9.50 E) pOH = 10.36 A) pOH = 0.00; there can be no hydroxide ion present when hydronium ion is present. B) pOH = 3.64 C) pOH = 4.50 D) pOH = 9.50 E) pOH = 10.36

A 0.010 M solution of the strong acid HNO3 is prepared. Which of the following statements is false ?

A) The acid is completely ionized. B) The pH of the solution is 2.0. C) The equilibrium [NO3 - ] is approximately 0.010 M. D) The aqueous NO3 - ion is a very weak base. E) The equilibrium [HNO3] is approximately 0.010 M. A) The acid is completely ionized. B) The pH of the solution is 2.0. C) The equilibrium [NO3 - ] is approximately 0.010 M. D) The aqueous NO3 - ion is a very weak base. E) The equilibrium [HNO3] is approximately 0.010 M.

The following equilibrium is established when 0.0120 M benzoic acid (C6H5COOH) is dissolved in water. C6H5COOH + H2O→C6H5COO - + H3O+ Which statement is false?

A) C6H5COOH is a weak acid. B) H2O is a weak base. C) C6H5COO - is the conjugate acid of benzoic acid. D) H3O+ is the conjugate acid of H2O. E) Hydroxide ion concentration is negligible with respect to hydrogen ion concentration. A) C6H5COOH is a weak acid. B) H2O is a weak base. C) C6H5COO - is the conjugate acid of benzoic acid. D) H3O+ is the conjugate acid of H2O. E) Hydroxide ion concentration is negligible with respect to hydrogen ion concentration.

Which of the following ammonium salts would be considered an acidic salt when dissolved in water? I. (NH4)(CH3COO) K a(CH3COOH) = 1.8×10 - 5 K b(NH3) = 1.8×10 - 5 II. NH4CN K a(HCN) = 6.2×10 - 10 K b(NH3) = 1.8×10 - 5 III. NH4Cl

A) All ammonium salts are acidic B) All ammonium salts are basic C) III only D) I and II E) II and III A) All ammonium salts are acidic B) All ammonium salts are basic C) III only D) I and II E) II and III

Exam 15: Solutions of Acids and Bases

What is the pH of a 0.25 M solution of the weak base , Aniline, C₆H₅NH₂? K _b(C₆H₅NH₂) = 4.0×10^{- 10}. You may want to complete the following table before getting started. A simplifying assumption would be valid here. C₆H₅NH₂ C₆H₅NH₃⁺ OH^{1 -} Initial Change @ equilibrium

(Multiple Choice)

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Question 121

Exhibit 15-3 Ephedrine (C₁₀H₁₅ON), a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base : C₁₀H₁₅ON (aq) + H₂ O HC₁₀H₁₅ON + (aq) + OH - (aq) Consider a 0.035 M Solution of ephedrine that has a pH of 11.33 to answer the following problem(s). -Refer to Exhibit 15-3. What is the equilibrium concentration of ephedrine, C₁₀H₁₅ON eq , in this 0.035 M solution?

(Multiple Choice)

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Question 122

Which solution is most basic, given K _b (NH₃) = 1.8×10^{- 5}; K _b(CH₃NH₂) = 3.7×10^{- 4}; K _b (C₅H₅N) = 1.8×10^{- 9}?

(Multiple Choice)

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Question 123

What is the pH of a solution prepared by dissolving 0.28 grams of KOH in 250 mL of solution? (molar mass KOH = 56.11 g/mol)

(Multiple Choice)

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Question 124

Which of the following salts is considered acidic when dissolved in water?

(Multiple Choice)

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Question 125

In the acid-base equilibrium PO₄ 3 - + NH ₄+ HPO₃ 2 - + NH₃, one conjugate acid-base pair is:

(Multiple Choice)

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Question 126

The hydronium ion concentration, [H₃O⁺], for a certain brand of beer is 3.16×10^{- 5} M. What is the pOH of this aqueous solution?

(Multiple Choice)

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Question 127

Select the best choice given the three following descriptions: I. A base is a proton acceptor. II. A base is a source of hydroxide ions in water. III. A base is an electron pair donor.

