BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 14, Problem 1RQ
Textbook Problem
442 views

What is meant by the presence of a common ion? How does the presence of a common ion affect an equilibrium such as

HNO2(aq) ⇌ H+(aq) + NO2-(aq)

What is an acid–base solution called that contains a common ion?

(a)

Interpretation Introduction

Interpretation:

The presence of a common ion is to be explained. The affect of the presence of a common ion on equilibrium of the given reaction is to be stated. The term used for an acid-base solution that contains a common ion is to be determined.

Concept introduction:

The presence of a common ion brings about a shift in the equilibrium position.

To determine: An explanation regarding the presence of a common ion.

Answer to Problem 1RQ

The presence of a common ion shifts the equilibrium position.

Explanation of Solution

The shift in the equilibrium state that happens due to the addition of an ion that is already present in the equilibrium reaction is stated as the presence of a common ion.

(b)

Interpretation Introduction

Interpretation:

The presence of a common ion is to be explained. The affect of the presence of a common ion on equilibrium of the given reaction is to be stated. The term used for an acid-base solution that contains a common ion is to be determined.

Concept introduction:

The presence of a common ion brings about a shift in the equilibrium position.

To determine: The affect of the presence of a common ion on equilibrium of the given reaction

Answer to Problem 1RQ

The presence of a common ion shifts the equilibrium of the given reaction towards left.

Explanation of Solution

The given reaction is,

HNO2(aq)H+(aq)+NO2(aq)

The presence of a common ion in the given reaction will reduce the solubility of the given acid shifting the equilibrium towards the left. The dissociation of the given acid will be suppressed.

(c)

Interpretation Introduction

Interpretation:

The presence of a common ion is to be explained. The affect of the presence of a common ion on equilibrium of the given reaction is to be stated. The term used for an acid-base solution that contains a common ion is to be determined.

Concept introduction:

The presence of a common ion brings about a shift in the equilibrium position.

To determine: The term used for an acid-base solution that contains a common ion.

Answer to Problem 1RQ

An acid-base solution that contains a common ion is a buffer solution.

Explanation of Solution

An acid-base solution that contains a common ion is a buffer solution.

A buffer solution is also defined as a solution that resists a change in the pH on addition of an acid or an alkali

Conclusion

A solution that resists a change in the pH on addition of an acid or an alkali is termed as a buffer solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Chapter 14 Solutions

