What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 aqueous acetic acid (CH3COOH)with 50.00 mL of 0.100 mol L-1 KOH(aq)? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3COOH

A) 8.26 B) 9.26 C) 11.13 D) 12.40 A) 8.26 B) 9.26 C) 11.13 D) 12.40

What volume of 5.00 × 10-3 mol L-1 HNO3(aq)is needed to titrate 80.00 mL of 5.00 × 10-3 mol L-1 Ca(OH)2(aq)to the equivalence point?

A) 10.0 mL B) 40.0 mL C) 80.0 mL D) 160.mL A) 10.0 mL B) 40.0 mL C) 80.0 mL D) 160.mL

An aqueous 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(aq)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

What is the pH of a buffer solution prepared by dissolving 25.5 g NaC2H3O2 in a sufficient volume of 0.550 M aqueous HC2H3O2 to make 500.0 mL of buffer?

A) 4.74 B) 4.68 C) 4.91 D) 4.57 E) 4.79 A) 4.74 B) 4.68 C) 4.91 D) 4.57 E) 4.79

Determine the pH of the following aqueous solution.Initial concentrations are given. [HC2H3O2] = 0.250 M,[NaC2H3O2] = 0.120 M ,Ka ( acetic acid)= 1.8 × 10-5

A) 5.1 B) 4.4 C) 8.9 D) 9.6 E) 7.0 A) 5.1 B) 4.4 C) 8.9 D) 9.6 E) 7.0

A handbook states that to prepare a particular buffer solution mix 63.0 mL of 0.200 M aqueous HC2H3O2 with 37.0 mL of 0.200 M aqueous 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

Choose the expression that gives the molar concentration of a H2SO4(aq)solution if 24.3 mL of a 0.105 M NaOH(aq)solution is required to titrate 60 mL of the acid.

A) (60 × 24.3)/0.105 B) (60 × 2)/(24.3 × 0.105) C) (24.3 × 0.105)/(60) D) (24.3 × 0.105)/(60 × 2) E) (60 × 0.105)/(2 × 24.3) A) (60 × 24.3)/0.105 B) (60 × 2)/(24.3 × 0.105) C) (24.3 × 0.105)/(60) D) (24.3 × 0.105)/(60 × 2) E) (60 × 0.105)/(2 × 24.3)

An aqueous 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 the solution after 10.00 mL of 5.00 M NaOH 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

1.80 grams of an impure mixture containing sodium carbonate required 84.0 mL of 0.125 M H2SO4(aq)for complete neutralization.What percent of the mixture is sodium carbonate?

A) 62% B) 31% C) 120% D) 57% E) 1.1% A) 62% B) 31% C) 120% D) 57% E) 1.1%

Exam 17: Additional Aspects of Acidbase Equilibria

A pH 4.88 buffer was prepared by dissolving 0.10 mol of benzoic acid (K_a = 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 aqueous HI solution.What was the pH of the new 72.0 mL solution?

(Multiple Choice)

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Question 41

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 mol L^-1 NaOH(aq)? K_a = 6.76 × 10^-4 for HF.

(Multiple Choice)

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Question 42

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 aqueous acetic acid (CH₃COOH)with 50.00 mL of 0.100 mol L^-1 KOH(aq)? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃COOH

(Multiple Choice)

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Question 43

What volume of 5.00 × 10^-3 mol L^-1 HNO₃(aq)is needed to titrate 80.00 mL of 5.00 × 10^-3 mol L^-1 Ca(OH)₂(aq)to the equivalence point?

(Multiple Choice)

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Question 44

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

(True/False)

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Question 45

An aqueous solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M.K_a = 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(aq)is added?

(Multiple Choice)

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Question 46

A 25.0 mL sample of 0.150 mol L^-1 aqueous hypochlorous acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10^-8.

(Multiple Choice)

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Question 47

What is the pH of a buffer solution prepared by dissolving 25.5 g NaC₂H₃O₂ in a sufficient volume of 0.550 M aqueous HC₂H₃O₂ to make 500.0 mL of buffer?

(Multiple Choice)

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Question 48

Determine the pH of the following aqueous solution.Initial concentrations are given. [NH₃] = 1.20 M,[KOH] = 0.320 M,K_b for NH₃= 1.8 × 10^-5

(Multiple Choice)

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Question 49

Determine the pH of the following aqueous solution.Initial concentrations are given. [HC₂H₃O₂] = 0.250 M,[NaC₂H₃O₂] = 0.120 M ,K_a ( acetic acid)= 1.8 × 10^-5

(Multiple Choice)

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Question 50

A 25.0 mL sample of 0.150 mol L^-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10^-4.

(Multiple Choice)

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Question 51

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

(Multiple Choice)

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Question 52

Choose the expression that gives the molar concentration of a H₂SO₄(aq)solution if 24.3 mL of a 0.105 M NaOH(aq)solution is required to titrate 60 mL of the acid.

(Multiple Choice)

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Question 53

For an accurate titration,the end point needs to match the equivalence point.

(True/False)

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Question 54

What is the change in pH after addition of 10.0 mL of 1.0 M aqueous sodium hydroxide to 90.0 mL of an aqueous 1.0 M NH₃/1.0 M NH₄⁺ buffer? (K_b for ammonia is 1.8 × 10^-5)

(Multiple Choice)

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Question 55

A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia (K_b for ammonia is 1.8 × 10^-5)and 1.00 mol of ammonium chloride in water to form a solution with a volume of 1.00 L.To a 200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M aqueous sodium hydroxide.What was the resulting pH?

