Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H3PO4 + H2O H2PO4- + H3O+ H2PO4- + H2O HPO42- + H3O+ HPO42- + H2O PO43- + H3O+ Which equilibrium is most important in determining the pH of a solution of sodium phosphate?

A) HPO42- + H2O PO43- + H3O+ B) H3PO4 + H2O H2PO4- + H3O+ C) PO43- + H2O HPO42- + OH- D) H2PO4- + H2O H3PO4 + OH- E) 2H2O H3O+ + OH- A) HPO42- + H2O PO43- + H3O+ B) H3PO4 + H2O H2PO4- + H3O+ C) PO43- + H2O HPO42- + OH- D) H2PO4- + H2O H3PO4 + OH- E) 2H2O H3O+ + OH-

Exam 17: Equilibrium in the Aqueous Phase

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H₃PO₄ + H₂O H₂PO₄^- + H₃O⁺ H₂PO₄^- + H₂O HPO₄²^- + H₃O⁺ HPO₄²^- + H₂O PO₄³^- + H₃O⁺ Which equilibrium is most important in determining the pH of a solution of sodium phosphate?

(Multiple Choice)

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Question 41

Which of the following can be mixed together in water to produce a buffer solution?

(Multiple Choice)

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Question 42

Which one of the following statements is not correct?

(Multiple Choice)

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Question 43

What is indicated by the shape of the titration curve?

(Multiple Choice)

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Question 44

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H₃PO₄ + H₂O H₂PO₄^- + H₃O⁺ H₂PO₄^- + H₂O HPO₄²^- + H₃O⁺ HPO₄²^- + H₂O PO₄³^- + H₃O⁺ What is the K_b expression for the base, dihydrogen phosphate?

(Multiple Choice)

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Question 45

The acid ionization equilibrium constant, K_a, describes the reaction (where HA is a generic weak acid):

(Multiple Choice)

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Question 46

In the following reaction in aqueous solution, the acid reactant is and its conjugate base product is . CH₃COOH + NH₃ CH₃COO^- + NH₄⁺

(Multiple Choice)

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Question 47

The following titration curve is most likely to be associated with __________

(Multiple Choice)

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Question 48

What is the pH of a 0.20 M solution of ammonia? The K_b value for ammonia is 1.8  10^-⁵

(Multiple Choice)

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Question 49

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pK_a values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has the conjugate bases of these acids in order of decreasing strength?

(Multiple Choice)

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Question 50

The degree of ionization of a strong acid is __________

(Multiple Choice)

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Question 51

A solution with pH of 9.50 has a pOH of __________

(Multiple Choice)

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Question 52

The first disinfectant used by Joseph Lister was called carbolic acid. This substance now is known as phenol, C₆H₅OH (pK_a = 10.0). What is the pH of a 0.10 M solution of phenol?

(Multiple Choice)

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Question 53

Give an example of a monoprotic acid and a polyprotic acid.

(Essay)

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Question 54

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 1.25  10^-³M, 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.

(Multiple Choice)

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Question 55

When values of K_a are small (e.g., 1  10^-⁵) and concentrations of weak acids [HA] are relatively large (e.g., 0.10 M), the hydronium ion concentration of the solution can be calculated using which expression?

(Multiple Choice)

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Question 56

The pH of a popular soft drink is 3.4; what is its hydronium ion concentration?

(Multiple Choice)

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Question 57

The degree of ionization __________

(Multiple Choice)

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Question 58

The acidic ingredient in vinegar is acetic acid. The pH of vinegar is around 2.4, and the molar concentration of acetic acid in vinegar is around 0.85 M. Based on this information, determine the value of the acid ionization constant, K_a, for acetic acid.

(Multiple Choice)

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Question 59

Acid-base indicators need to have very intense colors so that a very low concentration is visible. Could there be a problem in using too much indicator?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 156

Exam 17: Equilibrium in the Aqueous Phase

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H3PO4 + H2O H2PO4- + H3O+ H2PO4- + H2O HPO42- + H3O+ HPO42- + H2O PO43- + H3O+ Which equilibrium is most important in determining the pH of a solution of sodium phosphate?

Which of the following can be mixed together in water to produce a buffer solution?

Which one of the following statements is not correct?

What is indicated by the shape of the titration curve?

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H3PO4 + H2O H2PO4- + H3O+ H2PO4- + H2O HPO42- + H3O+ HPO42- + H2O PO43- + H3O+ What is the Kb expression for the base, dihydrogen phosphate?

The acid ionization equilibrium constant, Ka, describes the reaction (where HA is a generic weak acid):

In the following reaction in aqueous solution, the acid reactant is __________ and its conjugate base product is __________. CH3COOH + NH3 CH3COO- + NH4+

The following titration curve is most likely to be associated with __________

What is the pH of a 0.20 M solution of ammonia? The Kb value for ammonia is 1.8  10-5

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pKa values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has the conjugate bases of these acids in order of decreasing strength?

The degree of ionization of a strong acid is __________

A solution with pH of 9.50 has a pOH of __________

The first disinfectant used by Joseph Lister was called carbolic acid. This substance now is known as phenol, C6H5OH (pKa = 10.0). What is the pH of a 0.10 M solution of phenol?

Give an example of a monoprotic acid and a polyprotic acid.

When values of Ka are small (e.g., 1  10-5) and concentrations of weak acids [HA] are relatively large (e.g., 0.10 M), the hydronium ion concentration of the solution can be calculated using which expression?

The pH of a popular soft drink is 3.4; what is its hydronium ion concentration?

The degree of ionization __________

The acidic ingredient in vinegar is acetic acid. The pH of vinegar is around 2.4, and the molar concentration of acetic acid in vinegar is around 0.85 M. Based on this information, determine the value of the acid ionization constant, Ka, for acetic acid.

Acid-base indicators need to have very intense colors so that a very low concentration is visible. Could there be a problem in using too much indicator?

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Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H₃PO₄ + H₂O H₂PO₄^- + H₃O⁺ H₂PO₄^- + H₂O HPO₄²^- + H₃O⁺ HPO₄²^- + H₂O PO₄³^- + H₃O⁺ Which equilibrium is most important in determining the pH of a solution of sodium phosphate?

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H₃PO₄ + H₂O H₂PO₄^- + H₃O⁺ H₂PO₄^- + H₂O HPO₄²^- + H₃O⁺ HPO₄²^- + H₂O PO₄³^- + H₃O⁺ What is the K_b expression for the base, dihydrogen phosphate?

The acid ionization equilibrium constant, K_a, describes the reaction (where HA is a generic weak acid):

In the following reaction in aqueous solution, the acid reactant is and its conjugate base product is . CH₃COOH + NH₃ CH₃COO^- + NH₄⁺

What is the pH of a 0.20 M solution of ammonia? The K_b value for ammonia is 1.8  10^-⁵

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pK_a values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has the conjugate bases of these acids in order of decreasing strength?

The first disinfectant used by Joseph Lister was called carbolic acid. This substance now is known as phenol, C₆H₅OH (pK_a = 10.0). What is the pH of a 0.10 M solution of phenol?

When values of K_a are small (e.g., 1  10^-⁵) and concentrations of weak acids [HA] are relatively large (e.g., 0.10 M), the hydronium ion concentration of the solution can be calculated using which expression?

The acidic ingredient in vinegar is acetic acid. The pH of vinegar is around 2.4, and the molar concentration of acetic acid in vinegar is around 0.85 M. Based on this information, determine the value of the acid ionization constant, K_a, for acetic acid.