What is the pH of a 1.0 M solution of Na2SO3? Ka1 = 1.3 × 10-2, Ka2 = 6.2 × 10-8 ?

A) 6.8 B) 7.2 C) 7.0 D) 10.4 E) 3.6 A) 6.8 B) 7.2 C) 7.0 D) 10.4 E) 3.6

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

A) (60 × 24.3)/0.105 B) (60 × 2)/(24.3 × 0.1050) 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 × 0.1050) C) (24.3 × 0.105)/(60) D) (24.3 × 0.105)/(60 × 2) E) (60 × 0.105)/(2 × 24.3)

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

A) 10.21 B) 9.26 C) 8.31 D) 11.46 A) 10.21 B) 9.26 C) 8.31 D) 11.46

Exam 17: Additional Aspects of Acid-Base Equilibria

Explore all topics

The buffer capacity of a solution may be defined as the number of moles of H+ that will change the pH of 1.00 L of the buffer by 1.00 pH units. What is the buffer capacity of a solution which is 0.10 M in acetic acid (Ka = 1.8 × 10^-5) and 0.30 M in sodium acetate, in units of mol (H+) per liter?

Free

(Multiple Choice)

4.8/5

(36)

Question 1

Correct Answer:

Verified

Which of the pH indicators from the list above would be most appropriate for the titration of 0.30 M acetic acid (Ka = 1.8 × 10^-5) with 0.15 M sodium hydroxide?

Free

(Multiple Choice)

4.9/5

(36)

Question 2

Correct Answer:

Verified

In the titration of a solution of HCN(aq) with NaOH(aq), the equivalence point occurs at a pH greater than 7.

Free

(True/False)

4.9/5

(36)

Question 3

Correct Answer:

Verified

True

Why do we avoid titrating ammonia with acetic acid?

(Multiple Choice)

5.0/5

(34)

Question 4

An acid has a Ka = 1 × 10^-6. At what pH would this acid and its corresponding salt make a good buffer?

(Multiple Choice)

4.8/5

(41)

Question 5

How will addition of sodium acetate to an acetic acid solution affect the pH?

(Multiple Choice)

4.8/5

(34)

Question 6

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH before any NaOH is added?

(Multiple Choice)

4.9/5

(38)

Question 7

What is the [H₃O⁺] of a solution measured to be 0.20 M in sodium acetate and 0.40 M in acetic acid? [Ka = 1.8 × 10^-5]

(Multiple Choice)

4.9/5

(39)

Question 8

How many mL of 0.200 M acetic acid are mixed with 13.2 mL of 0.200 M sodium acetate to give a buffer with pH = 4.2?

(Multiple Choice)

4.9/5

(41)

Question 9

25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have been added? Ka for acetic acid = 1.8 × 10^-5.

(Multiple Choice)

4.8/5

(39)

Question 10

What is the pH of a 1.0 M solution of Na₂SO₃? Ka₁ = 1.3 × 10^-2, Ka₂ = 6.2 × 10^-8 ?

(Multiple Choice)

4.8/5

(43)

Question 11

Which among the following pairs is inefficient as buffer pair?

(Multiple Choice)

4.9/5

(29)

Question 12

For the following titration, determine whether the solution at the equivalence point is acidic, basic or neutral and why: HCl is titrated with NH₃(aq)

(Multiple Choice)

4.9/5

(30)

Question 13

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

(Multiple Choice)

4.7/5

(37)

Question 14

Acid-base indicators have two forms: an acid of one color and a base of another color.

(True/False)

4.9/5

(36)

Question 15

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

(Multiple Choice)

4.9/5

(42)

Question 16

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

(Multiple Choice)

4.8/5

(44)

Question 17

The pH of a buffer depends mainly on the pKa of the weak acid component of the buffer.

(True/False)

4.9/5

(40)

Question 18

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: 0.1 M NaCl

(Multiple Choice)

4.9/5

(36)

Question 19

The pH of a buffer solution changes only slightly with addition of a small amount of acid or base.

(True/False)

4.9/5

(40)

Question 20

Showing 1 - 20 of 99

Exam 17: Additional Aspects of Acid-Base Equilibria

The buffer capacity of a solution may be defined as the number of moles of H+ that will change the pH of 1.00 L of the buffer by 1.00 pH units. What is the buffer capacity of a solution which is 0.10 M in acetic acid (Ka = 1.8 × 10-5) and 0.30 M in sodium acetate, in units of mol (H+) per liter?

Which of the pH indicators from the list above would be most appropriate for the titration of 0.30 M acetic acid (Ka = 1.8 × 10-5) with 0.15 M sodium hydroxide?

In the titration of a solution of HCN(aq) with NaOH(aq), the equivalence point occurs at a pH greater than 7.

Why do we avoid titrating ammonia with acetic acid?

An acid has a Ka = 1 × 10-6. At what pH would this acid and its corresponding salt make a good buffer?

How will addition of sodium acetate to an acetic acid solution affect the pH?

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH before any NaOH is added?

What is the [H3O+] of a solution measured to be 0.20 M in sodium acetate and 0.40 M in acetic acid? [Ka = 1.8 × 10-5]

How many mL of 0.200 M acetic acid are mixed with 13.2 mL of 0.200 M sodium acetate to give a buffer with pH = 4.2?

25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have been added? Ka for acetic acid = 1.8 × 10-5.

What is the pH of a 1.0 M solution of Na2SO3? Ka1 = 1.3 × 10-2, Ka2 = 6.2 × 10-8 ?

Which among the following pairs is inefficient as buffer pair?

For the following titration, determine whether the solution at the equivalence point is acidic, basic or neutral and why: HCl is titrated with NH3(aq)

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

Acid-base indicators have two forms: an acid of one color and a base of another color.

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

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

The pH of a buffer depends mainly on the pKa of the weak acid component of the buffer.

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: 0.1 M NaCl

The pH of a buffer solution changes only slightly with addition of a small amount of acid or base.

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

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: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

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

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

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

The buffer capacity of a solution may be defined as the number of moles of H+ that will change the pH of 1.00 L of the buffer by 1.00 pH units. What is the buffer capacity of a solution which is 0.10 M in acetic acid (Ka = 1.8 × 10^-5) and 0.30 M in sodium acetate, in units of mol (H+) per liter?

Which of the pH indicators from the list above would be most appropriate for the titration of 0.30 M acetic acid (Ka = 1.8 × 10^-5) with 0.15 M sodium hydroxide?

An acid has a Ka = 1 × 10^-6. At what pH would this acid and its corresponding salt make a good buffer?

What is the [H₃O⁺] of a solution measured to be 0.20 M in sodium acetate and 0.40 M in acetic acid? [Ka = 1.8 × 10^-5]

25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have been added? Ka for acetic acid = 1.8 × 10^-5.

What is the pH of a 1.0 M solution of Na₂SO₃? Ka₁ = 1.3 × 10^-2, Ka₂ = 6.2 × 10^-8 ?

For the following titration, determine whether the solution at the equivalence point is acidic, basic or neutral and why: HCl is titrated with NH₃(aq)

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

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

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