What is the pH of a 1.0 M solution of Na3AsO4?( Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12 )

A) 2.5 B) 7.0 C) 8.2 D) 11.5 E) 5.8 A) 2.5 B) 7.0 C) 8.2 D) 11.5 E) 5.8

1.80 grams of an impure mixture containing sodium carbonate required 84.0 ml of 0.125 M H2SO4 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%

If some NH4Cl is added to an aqueous solution of NH3:

A) the pH of the solution will increase B) the pH of the solution will decrease C) the solution will not have pH D) the pH of the solution will not change E) NH4Cl cannot be added to NH3 A) the pH of the solution will increase B) the pH of the solution will decrease C) the solution will not have pH D) the pH of the solution will not change E) NH4Cl cannot be added to NH3

What will the pH at the neutralization point of 0.00812 M Ba(OH)2 be when titrated with HCl?

A) 7.0 B) 12.2 C) 8.0 D) 9.0 E) 6.0 A) 7.0 B) 12.2 C) 8.0 D) 9.0 E) 6.0

Determine the pH of the following solution. Initial concentrations are given. [HC2H3O2] = 0.250 M, [NaC2H3O2] = 0.120 M [Ka = 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

What volume in ml of 0.05 M NaOH would have to be added to 50.0 ml of 0.10 M H2SO4 in order to affect complete neutralization of the acid?

A) 50 mL B) 20 mL C) 100 mL D) 150 mL E) 200 mL A) 50 mL B) 20 mL C) 100 mL D) 150 mL E) 200 mL

The titration curve for 10.0 mL of 0.100 M H3PO4(aq) with 0.100 M NaOH(aq) is given below. Estimate the pKa2 of H3PO4.

A) 7.2 B) 4.8 C) 9.8 D) 2.2 A) 7.2 B) 4.8 C) 9.8 D) 2.2

Exam 17: Additional Aspects of Acid-Base Equilibria

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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 NH₄NO₃

(Multiple Choice)

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Question 41

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH at equivalence?

(Multiple Choice)

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Question 42

What is the pH of a 1.0 M solution of Na₃AsO₄?( Ka1 = 6 × 10^-3, Ka₂ = 1 × 10^-7, Ka₃ = 3 × 10^-12 )

(Multiple Choice)

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Question 43

What is the pH at the equivalence point for the titration of 0.20 M nitrous acid by 0.20 M sodium hydroxide? [Ka for nitrous acid is 4.5 × 10^-4]

(Multiple Choice)

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Question 44

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH when 30 ml of NaOH have been added?

(Multiple Choice)

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Question 45

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

(True/False)

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Question 46

25 ml of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH at the equivalence point? Ka for acetic acid = 1.8 × 10^-5.

(Multiple Choice)

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Question 47

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

(Multiple Choice)

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Question 48

If some NH₄Cl is added to an aqueous solution of NH₃:

(Multiple Choice)

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Question 49

What will the pH at the neutralization point of 0.00812 M Ba(OH)₂ be when titrated with HCl?

(Multiple Choice)

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Question 50

Determine the pH of the following solution. Initial concentrations are given. [HF] = 1.296 M, [HCl] = 1.045 M, Ka for HF is 6.6 × 10^-4

(Multiple Choice)

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Question 51

What is the pH of a 1.0 M solution of trisodium phosphate? Ka1 = 7.1 × 10^-3, Ka2 = 6.3 × 10^-8, Ka3 = 4.2 × 10^-13

(Multiple Choice)

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Question 52

Determine the pH of the following solution. Initial concentrations are given. [NaCHO₂] = 0.815 M, [HBr] = 0.105 M, Ka (HCHO₂) = 1.8 × 10^-4

(Multiple Choice)

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Question 53

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

(Multiple Choice)

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Question 54

What volume in ml of 0.05 M NaOH would have to be added to 50.0 ml of 0.10 M H₂SO₄ in order to affect complete neutralization of the acid?

(Multiple Choice)

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Question 55

For the following titration, determine whether the solution at the equivalence point is acidic, basic, or neutral and why: NaHCO₃(aq) titrated with NaOH(aq)

(Multiple Choice)

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Question 56

Choose the correct statement.