(Multiple Choice)

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Question 128

What is the pH of a 0.45 M solution of sodium acetate, CH₃COO^-Na⁺? K _a(CH₃COOH) = 1.8×10^{- 5}. You may want to complete the following table before getting started. A simplifying assumption would be valid here. CH₃COO^-Na⁺ CH₃COOH OH^{1 -} Initial Change @ equilibrium

(Multiple Choice)

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Question 129

A 0.010 M solution of the strong acid HNO₃ is prepared. Which of the following statements is false ?

(Multiple Choice)

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Question 130

Exhibit 15-6 Consider an aqueous 0.25 M solution of NaCN to answer the following question(s). -Refer to Exhibit 15-6. What is the pH of this 0.25 M solution of NaCN?

(Multiple Choice)

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Question 131

The following equilibrium is established when 0.0120 M benzoic acid (C₆H₅COOH) is dissolved in water. C₆H₅COOH + H₂O→C₆H₅COO^- + H₃O⁺ Which statement is false?

(Multiple Choice)

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Question 132

What is the pH of a 0.20 M solution of the weak base ephedrine ( K _b = 1.4×10^{- 4})?

(Multiple Choice)

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Question 133

Which of the following ammonium salts would be considered an acidic salt when dissolved in water? I. (NH₄)(CH₃COO) K _a(CH₃COOH) = 1.8×10^{- 5} K _b(NH₃) = 1.8×10^{- 5} II. NH₄CN K _a(HCN) = 6.2×10^{- 10} K _b(NH₃) = 1.8×10^{- 5} III. NH₄Cl

(Multiple Choice)

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Question 134

After completing the following unfinished Base Ionization table, what is the order of increasing base strength ? Base K _b p K _b Bicarbonate ion, HCO₃^- 2.2×10^{- 8} Pyridine, C₅H₅N 8.77 Acetate ion, CH₃COO^- 5.7×10^{- 10}

(Multiple Choice)

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Question 135

Which of the following salts is(are) considered acidic when dissolved in water? I. NaCN II. (CH₃NH₃)⁺NO₃^- III. KF

(Multiple Choice)

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Question 136

Acetic acid has K _a = 1.8×10^{- 5}. A solution of 0.10 M sodium acetate has a pH of:

(Multiple Choice)

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Question 137

When comparing Bronsted-Lowery acid strengths, which one of the items listed below is falsely labeled?

(Multiple Choice)

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Question 138

Which compound is a strong acid in water?

(Multiple Choice)

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Question 139

Hypochlorous acid (HClO) has an acid ionization constant, K _a, equal to 2.9×10^{- 8}. What is the pH of a 0.20 M aqueous solution of hypochlorous acid?

(Multiple Choice)

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Question 140

Showing 121 - 140 of 179

Exam 15: Solutions of Acids and Bases

What is the pH of a 0.25 M solution of the weak base , Aniline, C6H5NH2? K b(C6H5NH2) = 4.0×10 - 10. You may want to complete the following table before getting started. A simplifying assumption would be valid here. C6H5NH2 C6H5NH3+ OH1 - Initial Change @ equilibrium

Which solution is most basic, given K b (NH3) = 1.8×10 - 5; K b (CH3NH2) = 3.7×10 - 4; K b (C5H5N) = 1.8×10 - 9?

What is the pH of a solution prepared by dissolving 0.28 grams of KOH in 250 mL of solution? (molar mass KOH = 56.11 g/mol)

Which of the following salts is considered acidic when dissolved in water?

In the acid-base equilibrium PO4 3 - + NH ₄+ HPO3 2 - + NH₃, one conjugate acid-base pair is:

The hydronium ion concentration, [H3O+], for a certain brand of beer is 3.16×10 - 5 M. What is the pOH of this aqueous solution?

Select the best choice given the three following descriptions: I. A base is a proton acceptor. II. A base is a source of hydroxide ions in water. III. A base is an electron pair donor.

What is the pH of a 0.45 M solution of sodium acetate, CH3COO - Na+? K a(CH3COOH) = 1.8×10 - 5. You may want to complete the following table before getting started. A simplifying assumption would be valid here. CH3COO - Na+ CH3COOH OH1 - Initial Change @ equilibrium

A 0.010 M solution of the strong acid HNO3 is prepared. Which of the following statements is false ?