Chemistry: An Atoms First Approach
Show all chapter solutions
add
Ch. 14 - What are the major species in solution after...Ch. 14 - A friend asks the following: Consider a buffered...Ch. 14 - Mixing together solutions of acetic acid and...Ch. 14 - Could a buffered solution be made by mixing...Ch. 14 - Sketch two pH curves, one for the titration of a...Ch. 14 - Sketch a pH curve for the titration of a weak acid...Ch. 14 - You have a solution of the weak acid HA and add...Ch. 14 - You have a solution of the weak acid HA and add...Ch. 14 - The common ion effect for weak acids is to...Ch. 14 - Consider a buffer solution where [weak acid] ...Ch. 14 - A best buffer has about equal quantities of weak...Ch. 14 - Consider the following pH curves for 100.0 mL of...Ch. 14 - An acid is titrated with NaOH. The following...Ch. 14 - Consider the following four titrations. i. 100.0...Ch. 14 - Figure 14-4 shows the pH curves for the titrations...Ch. 14 - Acidbase indicators mark the end point of...Ch. 14 - How many of the following are buffered solutions?...Ch. 14 - Which of the following can be classified as buffer...Ch. 14 - A certain buffer is made by dissolving NaHCO3 and...Ch. 14 - A buffer is prepared by dissolving HONH2 and...Ch. 14 - Calculate the pH of each of the following...Ch. 14 - Calculate the pH of each of the following...Ch. 14 - Compare the percent dissociation of the acid in...Ch. 14 - Compare the percent ionization of the base in...Ch. 14 - Calculate the pH after 0.020 mole of HCl is added...Ch. 14 - Calculate the pH after 0.020 mole of HCl is added...Ch. 14 - Calculate the pH after 0.020 mole of NaOH is added...Ch. 14 - Calculate the pH after 0.020 mole of NaOH is added...Ch. 14 - Which of the solutions in Exercise 21 shows the...Ch. 14 - Which of the solutions in Exercise 22 is a...Ch. 14 - Calculate the pH of a solution that is 1.00 M HNO2...Ch. 14 - Calculate the pH of a solution that is 0.60 M HF...Ch. 14 - Calculate the pH after 0.10 mole of NaOH is added...Ch. 14 - Calculate the pH after 0.10 mole of NaOH is added...Ch. 14 - Calculate the pH of each of the following buffered...Ch. 14 - Calculate the pH of each of the following buffered...Ch. 14 - Calculate the pH of a buffered solution prepared...Ch. 14 - A buffered solution is made by adding 50.0 g NH4Cl...Ch. 14 - Calculate the pH after 0.010 mole of gaseous HCl...Ch. 14 - An aqueous solution contains dissolved C6H5NH3Cl...Ch. 14 - Calculate the mass of sodium acetate that must be...Ch. 14 - What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must...Ch. 14 - Consider a solution that contains both C5H5N and...Ch. 14 - Calculate the ratio [NH3]/[NH4+] in...Ch. 14 - Carbonate buffers are important in regulating the...Ch. 14 - When a person exercises, muscle contractions...Ch. 14 - Consider the acids in Table 13-2. Which acid would...Ch. 14 - Consider the bases in Table 13-3. Which base would...Ch. 14 - Calculate the pH of a solution that is 0.40 M...Ch. 14 - Calculate the pH of a solution that is 0.20 M HOCl...Ch. 14 - Which of the following mixtures would result in...Ch. 14 - Which of the following mixtures would result in a...Ch. 14 - What quantity (moles) of NaOH must be added to 1.0...Ch. 14 - Calculate the number of moles of HCl(g) that must...Ch. 14 - Consider the titration of a generic weak acid HA...Ch. 14 - Sketch the titration curve for the titration of a...Ch. 14 - Consider the titration of 40.0 mL of 0.200 M HClO4...Ch. 14 - Consider the titration of 80.0 mL of 0.100 M...Ch. 14 - Consider the titration of 100.0 mL of 0.200 M...Ch. 14 - Consider the titration of 100.0 mL of 0.100 M...Ch. 14 - Lactic acid is a common by-product of cellular...Ch. 14 - Repeat the procedure in Exercise 61, but for the...Ch. 14 - Repeat the procedure in Exercise 61, but for the...Ch. 14 - Repeat the procedure in Exercise 61, but for the...Ch. 14 - Calculate the pH at the halfway point and at the...Ch. 14 - In the titration of 50.0 mL of 1.0 M methylamine,...Ch. 14 - You have 75.0 mL of 0.10 M HA. After adding 30.0...Ch. 14 - A student dissolves 0.0100 mole of an unknown weak...Ch. 14 - Two drops of indicator HIn (Ka = 1.0 109), where...Ch. 14 - Methyl red has the following structure: It...Ch. 14 - Potassium hydrogen phthalate, known as KHP (molar...Ch. 14 - A certain indicator HIn has a pKa of 3.00 and a...Ch. 14 - Which of the indicators in Fig. 14-8 could be used...Ch. 14 - Which of the indicators in Fig. 14-8 could be used...Ch. 14 - Which of the indicators in Fig. 14-8 could be used...Ch. 14 - Which of the indicators in Fig. 14-8 could be used...Ch. 14 - Estimate the pH of a solution in which bromcresol...Ch. 14 - Estimate the pH of a solution in which crystal...Ch. 14 - A solution has a pH of 7.0. What would be the...Ch. 14 - A solution has a pH of 4.5. What would be the...Ch. 14 - Derive an equation analogous to the...Ch. 14 - a. Calculate the pH of a buffered solution that is...Ch. 14 - Tris(hydroxymethyl)aminomethane, commonly called...Ch. 14 - You make 1.00 L of a buffered solution (pH = 4.00)...Ch. 14 - You have the following reagents on hand: Solids...Ch. 14 - Amino acids are the building blocks for all...Ch. 14 - Phosphate buffers are important in regulating the...Ch. 14 - What quantity (moles) of HCl(g) must be added to...Ch. 14 - Calculate the value of the equilibrium constant...Ch. 14 - The following plot shows the pH curves for the...Ch. 14 - Calculate the volume of 1.50 102 M NaOH that must...Ch. 14 - Repeat the procedure in Exercise 61, but for the...Ch. 14 - A certain acetic acid solution has pH = 2.68....Ch. 14 - A 0.210-g sample of an acid (molar mass = 192...Ch. 14 - The active ingredient in aspirin is...Ch. 14 - One method for determining the purity of aspirin...Ch. 14 - A student intends to titrate a solution of a weak...Ch. 14 - A student titrates an unknown weak acid, HA, to a...Ch. 14 - A sample of a certain monoprotic weak acid was...Ch. 14 - Consider 1.0 L of a solution that is 0.85 M HOC6H5...Ch. 14 - What concentration of NH4Cl is necessary to buffer...Ch. 14 - Consider the following acids and bases: HCO2H Ka =...Ch. 14 - Consider a buffered solution containing CH3NH3Cl...Ch. 14 - Consider the titration of 150.0 mL of 0.100 M HI...Ch. 14 - Consider the titration of 100.0 mL of 0.100 M HCN...Ch. 14 - Consider the titration of 100.0 mL of 0.200 M...Ch. 14 - Consider the following four titrations (iiv): i....Ch. 14 - Another way to treat data from a pH titration is...Ch. 14 - A buffer is made using 45.0 mL of 0.750 M HC3H5O2...Ch. 14 - A 0.400-M solution of ammonia was titrated with...Ch. 14 - What volume of 0.0100 M NaOH must be added to 1.00...Ch. 14 - Consider a solution formed by mixing 50.0 mL of...Ch. 14 - When a diprotic acid, H2A, is titrated with NaOH,...Ch. 14 - Consider the following two acids: In two separate...Ch. 14 - The titration of Na2CO3 with HCl bas the following...Ch. 14 - Consider the titration curve in Exercise 115 for...Ch. 14 - A few drops of each of the indicators shown in the...Ch. 14 - Malonic acid (HO2CCH2CO2H) is a diprotic acid. In...Ch. 14 - A buffer solution is prepared by mixing 75.0 mL of...Ch. 14 - A 10.00-g sample of the ionic compound NaA, where...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Consider a solution prepared by mixing the...

Additional Science Textbook Solutions

Find more solutions based on key concepts
Show solutions add
Brown adipose tissue. develops during starvation is a well-known heat-generating tissue develops as fat cells d...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

13. What is spectroscopy?

Chemistry In Focus

What functional groups are found in all amino acids?

Chemistry for Today: General, Organic, and Biochemistry

A system consists of three particles, each of mass 5.00 g, located at the corners of an equilateral triangle wi...

Physics for Scientists and Engineers, Technology Update (No access codes included)

What forces control the shape of a continental shelf? A continental slope? A continental rise?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin