The complete reaction of an acid and base is as follows. HNO3(aq) + LiOH(aq) ? H2O( $\ell$ ) + LiNO3(aq) What is the equilibrium constant for the net ionic reaction at 25 °C?

A) 1.01 × 10-14 B) 1.01 × 10-7 C) 1.01 × 107 D) 1.01 × 1014 E) more information required A) 1.01 × 10-14 B) 1.01 × 10-7 C) 1.01 × 107 D) 1.01 × 1014 E) more information required

Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 × 10-4 Formic acid, HCHO2, 1.7 × 10-4 Lactic acid, HC3H5O3, 1.3 × 10-4 Propionic acid, HC3H5O2, 1.3 × 10-5 Benzoic acid, HC7H5O2, 6.3 × 10-5 Given initially equimolar solutions of each weak acid, which solution will have the highest pH once equilibrium is established?

A) HOCN B) HC7H5O2 C) HC3H5O2 D) HC3H5O3 E) HCHO2 A) HOCN B) HC7H5O2 C) HC3H5O2 D) HC3H5O3 E) HCHO2

What is the hydroxide-ion concentration of a 0.190 M sodium oxalate (Na2C2O4) solution? For oxalic acid (H2C2O4), Ka1 = 5.6 × 10-2 and Ka2 = 5.1 × 10-5. (Kw = 1.01 × 10-14)

A) 6.1 × 10-6 M B) 1.0 × 10-7 M C) 7.9 × 10-2 M D) 3.1 × 10-3 M E) 1.8 × 10-7 M A) 6.1 × 10-6 M B) 1.0 × 10-7 M C) 7.9 × 10-2 M D) 3.1 × 10-3 M E) 1.8 × 10-7 M

What is the pH of the solution that results from mixing 75 mL of 0.50 M NH3(aq) and 75 mL of 0.50 HCl(aq) at 25 °C? (Kb for NH3 = 1.8 × 10-5)

A) 0.60 B) 2.67 C) 4.74 D) 4.93 E) 9.26 A) 0.60 B) 2.67 C) 4.74 D) 4.93 E) 9.26

The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.09. What is the Kb of this base?

A) 8.0 × 10-10 B) 1.5 × 10-9 C) 9.0 × 10-6 D) 1.6 × 10-5 E) 1.2 × 10-5 A) 8.0 × 10-10 B) 1.5 × 10-9 C) 9.0 × 10-6 D) 1.6 × 10-5 E) 1.2 × 10-5

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

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The complete reaction of an acid and base is as follows. HNO₃(aq) + LiOH(aq) ? H₂O( $\ell$ ) + LiNO₃(aq) What is the equilibrium constant for the net ionic reaction at 25 °C?

(Multiple Choice)

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Question 21

Which of the following species cannot act as a Lewis base?

(Multiple Choice)

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Question 22

Consider the K_a values for the following acids: Cyanic acid, HOCN, 3.5 × 10^-4Formic acid, HCHO₂, 1.7 × 10^-4Lactic acid, HC₃H₅O₃, 1.3 × 10^-4Propionic acid, HC₃H₅O₂, 1.3 × 10^-5 Benzoic acid, HC₇H₅O₂, 6.3 × 10^-5 Given initially equimolar solutions of each weak acid, which solution will have the highest pH once equilibrium is established?

(Multiple Choice)

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Question 23

What is the hydroxide-ion concentration of a 0.190 M sodium oxalate (Na₂C₂O₄) solution? For oxalic acid (H₂C₂O₄), K_a1 = 5.6 × 10^-2 and K_a2 = 5.1 × 10^-5. (K_w = 1.01 × 10^-14)

(Multiple Choice)

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Question 24

What is the pH of the solution that results from mixing 75 mL of 0.50 M NH₃(aq) and 75 mL of 0.50 HCl(aq) at 25 °C? (K_b for NH₃ = 1.8 × 10^-5)

(Multiple Choice)

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Question 25

The equilibrium constant, K_a,for a monoprotic acid (benzoic acid) is 6.3 × 10^-5. Which of the following is the correct value of K_b for the benzoate ion, the conjugate base of benzoic acid?

(Multiple Choice)

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Question 26

According to the Brønsted-Lowry definition, a base

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Question 27

The H₃O⁺ concentration of a solution is 5.9 × 10^-6 M. What is the pH of the solution?

(Multiple Choice)

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Question 28

Which of the following does not behave as an amphiprotic species in water?

(Multiple Choice)

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Question 29

What is the equilibrium pH of an initially 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25°C (K_a = $7.8 \times 10 ^ { - 5 }$ )?

(Multiple Choice)

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Question 30

Which of the following statements is/are consistent with the Brønsted-Lowry concept of acids and bases? 1.A conjugate acid–base pair consists of two species that may differ by one proton. 2. A Brønsted–Lowry base is defined as a hydroxide ion donor. 3.Brønsted–Lowry acid-base reactions are restricted to only aqueous solutions.

(Multiple Choice)

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Question 31

A molecule that can behave as either a Brønsted-Lowry acid or base is termed ________.

