Ten milliliters of 0.10 M NH3(aq) (K = 1.8 × 10-5) is mixed with 10 mL of 0.10 M NH4Cl. Neglecting the differences between activities and concentrations, the resulting solution:

A) has a pH = 4.74 B) has a [H+] of approximately 10-3 M C) has a [NH4+] greater than that of the NH4Cl(aq) D) has an [OH-] of 1.8 × 10-5 M E) is acidic A) has a pH = 4.74 B) has a [H+] of approximately 10-3 M C) has a [NH4+] greater than that of the NH4Cl(aq) D) has an [OH-] of 1.8 × 10-5 M E) is acidic

A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of this solution after 5.00 ml 10.0 M HCl is added?

A) 4.80 B) 4.86 C) 4.65 D) 4.70 E) 4.75 A) 4.80 B) 4.86 C) 4.65 D) 4.70 E) 4.75

A handbook states that to prepare a particular buffer solution mix 63.0 mL of 0.200 M HC2H3O2 with 37.0 mL of 0.200 M NaC2H3O2. What is the pH of this buffer? (Ka = 1.8 × 10-5)

A) 4.74 B) 4.51 C) 4.98 D) 5.33 E) 7.00 A) 4.74 B) 4.51 C) 4.98 D) 5.33 E) 7.00

Calculate the pH of an aqueous solution that is 1.0 M Na2CO3. Ka2 for H2CO3 is 4.7 × 10-11.

A) 8.8 B) 10.3 C) 3.7 D) 12.2 E) 1.8 A) 8.8 B) 10.3 C) 3.7 D) 12.2 E) 1.8

If 25 mL of 0.20 M NaOH is added to 50 mL of 0.10 M HC2H3O2 (Ka = 1.8 × 10-5), what is the pH?

A) 5.33 B) 10.21 C) 8.78 D) 13.56 E) 1.34 A) 5.33 B) 10.21 C) 8.78 D) 13.56 E) 1.34

What is the pH of a solution made by dissolving 2.16 g of sodium benzoate (NaC6H5CO2) in a sufficient volume of 0.033 M benzoic acid solution to prepare 500.0 mL of buffer? [Ka for benzoic acid is 6.3 × 10-5]

A) 4.16 B) 4.37 C) 4.64 D) 5.77 E) 6.30 A) 4.16 B) 4.37 C) 4.64 D) 5.77 E) 6.30

Calculate the pH of a 1.00 L solution of 0.100 M NH3(aq) after the addition of 0.010 mol NH4Cl(s). For NH3, pKb = 4.74.

A) 10.26 B) 9.26 C) 8.26 D) 11.56 A) 10.26 B) 9.26 C) 8.26 D) 11.56

Exam 17: Additional Aspects of Acid-Base Equilibria

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.10 M NaCN

(Multiple Choice)

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Question 61

Assuming no volume change on mixing, what mass of ammonium chloride should be added to 250.0 mL of 0.25 M ammonia to produce a solution of pH 10.70? [Kb for ammonia is 1.8 × 10^-5]

(Multiple Choice)

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Question 62

Ten milliliters of 0.10 M NH₃(aq) (K = 1.8 × 10^-5) is mixed with 10 mL of 0.10 M NH₄Cl. Neglecting the differences between activities and concentrations, the resulting solution:

(Multiple Choice)

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Question 63

What is the buffer range (for an effective 2.0 pH unit) for a benzoic acid/sodium benzoate buffer? [Ka for benzoic acid is 6.3 × 10^-5]

(Multiple Choice)

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Question 64

A solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M. Ka = 6.3 × 10^-5 for HC₇H₅O₂. The solution volume is 5.00 L. What is the pH of this solution after 5.00 ml 10.0 M HCl is added?

(Multiple Choice)

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Question 65

25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH have been added? Ka for acetic acid = 1.8 × 10^-5.

(Multiple Choice)

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Question 66

A strong acid and its conjugate base will form a buffer.

