Calculate the pH of a 0.020 M carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

A) 1.70 B) 4.03 C) 6.37 D) 10.25 A) 1.70 B) 4.03 C) 6.37 D) 10.25 B

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent AS1U1P1yS1S1P0S1U1P1-S1S1P0 ions;gray spheres represent MS1U1P1x+S1S1P0 ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a basic salt?

A) (1) B) (2) C) (3) D) None of these A) (1) B) (2) C) (3) D) None of these

What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

A) 3.6 × 10-3 M B) 1.3 × 10-4 M C) 1.3 × 10-5 M D) 1.0 × 10-11 M A) 3.6 × 10-3 M B) 1.3 × 10-4 M C) 1.3 × 10-5 M D) 1.0 × 10-11 M

Calculate the pH of a 0.100 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

A) 2.87 B) 5.13 C) 8.87 D) 11.13 A) 2.87 B) 5.13 C) 8.87 D) 11.13

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent AS1U1P1yS1S1P0S1U1P1-S1S1P0 ions;gray spheres represent MS1U1P1x+S1S1P0 ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a neutral salt?

A) (1) B) (2) C) (3) D) None of these A) (1) B) (2) C) (3) D) None of these

Exam 15: Aqueous Equilibria: Acids and Bases

Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃(aq),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7and K_a2 = 5.6 × 10^-11.

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

BF₃ and NH₃ undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

Which Br∅nsted-Lowry base has the strongest conjugate acid?

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

What is the approximate pH of a solution X that gives the following responses with the indicators shown?

(Multiple Choice)

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Question 4

A solution with a hydrogen ion concentration of 3.25 × 10^-2 M is and has a hydroxide concentration of .

(Multiple Choice)

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Question 5

In the aquation reaction Co²⁺ + 6 H₂O → [Co(H₂O)₆]²⁺,the Lewis acid is and the Lewis base is .

(Short Answer)

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Question 6

Which of the following should have the lowest bond strength?

(Multiple Choice)

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Question 7

What are the Br∅nsted-Lowry acids in the following chemical reaction? HBr(sol)+ CH₃COOH(sol)⇌ CH₃C(OH)₂⁺(sol)+ Br^-(sol)

(Multiple Choice)

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Question 8

What is the pH of a solution made by mixing 100.00 mL of 0.20 M HCl with 50.00 mL of 0.10 M HCl? Assume that the volumes are additive.

(Multiple Choice)

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Question 9

What is the hydronium ion concentration of a 0.100 M acetic acid solution with a K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH₃CO₂H(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CH₃CO₂^-(aq).

(Multiple Choice)

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Question 10

Which of the following is a weak diprotic acids?

(Multiple Choice)

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Question 11

If an equal number of moles of the weak acid HF and the strong base KOH are added to water,is the resulting solution acidic,basic,or neutral?

(Multiple Choice)

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Question 12

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent A^y^- ions;gray spheres represent M^x+ ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a basic salt?

(Multiple Choice)

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Question 13

What is the selenide ion concentration [Se^2-] for a 0.100 M H₂Se solution that has the stepwise dissociation constants of K_a1 = 1.3 × 10^-4 and K_a2 = 1.0 × 10^-11?

(Multiple Choice)

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Question 14

Which one of the following salts,when dissolved in water,produces the solution with a pH closest to 7.00?

(Multiple Choice)

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Question 15

Calculate the pH of a 0.100 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-5.

(Multiple Choice)

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Question 16

Determine the acid dissociation constant for a 0.010 M nitrous acid solution that has a pH of 2.70.Nitrous acid is a weak monoprotic acid and the equilibrium equation of interest is HNO₂(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ NO₂^-(aq).

(Multiple Choice)

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Question 17

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent A^y^- ions;gray spheres represent M^x+ ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a neutral salt?

(Multiple Choice)

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Question 18

Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.