(Multiple Choice)

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Question 56

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

(Multiple Choice)

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Question 57

What is the pH of a buffer solution that is 0.255 mol L^-1 in hypochlorous acid (HClO)and 0.333 mol L^-1 in sodium hypochlorite (NaClO)? The Of hypochlorous acid is 3.8 × .

(Multiple Choice)

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Question 58

An aqueous solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M.K_a = 6.3 × 10^-5 for HC₇H₅O₂.The solution volume is 5.00 L.What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?

(Multiple Choice)

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Question 59

1.80 grams of an impure mixture containing sodium carbonate required 84.0 mL of 0.125 M H₂SO₄(aq)for complete neutralization.What percent of the mixture is sodium carbonate?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 130

Exam 17: Additional Aspects of Acidbase Equilibria

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 mol L-1 NaOH(aq)? Ka = 6.76 × 10-4 for HF.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 aqueous acetic acid (CH3COOH)with 50.00 mL of 0.100 mol L-1 KOH(aq)? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3COOH

What volume of 5.00 × 10-3 mol L-1 HNO3(aq)is needed to titrate 80.00 mL of 5.00 × 10-3 mol L-1 Ca(OH)2(aq)to the equivalence point?

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

An aqueous 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(aq)is added?

A 25.0 mL sample of 0.150 mol L-1 aqueous hypochlorous acid is titrated with a 0.150 mol L-1 NaOH(aq)solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10-8.

What is the pH of a buffer solution prepared by dissolving 25.5 g NaC2H3O2 in a sufficient volume of 0.550 M aqueous HC2H3O2 to make 500.0 mL of buffer?

Determine the pH of the following aqueous solution.Initial concentrations are given. [NH3] = 1.20 M,[KOH] = 0.320 M,Kb for NH3= 1.8 × 10-5

Determine the pH of the following aqueous solution.Initial concentrations are given. [HC2H3O2] = 0.250 M,[NaC2H3O2] = 0.120 M ,Ka ( acetic acid)= 1.8 × 10-5

A 25.0 mL sample of 0.150 mol L-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH(aq)solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10-4.

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

Choose the expression that gives the molar concentration of a H2SO4(aq)solution if 24.3 mL of a 0.105 M NaOH(aq)solution is required to titrate 60 mL of the acid.

For an accurate titration,the end point needs to match the equivalence point.

What is the change in pH after addition of 10.0 mL of 1.0 M aqueous sodium hydroxide to 90.0 mL of an aqueous 1.0 M NH3/1.0 M NH4+ buffer? (Kb for ammonia is 1.8 × 10-5)

A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia (Kb for ammonia is 1.8 × 10-5)and 1.00 mol of ammonium chloride in water to form a solution with a volume of 1.00 L.To a 200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M aqueous sodium hydroxide.What was the resulting pH?

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

What is the pH of a buffer solution that is 0.255 mol L-1 in hypochlorous acid (HClO)and 0.333 mol L-1 in sodium hypochlorite (NaClO)? The Of hypochlorous acid is 3.8 × .

An aqueous 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 the solution after 10.00 mL of 5.00 M NaOH is added?

1.80 grams of an impure mixture containing sodium carbonate required 84.0 mL of 0.125 M H2SO4(aq)for complete neutralization.What percent of the mixture is sodium carbonate?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

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Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

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Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

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What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 mol L^-1 NaOH(aq)? K_a = 6.76 × 10^-4 for HF.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 aqueous acetic acid (CH₃COOH)with 50.00 mL of 0.100 mol L^-1 KOH(aq)? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃COOH

What volume of 5.00 × 10^-3 mol L^-1 HNO₃(aq)is needed to titrate 80.00 mL of 5.00 × 10^-3 mol L^-1 Ca(OH)₂(aq)to the equivalence point?

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

An aqueous solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M.K_a = 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(aq)is added?

A 25.0 mL sample of 0.150 mol L^-1 aqueous hypochlorous acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10^-8.

What is the pH of a buffer solution prepared by dissolving 25.5 g NaC₂H₃O₂ in a sufficient volume of 0.550 M aqueous HC₂H₃O₂ to make 500.0 mL of buffer?

Determine the pH of the following aqueous solution.Initial concentrations are given. [NH₃] = 1.20 M,[KOH] = 0.320 M,K_b for NH₃= 1.8 × 10^-5

Determine the pH of the following aqueous solution.Initial concentrations are given. [HC₂H₃O₂] = 0.250 M,[NaC₂H₃O₂] = 0.120 M ,K_a ( acetic acid)= 1.8 × 10^-5

A 25.0 mL sample of 0.150 mol L^-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10^-4.

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

Choose the expression that gives the molar concentration of a H₂SO₄(aq)solution if 24.3 mL of a 0.105 M NaOH(aq)solution is required to titrate 60 mL of the acid.

What is the change in pH after addition of 10.0 mL of 1.0 M aqueous sodium hydroxide to 90.0 mL of an aqueous 1.0 M NH₃/1.0 M NH₄⁺ buffer? (K_b for ammonia is 1.8 × 10^-5)

A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia (K_b for ammonia is 1.8 × 10^-5)and 1.00 mol of ammonium chloride in water to form a solution with a volume of 1.00 L.To a 200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M aqueous sodium hydroxide.What was the resulting pH?

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

What is the pH of a buffer solution that is 0.255 mol L^-1 in hypochlorous acid (HClO)and 0.333 mol L^-1 in sodium hypochlorite (NaClO)? The Of hypochlorous acid is 3.8 × .

An aqueous solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M.K_a = 6.3 × 10^-5 for HC₇H₅O₂.The solution volume is 5.00 L.What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?

1.80 grams of an impure mixture containing sodium carbonate required 84.0 mL of 0.125 M H₂SO₄(aq)for complete neutralization.What percent of the mixture is sodium carbonate?