(Multiple Choice)

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Question 57

Phenolphthalein may be used as an indicator for the titration of:

(Multiple Choice)

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Question 58

A solution of sodium carbonate is easier to calculate the pH than sodium hydrogen carbonate because there is only one hydrolysis reaction instead of two.

(True/False)

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Question 59

The titration curve for 10.0 mL of 0.100 M H₃PO₄(aq) with 0.100 M NaOH(aq) is given below. Estimate the pKa₂of H₃PO₄.

(Multiple Choice)

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Question 60

Showing 41 - 60 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 NH4NO3

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH at equivalence?

What is the pH of a 1.0 M solution of Na3AsO4?( Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12 )

What is the pH at the equivalence point for the titration of 0.20 M nitrous acid by 0.20 M sodium hydroxide? [Ka for nitrous acid is 4.5 × 10-4]

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH when 30 ml of NaOH have been added?

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

25 ml of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH at the equivalence point? Ka for acetic acid = 1.8 × 10-5.

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

If some NH4Cl is added to an aqueous solution of NH3:

What will the pH at the neutralization point of 0.00812 M Ba(OH)2 be when titrated with HCl?

Determine the pH of the following solution. Initial concentrations are given. [HF] = 1.296 M, [HCl] = 1.045 M, Ka for HF is 6.6 × 10-4

What is the pH of a 1.0 M solution of trisodium phosphate? Ka1 = 7.1 × 10-3, Ka2 = 6.3 × 10-8, Ka3 = 4.2 × 10-13

Determine the pH of the following solution. Initial concentrations are given. [NaCHO2] = 0.815 M, [HBr] = 0.105 M, Ka (HCHO2) = 1.8 × 10-4

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

What volume in ml of 0.05 M NaOH would have to be added to 50.0 ml of 0.10 M H2SO4 in order to affect complete neutralization of the acid?

For the following titration, determine whether the solution at the equivalence point is acidic, basic, or neutral and why: NaHCO3(aq) titrated with NaOH(aq)

Choose the correct statement.

Phenolphthalein may be used as an indicator for the titration of:

A solution of sodium carbonate is easier to calculate the pH than sodium hydrogen carbonate because there is only one hydrolysis reaction instead of two.

The titration curve for 10.0 mL of 0.100 M H3PO4(aq) with 0.100 M NaOH(aq) is given below. Estimate the pKa2 of H3PO4.

Matter - Its Properties and Measurement

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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

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Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

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Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

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Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

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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 NH₄NO₃

What is the pH of a 1.0 M solution of Na₃AsO₄?( Ka1 = 6 × 10^-3, Ka₂ = 1 × 10^-7, Ka₃ = 3 × 10^-12 )

What is the pH at the equivalence point for the titration of 0.20 M nitrous acid by 0.20 M sodium hydroxide? [Ka for nitrous acid is 4.5 × 10^-4]

25 ml of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH at the equivalence point? Ka for acetic acid = 1.8 × 10^-5.

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

If some NH₄Cl is added to an aqueous solution of NH₃:

What will the pH at the neutralization point of 0.00812 M Ba(OH)₂ be when titrated with HCl?

Determine the pH of the following solution. Initial concentrations are given. [HF] = 1.296 M, [HCl] = 1.045 M, Ka for HF is 6.6 × 10^-4

What is the pH of a 1.0 M solution of trisodium phosphate? Ka1 = 7.1 × 10^-3, Ka2 = 6.3 × 10^-8, Ka3 = 4.2 × 10^-13

Determine the pH of the following solution. Initial concentrations are given. [NaCHO₂] = 0.815 M, [HBr] = 0.105 M, Ka (HCHO₂) = 1.8 × 10^-4

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

What volume in ml of 0.05 M NaOH would have to be added to 50.0 ml of 0.10 M H₂SO₄ in order to affect complete neutralization of the acid?

For the following titration, determine whether the solution at the equivalence point is acidic, basic, or neutral and why: NaHCO₃(aq) titrated with NaOH(aq)

The titration curve for 10.0 mL of 0.100 M H₃PO₄(aq) with 0.100 M NaOH(aq) is given below. Estimate the pKa₂of H₃PO₄.