(Multiple Choice)

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Question 19

How many grams of pyridine are there in 100 mL of an aqueous solution that has a pH of 9.00? The K_b for pyridine is 1.9 × 10^-9 and the equation of interest is C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq).

(Multiple Choice)

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Question 20

Showing 1 - 20 of 231

Exam 15: Aqueous Equilibria: Acids and Bases

Calculate the pH of a 0.020 M carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

BF3 and NH3 undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

Which Br∅nsted-Lowry base has the strongest conjugate acid?

What is the approximate pH of a solution X that gives the following responses with the indicators shown?

A solution with a hydrogen ion concentration of 3.25 × 10-2 M is ________ and has a hydroxide concentration of ________.

In the aquation reaction Co2+ + 6 H2O → [Co(H2O)6]2+,the Lewis acid is ________ and the Lewis base is ________.

Which of the following should have the lowest bond strength?

What are the Br∅nsted-Lowry acids in the following chemical reaction? HBr(sol)+ CH3COOH(sol)⇌ CH3C(OH)2+(sol)+ Br-(sol)

What is the pH of a solution made by mixing 100.00 mL of 0.20 M HCl with 50.00 mL of 0.10 M HCl? Assume that the volumes are additive.

What is the hydronium ion concentration of a 0.100 M acetic acid solution with a Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq)+ H2O(l)⇌ H3O+(aq)+ CH3CO2-(aq).

Which of the following is a weak diprotic acids?

If an equal number of moles of the weak acid HF and the strong base KOH are added to water,is the resulting solution acidic,basic,or neutral?

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent Ay- ions;gray spheres represent Mx+ ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a basic salt?

What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

Which one of the following salts,when dissolved in water,produces the solution with a pH closest to 7.00?

Calculate the pH of a 0.100 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Determine the acid dissociation constant for a 0.010 M nitrous acid solution that has a pH of 2.70.Nitrous acid is a weak monoprotic acid and the equilibrium equation of interest is HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq).

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent Ay- ions;gray spheres represent Mx+ ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a neutral salt?

Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.

How many grams of pyridine are there in 100 mL of an aqueous solution that has a pH of 9.00? The Kb for pyridine is 1.9 × 10-9 and the equation of interest is C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq).

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Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃(aq),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7and K_a2 = 5.6 × 10^-11.

BF₃ and NH₃ undergo a Lewis acid-base reaction forming an adduct.Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction;what is the Lewis acid and the Lewis base?

A solution with a hydrogen ion concentration of 3.25 × 10^-2 M is and has a hydroxide concentration of .

In the aquation reaction Co²⁺ + 6 H₂O → [Co(H₂O)₆]²⁺,the Lewis acid is and the Lewis base is .

What are the Br∅nsted-Lowry acids in the following chemical reaction? HBr(sol)+ CH₃COOH(sol)⇌ CH₃C(OH)₂⁺(sol)+ Br^-(sol)

What is the hydronium ion concentration of a 0.100 M acetic acid solution with a K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH₃CO₂H(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CH₃CO₂^-(aq).

The following pictures represent solutions of three salts MA;water molecules have been omitted for clarity.Dotted spheres represent A^y^- ions;gray spheres represent M^x+ ions;black spheres represent oxygen atoms;and unshaded spheres represent hydrogen atoms. -Which picture represents a basic salt?

What is the selenide ion concentration [Se^2-] for a 0.100 M H₂Se solution that has the stepwise dissociation constants of K_a1 = 1.3 × 10^-4 and K_a2 = 1.0 × 10^-11?

Calculate the pH of a 0.100 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-5.

Determine the acid dissociation constant for a 0.010 M nitrous acid solution that has a pH of 2.70.Nitrous acid is a weak monoprotic acid and the equilibrium equation of interest is HNO₂(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ NO₂^-(aq).

How many grams of pyridine are there in 100 mL of an aqueous solution that has a pH of 9.00? The K_b for pyridine is 1.9 × 10^-9 and the equation of interest is C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq).