menu
bartleby
search
close search
Hit Return to see all results
close solutoin list

a. Calculate the pH of a buffered solution that is 0.100 M in C 6 H 5 CO 2 H (benzoic acid, K a = 6.4 × 10 −5 ) and 0.100 M in C 6 H 5 CO 2 Na. b. Calculate the pH after 20.0% (by moles) of the benzoic acid is converted to benzoate anion by addition of a strong base. Use the dissociation equilibrium C 6 H 5 CO 2 H(aq) ⇌ C 6 H 5 CO 2 - (aq) + H + (aq) to calculate the pH. c. Do the same as in part b, but use the following equilibrium to calculate the pH: C 6 H 5 CO 2 - (aq) + H 2 O(l) ⇌ C 6 H 5 CO 2 H(aq) + OH - (aq) d. Do your answers in parts b and c agree? Explain.

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 82AE
Textbook Problem
1 views

a. Calculate the pH of a buffered solution that is 0.100 M in C6H5CO2H (benzoic acid, Ka = 6.4 × 10−5) and 0.100 M in C6H5CO2Na.

b. Calculate the pH after 20.0% (by moles) of the benzoic acid is converted to benzoate anion by addition of a strong base. Use the dissociation equilibrium

C6H5CO2H(aq) ⇌ C6H5CO2-(aq) + H+(aq)

to calculate the pH.

c. Do the same as in part b, but use the following equilibrium to calculate the pH:

C6H5CO2-(aq) + H2O(l) ⇌ C6H5CO2H(aq) + OH-(aq)

d. Do your answers in parts b and c agree? Explain.

(a)

Interpretation Introduction

Interpretation:

The pH value of the given solutions is to be calculated.

Concept introduction:

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

The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

Explanation of Solution

Explanation

Given

The concentration of benzoic acid is 0.100M .

The concentration of sodium benzoate is 0.100M .

The Ka of benzoic acid is 6.4×105 .

The relation between pH and pKa is given by Henderson-Hasselbach equation. According to this equation,

pH=pKa+log[Salt][Acid]

The value of pKa is calculated by the formula,

pKa=log(Ka)

Substitute the value of pKa in the Henderson-Hasselbach equation

(b)

Interpretation Introduction

Interpretation:

The pH value of the given solutions is to be calculated.

Concept introduction:

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

The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

(c)

Interpretation Introduction

Interpretation:

The pH value of the given solutions is to be calculated.

Concept introduction:

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

The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

(d)

Interpretation Introduction

Interpretation:

The pH value of the given solutions is to be calculated.

Concept introduction:

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

The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample 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
Vitamin A supplements can help treat acne. T F

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

Why does the expansion of a stars envelope make it cooler and more luminous?

Horizons: Exploring the Universe (MindTap Course List)

4. Define chemistry.

Chemistry In Focus

Within a cylindrical region of space of radius 100 Mm, a magnetic field is uniform with a magnitude 25.0 T and ...

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