Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH→C6H5NH3+ + HCOO - Which of the following is a conjugate acid-base pair?

A) C6H5NH2 and HCO2H B) HCOOH and C6H5NH3+ C) HCOO - and C6H5NH2 D) C6H5NH3+ and C6H5NH2 E) C6H5NH3+ and HCOO - A) C6H5NH2 and HCO2H B) HCOOH and C6H5NH3+ C) HCOO - and C6H5NH2 D) C6H5NH3+ and C6H5NH2 E) C6H5NH3+ and HCOO - D

Consider adding NaClO4 to a basic solution. Which statement below is true?

A) NaClO4 is an acidic salt and the pH of the resulting solution rises. B) NaClO4 is an acidic salt and the pH of the resulting solution lowers. C) NaClO4 is a basic salt and the pH of the resulting solution rises. D) NaClO4 is a basic salt and the pH of the resulting solution lowers. E) NaClO4 is a neutral salt and the pH of the resulting solution does not change. A) NaClO4 is an acidic salt and the pH of the resulting solution rises. B) NaClO4 is an acidic salt and the pH of the resulting solution lowers. C) NaClO4 is a basic salt and the pH of the resulting solution rises. D) NaClO4 is a basic salt and the pH of the resulting solution lowers. E) NaClO4 is a neutral salt and the pH of the resulting solution does not change.

If the reaction below proceeds, which of the following is true? NH3 + C2H5OH→NH2 - + C2H5OH2+

A) C2H5OH is an acid. B) NH2 - is the conjugate base of NH3. C) NH3 is a base. D) C2H5OH2+ is a base. E) none of these A) C2H5OH is an acid. B) NH2 - is the conjugate base of NH3. C) NH3 is a base. D) C2H5OH2+ is a base. E) none of these

In the reaction: N₂H4 (aq) + H₂ O N₂H5 + (aq) + OH - (aq)

A) N2H4 and N2H5+ act as acids. B) H2O and N2H5+ act as acids. C) N2H5+ and OH - act as acids. D) only OH - acts as a base. E) none of these. A) N2H4 and N2H5+ act as acids. B) H2O and N2H5+ act as acids. C) N2H5+ and OH - act as acids. D) only OH - acts as a base. E) none of these.

A nitric acid (HNO3) solution is 16.2 M. Which of the following is correct?

A) pH = 1.21 B) pH = 2.78 C) pOH = 15.21 D) [OH - ] = 1.62×1015 E) must know K a A) pH = 1.21 B) pH = 2.78 C) pOH = 15.21 D) [OH - ] = 1.62×1015 E) must know K a

Exam 15: Solutions of Acids and Bases

When 20.0 grams of a water soluble salt dissolves in 1.0 L of pure water the pH was found to be less than seven. Which of the following statements about the salt is most probable?

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Question 1

Correct Answer:

Verified

Consider the following Bronsted-Lowry acid-base reaction: C₆H₅NH₂ + HCOOH→C₆H₅NH₃⁺ + HCOO^- Which of the following is a conjugate acid-base pair?

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Question 2

Correct Answer:

Verified

Regarding acid strength, which of the following is not correctly assigned?

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Question 3

Correct Answer:

Verified

Consider adding NaClO₄ to a basic solution. Which statement below is true?

(Multiple Choice)

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Question 4

After completing the following unfinished table, what is the order of increasing base strength ? Base K _b p K _b Fluoride ion, F^- 1.5×10^{- 11} Ammonia, NH₃ 4.75 Acetate ion, CH₃COO^- 5.7×10^{- 10}

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Question 5

Which aqueous solution(s) below is(are) considered basic ? I. A solution with a pH = 6 II. A solution with [OH^-] = 1×10^{- 7} III. A solution with [H₃O⁺] = 1×10^{- 9}

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Question 6

At 37 ° C the autoionization constant of water is K _w = 2.4×10^{- 14}. What is the pH of pure water at 37 ° C?

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Question 7

K _b for ammonia is 1.8×10^{- 5}. Calculate K _a for the ammonium ion.

(Multiple Choice)

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Question 8

If the reaction below proceeds, which of the following is true? NH₃ + C₂H₅OH→NH₂^- + C₂H₅OH₂⁺

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Question 9

In the reaction: N₂H₄ (aq) + H₂ O N₂H₅ + (aq) + OH - (aq)

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Question 10

What is the pH of a 0.025 M solution of HSCN ( K _a = 4.0×10^{- 6})?

(Multiple Choice)

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Question 11

A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K _a for this weak acid?

(Multiple Choice)

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Question 12

What is the acid ionization constant , K _a, for Chlorous acid, HClO₂, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33? You may want to complete the ICE table before getting started. HClO₂ H₃O⁺ ClO₂^{1 -} Initial Change @ equilibrium

(Multiple Choice)

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Question 13

What is the pH of an aqueous 0.036 M NaF solution? K _a(HF) = 6.8×10^{- 4}

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Question 14

50 mL of 0.50 M NaOH is added to enough water to make 1.0 liter of solution. Calculate the pH.