(True/False)

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Question 67

The common ion in a mixture of a weak acid and a strong acid is the hydronium ion.

(True/False)

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Question 68

A solution of an unknown acid had a pH of 3.70. Titration of a 25.0 mL aliquot of the acid solution required 21.7 mL of 0.104 M sodium hydroxide for complete reaction. Assuming that the acid is monoprotic, what is its ionization constant?

(Multiple Choice)

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Question 69

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.10 M HC₂H₃O₂

(Multiple Choice)

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Question 70

A salt of a polyprotic acid such as NaHCO₃ cannot act as an acid.

(True/False)

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Question 71

A handbook states that to prepare a particular buffer solution mix 63.0 mL of 0.200 M HC₂H₃O₂ with 37.0 mL of 0.200 M NaC₂H₃O₂. What is the pH of this buffer? (Ka = 1.8 × 10^-5)

(Multiple Choice)

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Question 72

Calculate the pH of an aqueous solution that is 1.0 M Na₂CO₃. Ka₂ for H₂CO₃ is 4.7 × 10^-11.

(Multiple Choice)

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Question 73

For the following titration, determine whether the solution at the equivalence point is acidic, basic or neutral and why: KOH is titrated with HI(aq)

(Multiple Choice)

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Question 74

If 25 mL of 0.20 M NaOH is added to 50 mL of 0.10 M HC₂H₃O₂ (Ka = 1.8 × 10^-5), what is the pH?

(Multiple Choice)

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Question 75

The solution that is added from the burret during a titration is the:

(Multiple Choice)

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Question 76

Which of the following mixtures would you dismiss as a potential buffer in a laboratory?

(Multiple Choice)

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Question 77

A pH 4.88 buffer was prepared by dissolving 0.10 mol of benzoic acid (Ka = 6.3 × 10^-5) and 0.50 mol of sodium benzoate in sufficient pure water to form a 1.00 L solution. To a 70.0 mL aliquot of this solution was added 2.00 mL of 2.00 M HI solution. What was the pH of the new 72.0 mL solution?

(Multiple Choice)

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Question 78

What is the pH of a solution made by dissolving 2.16 g of sodium benzoate (NaC₆H₅CO₂) in a sufficient volume of 0.033 M benzoic acid solution to prepare 500.0 mL of buffer? [Ka for benzoic acid is 6.3 × 10^-5]

(Multiple Choice)

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Question 79

Calculate the pH of a 1.00 L solution of 0.100 M NH₃(aq) after the addition of 0.010 mol NH₄Cl(s). For NH₃, pKb = 4.74.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 99

Exam 17: Additional Aspects of Acid-Base Equilibria

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.10 M NaCN

Assuming no volume change on mixing, what mass of ammonium chloride should be added to 250.0 mL of 0.25 M ammonia to produce a solution of pH 10.70? [Kb for ammonia is 1.8 × 10-5]

Ten milliliters of 0.10 M NH3(aq) (K = 1.8 × 10-5) is mixed with 10 mL of 0.10 M NH4Cl. Neglecting the differences between activities and concentrations, the resulting solution:

What is the buffer range (for an effective 2.0 pH unit) for a benzoic acid/sodium benzoate buffer? [Ka for benzoic acid is 6.3 × 10-5]

A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of this solution after 5.00 ml 10.0 M HCl is added?

25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH have been added? Ka for acetic acid = 1.8 × 10-5.

A strong acid and its conjugate base will form a buffer.

The common ion in a mixture of a weak acid and a strong acid is the hydronium ion.

A solution of an unknown acid had a pH of 3.70. Titration of a 25.0 mL aliquot of the acid solution required 21.7 mL of 0.104 M sodium hydroxide for complete reaction. Assuming that the acid is monoprotic, what is its ionization constant?

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.10 M HC2H3O2

A salt of a polyprotic acid such as NaHCO3 cannot act as an acid.