Exhibit 15-6 Consider an aqueous 0.25 M solution of NaCN to answer the following question(s). -Refer to Exhibit 15-6. What is the pH of this 0.25 M solution of NaCN?

The following equilibrium is established when 0.0120 M benzoic acid (C6H5COOH) is dissolved in water. C6H5COOH + H2O→C6H5COO - + H3O+ Which statement is false?

What is the pH of a 0.20 M solution of the weak base ephedrine ( K b = 1.4×10 - 4)?

Which of the following ammonium salts would be considered an acidic salt when dissolved in water? I. (NH4)(CH3COO) K a(CH3COOH) = 1.8×10 - 5 K b(NH3) = 1.8×10 - 5 II. NH4CN K a(HCN) = 6.2×10 - 10 K b(NH3) = 1.8×10 - 5 III. NH4Cl

After completing the following unfinished Base Ionization table, what is the order of increasing base strength ? Base K b p K b Bicarbonate ion, HCO3 - 2.2×10 - 8 Pyridine, C5H5N 8.77 Acetate ion, CH3COO - 5.7×10 - 10

Which of the following salts is(are) considered acidic when dissolved in water? I. NaCN II. (CH3NH3)+NO3 - III. KF

Acetic acid has K a = 1.8×10 - 5. A solution of 0.10 M sodium acetate has a pH of:

When comparing Bronsted-Lowery acid strengths, which one of the items listed below is falsely labeled?

Which compound is a strong acid in water?

Hypochlorous acid (HClO) has an acid ionization constant, K a, equal to 2.9×10 - 8. What is the pH of a 0.20 M aqueous solution of hypochlorous acid?

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Which solution is most basic, given K _b (NH₃) = 1.8×10^{- 5}; K _b(CH₃NH₂) = 3.7×10^{- 4}; K _b (C₅H₅N) = 1.8×10^{- 9}?

In the acid-base equilibrium PO₄ 3 - + NH ₄+ HPO₃ 2 - + NH₃, one conjugate acid-base pair is:

The hydronium ion concentration, [H₃O⁺], for a certain brand of beer is 3.16×10^{- 5} M. What is the pOH of this aqueous solution?

What is the pH of a 0.45 M solution of sodium acetate, CH₃COO^-Na⁺? K _a(CH₃COOH) = 1.8×10^{- 5}. You may want to complete the following table before getting started. A simplifying assumption would be valid here. CH₃COO^-Na⁺ CH₃COOH OH^{1 -} Initial Change @ equilibrium

A 0.010 M solution of the strong acid HNO₃ is prepared. Which of the following statements is false ?

The following equilibrium is established when 0.0120 M benzoic acid (C₆H₅COOH) is dissolved in water. C₆H₅COOH + H₂O→C₆H₅COO^- + H₃O⁺ Which statement is false?

What is the pH of a 0.20 M solution of the weak base ephedrine ( K _b = 1.4×10^{- 4})?

Which of the following ammonium salts would be considered an acidic salt when dissolved in water? I. (NH₄)(CH₃COO) K _a(CH₃COOH) = 1.8×10^{- 5} K _b(NH₃) = 1.8×10^{- 5} II. NH₄CN K _a(HCN) = 6.2×10^{- 10} K _b(NH₃) = 1.8×10^{- 5} III. NH₄Cl

After completing the following unfinished Base Ionization table, what is the order of increasing base strength ? Base K _b p K _b Bicarbonate ion, HCO₃^- 2.2×10^{- 8} Pyridine, C₅H₅N 8.77 Acetate ion, CH₃COO^- 5.7×10^{- 10}

Which of the following salts is(are) considered acidic when dissolved in water? I. NaCN II. (CH₃NH₃)⁺NO₃^- III. KF

Acetic acid has K _a = 1.8×10^{- 5}. A solution of 0.10 M sodium acetate has a pH of:

Hypochlorous acid (HClO) has an acid ionization constant, K _a, equal to 2.9×10^{- 8}. What is the pH of a 0.20 M aqueous solution of hypochlorous acid?