(Multiple Choice)

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Question 15

A nitric acid (HNO₃) solution is 16.2 M. Which of the following is correct?

(Multiple Choice)

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Question 16

Aniline, C₆ H₅ NH₂ , is commonly used as a precursor for making dyes. Aniline is a base when dissolved in water. It ionizes as shown below. What is the base ionization constant, K b , of aniline if an aqueous 0.20 M C₆ H₅ NH₂ solution has a pOH value equal tO₅ .05? C₆ H₅ NH₂ + H₂ O C₆ H₅ NH₃+ + OH -

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Question 17

Which anionic base listed below would be the strongest given the corresponding acid ionization constants for their conjugate acids?

(Multiple Choice)

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Question 18

What is the pOH of a 1.0×10^{- 4} M solution of HI?

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Question 19

An acid HB⁺ has a K _a of 1.0×10^{- 9}. What is the p K _b of the base B?

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Question 20

Showing 1 - 20 of 179

Exam 15: Solutions of Acids and Bases

When 20.0 grams of a water soluble salt dissolves in 1.0 L of pure water the pH was found to be less than seven. Which of the following statements about the salt is most probable?

Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH→C6H5NH3+ + HCOO - Which of the following is a conjugate acid-base pair?

Regarding acid strength, which of the following is not correctly assigned?

Consider adding NaClO4 to a basic solution. Which statement below is true?

After completing the following unfinished table, what is the order of increasing base strength ? Base K b p K b Fluoride ion, F - 1.5×10 - 11 Ammonia, NH3 4.75 Acetate ion, CH3COO - 5.7×10 - 10

Which aqueous solution(s) below is(are) considered basic ? I. A solution with a pH = 6 II. A solution with [OH - ] = 1×10 - 7 III. A solution with [H3O+] = 1×10 - 9

At 37 ° C the autoionization constant of water is K w = 2.4×10 - 14. What is the pH of pure water at 37 ° C?

K b for ammonia is 1.8×10 - 5. Calculate K a for the ammonium ion.

If the reaction below proceeds, which of the following is true? NH3 + C2H5OH→NH2 - + C2H5OH2+

In the reaction: N₂H4 (aq) + H₂ O N₂H5 + (aq) + OH - (aq)

What is the pH of a 0.025 M solution of HSCN ( K a = 4.0×10 - 6)?

A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K a for this weak acid?

What is the acid ionization constant , K a, for Chlorous acid, HClO2, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33? You may want to complete the ICE table before getting started. HClO2 H3O+ ClO21 - Initial Change @ equilibrium

What is the pH of an aqueous 0.036 M NaF solution? K a(HF) = 6.8×10 - 4

50 mL of 0.50 M NaOH is added to enough water to make 1.0 liter of solution. Calculate the pH.

A nitric acid (HNO3) solution is 16.2 M. Which of the following is correct?

Which anionic base listed below would be the strongest given the corresponding acid ionization constants for their conjugate acids?

What is the pOH of a 1.0×10 - 4 M solution of HI?

An acid HB+ has a K a of 1.0×10 - 9. What is the p K b of the base B?

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Consider the following Bronsted-Lowry acid-base reaction: C₆H₅NH₂ + HCOOH→C₆H₅NH₃⁺ + HCOO^- Which of the following is a conjugate acid-base pair?

Consider adding NaClO₄ to a basic solution. Which statement below is true?

After completing the following unfinished table, what is the order of increasing base strength ? Base K _b p K _b Fluoride ion, F^- 1.5×10^{- 11} Ammonia, NH₃ 4.75 Acetate ion, CH₃COO^- 5.7×10^{- 10}

Which aqueous solution(s) below is(are) considered basic ? I. A solution with a pH = 6 II. A solution with [OH^-] = 1×10^{- 7} III. A solution with [H₃O⁺] = 1×10^{- 9}

At 37 ° C the autoionization constant of water is K _w = 2.4×10^{- 14}. What is the pH of pure water at 37 ° C?

K _b for ammonia is 1.8×10^{- 5}. Calculate K _a for the ammonium ion.

If the reaction below proceeds, which of the following is true? NH₃ + C₂H₅OH→NH₂^- + C₂H₅OH₂⁺

In the reaction: N₂H₄ (aq) + H₂ O N₂H₅ + (aq) + OH - (aq)

What is the pH of a 0.025 M solution of HSCN ( K _a = 4.0×10^{- 6})?

A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K _a for this weak acid?

What is the acid ionization constant , K _a, for Chlorous acid, HClO₂, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33? You may want to complete the ICE table before getting started. HClO₂ H₃O⁺ ClO₂^{1 -} Initial Change @ equilibrium

What is the pH of an aqueous 0.036 M NaF solution? K _a(HF) = 6.8×10^{- 4}

A nitric acid (HNO₃) solution is 16.2 M. Which of the following is correct?

What is the pOH of a 1.0×10^{- 4} M solution of HI?

An acid HB⁺ has a K _a of 1.0×10^{- 9}. What is the p K _b of the base B?