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Chemistry: An Atoms First Approach

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

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Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 14, Problem 28E
Textbook Problem
25 views

Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of each of the solutions in Exercise 22.

(a)

Interpretation Introduction

Interpretation:

The pH value after 0.020mole of NaOH is added to 1.00L of each of the given four solutions in Exercise 22 is to be calculated.

Concept introduction:

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

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

Explanation of Solution

Explanation

To determine the pOH

The volume of the solution is given to be 1.00L .

Therefore, the number of moles of HONH2 is 0.1mol .

The pH value of the solution formed will be affected by the OH ions from NaOH that is added to the given solution and by the OH ions from HONH2 .

Since, NaOH is a strong base, it will completely ionize to give OH ions.

Therefore, after the addition of NaOH ,

The overall [OH] =0.02+0.12=0.06M

The pOH of a solution is calculated by the formula,

pOH=log[OH]

Substitute the value of [OH] in the above expression

(b)

Interpretation Introduction

Interpretation:

The pH value after 0.020mole of NaOH is added to 1.00L of each of the given four solutions in Exercise 22 is to be calculated.

Concept introduction:

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

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

(c)

Interpretation Introduction

Interpretation:

The pH value after 0.020mole of NaOH is added to 1.00L of each of the given four solutions in Exercise 22 is to be calculated.

Concept introduction:

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

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

(d)

Interpretation Introduction

Interpretation:

The pH value after 0.020mole of NaOH is added to 1.00L of each of the given four solutions in Exercise 22 is to be calculated.

Concept introduction:

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

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

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Chapter 14 Solutions

Chemistry: An Atoms First Approach
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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. 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