(Short Answer)

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Question 32

Which of the following species is the strongest acid in an aqueous solution?

(Multiple Choice)

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Question 33

The pH of a solution at 25 °C in which [OH^-] = 3.9 × 10^-5 M is _____. (K_w = 1.01 × 10^-14)

(Multiple Choice)

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Question 34

A Brønsted-Lowry base is defined as a hydroxide ion donor.

(Essay)

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Question 35

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 8.0 × 10^-4 M. What is the acid-ionization constant, K_a, for this acid?

(Multiple Choice)

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Question 36

Which acid-base reaction results in acidic solution?

(Multiple Choice)

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Question 37

Calculate the pH of a 0.09 M solution of ascorbic acid (K_a1= 7.9 × 10^-5; K_a2 is 1.6 × 10^-12).

(Multiple Choice)

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Question 38

The pH of aqueous 0.10 M pyridine (C₅H₅N) ion is 9.09. What is the K_b of this base?

(Multiple Choice)

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Question 39

A conjugate acid-base pair consists of two species that may differ by one proton.

(Essay)

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Question 40

Showing 21 - 40 of 97

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

The complete reaction of an acid and base is as follows. HNO3(aq) + LiOH(aq) ? H2O( ℓ\ellℓ ) + LiNO3(aq) What is the equilibrium constant for the net ionic reaction at 25 °C?

Which of the following species cannot act as a Lewis base?

What is the hydroxide-ion concentration of a 0.190 M sodium oxalate (Na2C2O4) solution? For oxalic acid (H2C2O4), Ka1 = 5.6 × 10-2 and Ka2 = 5.1 × 10-5. (Kw = 1.01 × 10-14)

What is the pH of the solution that results from mixing 75 mL of 0.50 M NH3(aq) and 75 mL of 0.50 HCl(aq) at 25 °C? (Kb for NH3 = 1.8 × 10-5)

The equilibrium constant, Ka,for a monoprotic acid (benzoic acid) is 6.3 × 10-5. Which of the following is the correct value of Kb for the benzoate ion, the conjugate base of benzoic acid?

According to the Brønsted-Lowry definition, a base

The H3O+ concentration of a solution is 5.9 × 10-6 M. What is the pH of the solution?

Which of the following does not behave as an amphiprotic species in water?

What is the equilibrium pH of an initially 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25°C (Ka = 7.8×10−57.8 \times 10 ^ { - 5 }7.8×10−5 )?

A molecule that can behave as either a Brønsted-Lowry acid or base is termed ________.

Which of the following species is the strongest acid in an aqueous solution?

The pH of a solution at 25 °C in which [OH-] = 3.9 × 10-5 M is _____. (Kw = 1.01 × 10-14)

A Brønsted-Lowry base is defined as a hydroxide ion donor.

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 8.0 × 10-4 M. What is the acid-ionization constant, Ka, for this acid?

Which acid-base reaction results in acidic solution?

Calculate the pH of a 0.09 M solution of ascorbic acid (Ka1 = 7.9 × 10-5; Ka2 is 1.6 × 10-12).

The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.09. What is the Kb of this base?

A conjugate acid-base pair consists of two species that may differ by one proton.

Basic Concepts of Chemistry

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Principles of Chemical Reactivity: Equilibria

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Principles of Chemical Reactivity: Entropy and Free Energy

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The complete reaction of an acid and base is as follows. HNO₃(aq) + LiOH(aq) ? H₂O( $\ell$ ) + LiNO₃(aq) What is the equilibrium constant for the net ionic reaction at 25 °C?

What is the hydroxide-ion concentration of a 0.190 M sodium oxalate (Na₂C₂O₄) solution? For oxalic acid (H₂C₂O₄), K_a1 = 5.6 × 10^-2 and K_a2 = 5.1 × 10^-5. (K_w = 1.01 × 10^-14)

What is the pH of the solution that results from mixing 75 mL of 0.50 M NH₃(aq) and 75 mL of 0.50 HCl(aq) at 25 °C? (K_b for NH₃ = 1.8 × 10^-5)

The equilibrium constant, K_a,for a monoprotic acid (benzoic acid) is 6.3 × 10^-5. Which of the following is the correct value of K_b for the benzoate ion, the conjugate base of benzoic acid?

The H₃O⁺ concentration of a solution is 5.9 × 10^-6 M. What is the pH of the solution?

What is the equilibrium pH of an initially 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25°C (K_a = $7.8 \times 10 ^ { - 5 }$ )?

The pH of a solution at 25 °C in which [OH^-] = 3.9 × 10^-5 M is _____. (K_w = 1.01 × 10^-14)

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 8.0 × 10^-4 M. What is the acid-ionization constant, K_a, for this acid?

Calculate the pH of a 0.09 M solution of ascorbic acid (K_a1= 7.9 × 10^-5; K_a2 is 1.6 × 10^-12).

The pH of aqueous 0.10 M pyridine (C₅H₅N) ion is 9.09. What is the K_b of this base?