A handbook states that to prepare a particular buffer solution mix 63.0 mL of 0.200 M HC2H3O2 with 37.0 mL of 0.200 M NaC2H3O2. What is the pH of this buffer? (Ka = 1.8 × 10-5)

Calculate the pH of an aqueous solution that is 1.0 M Na2CO3. Ka2 for H2CO3 is 4.7 × 10-11.

For the following titration, determine whether the solution at the equivalence point is acidic, basic or neutral and why: KOH is titrated with HI(aq)

If 25 mL of 0.20 M NaOH is added to 50 mL of 0.10 M HC2H3O2 (Ka = 1.8 × 10-5), what is the pH?

The solution that is added from the burret during a titration is the:

Which of the following mixtures would you dismiss as a potential buffer in a laboratory?

A pH 4.88 buffer was prepared by dissolving 0.10 mol of benzoic acid (Ka = 6.3 × 10-5) and 0.50 mol of sodium benzoate in sufficient pure water to form a 1.00 L solution. To a 70.0 mL aliquot of this solution was added 2.00 mL of 2.00 M HI solution. What was the pH of the new 72.0 mL solution?

What is the pH of a solution made by dissolving 2.16 g of sodium benzoate (NaC6H5CO2) in a sufficient volume of 0.033 M benzoic acid solution to prepare 500.0 mL of buffer? [Ka for benzoic acid is 6.3 × 10-5]

Calculate the pH of a 1.00 L solution of 0.100 M NH3(aq) after the addition of 0.010 mol NH4Cl(s). For NH3, pKb = 4.74.

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Assuming no volume change on mixing, what mass of ammonium chloride should be added to 250.0 mL of 0.25 M ammonia to produce a solution of pH 10.70? [Kb for ammonia is 1.8 × 10^-5]

Ten milliliters of 0.10 M NH₃(aq) (K = 1.8 × 10^-5) is mixed with 10 mL of 0.10 M NH₄Cl. Neglecting the differences between activities and concentrations, the resulting solution:

What is the buffer range (for an effective 2.0 pH unit) for a benzoic acid/sodium benzoate buffer? [Ka for benzoic acid is 6.3 × 10^-5]

A solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M. Ka = 6.3 × 10^-5 for HC₇H₅O₂. The solution volume is 5.00 L. What is the pH of this solution after 5.00 ml 10.0 M HCl is added?

25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH have been added? Ka for acetic acid = 1.8 × 10^-5.

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.10 M HC₂H₃O₂

A salt of a polyprotic acid such as NaHCO₃ cannot act as an acid.

A handbook states that to prepare a particular buffer solution mix 63.0 mL of 0.200 M HC₂H₃O₂ with 37.0 mL of 0.200 M NaC₂H₃O₂. What is the pH of this buffer? (Ka = 1.8 × 10^-5)

Calculate the pH of an aqueous solution that is 1.0 M Na₂CO₃. Ka₂ for H₂CO₃ is 4.7 × 10^-11.

If 25 mL of 0.20 M NaOH is added to 50 mL of 0.10 M HC₂H₃O₂ (Ka = 1.8 × 10^-5), what is the pH?

A pH 4.88 buffer was prepared by dissolving 0.10 mol of benzoic acid (Ka = 6.3 × 10^-5) and 0.50 mol of sodium benzoate in sufficient pure water to form a 1.00 L solution. To a 70.0 mL aliquot of this solution was added 2.00 mL of 2.00 M HI solution. What was the pH of the new 72.0 mL solution?

What is the pH of a solution made by dissolving 2.16 g of sodium benzoate (NaC₆H₅CO₂) in a sufficient volume of 0.033 M benzoic acid solution to prepare 500.0 mL of buffer? [Ka for benzoic acid is 6.3 × 10^-5]

Calculate the pH of a 1.00 L solution of 0.100 M NH₃(aq) after the addition of 0.010 mol NH₄Cl(s). For NH₃, pKb = 4.74.