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Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
Publisher: Cengage Learning
ISBN: 9781305079373

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Chapter
Section
BuyFindarrow_forward

Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
Publisher: Cengage Learning
ISBN: 9781305079373
Chapter 13, Problem 11QAP
Textbook Problem
1 views

Using the Brønsted-Lowry model, write an equation to show why each of the following species produces a basic aqueous solution.

(a) NH3(b) NO2-

(c) C6H5NH2

(d) CO32-

(e) F-(f) HCO3-

Interpretation Introduction

(a)

Interpretation:

The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.

Concept introduction:

According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.

For example:

HAH++A

Here, HA is an acid as it donates a proton to form A a conjugate base.

Similarly,

A+H+HA

Here, A is a base as it accepts a proton to from HA which is a conjugate acid.

Explanation of Solution

The given species is NH3.

On reaction with water, it can act as a base by accepting hydrogen ion from the water molecule. The reaction is shown as follows:

NH3+H2ONH4++OH

In the above reaction,

Interpretation Introduction

(b)

Interpretation:

The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.

Concept introduction:

According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.

For example:

HAH++A

Here, HA is an acid as it donates a proton to form A a conjugate base.

Similarly,

A+H+HA

Here, A is a base as it accepts a proton to from HA which is a conjugate acid.

Interpretation Introduction

(c)

Interpretation:

The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.

Concept introduction:

According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.

For example:

HAH++A

Here, HA is an acid as it donates a proton to form A a conjugate base.

Similarly,

A+H+HA

Here, A is a base as it accepts a proton to from HA which is a conjugate acid.

Interpretation Introduction

(d)

Interpretation:

The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.

Concept introduction:

According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.

For example:

HAH++A

Here, HA is an acid as it donates a proton to form A a conjugate base.

Similarly,

A+H+HA

Here, A is a base as it accepts a proton to from HA which is a conjugate acid.

Interpretation Introduction

(e)

Interpretation:

The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.

Concept introduction:

According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.

For example:

HAH++A

Here, HA is an acid as it donates a proton to form A a conjugate base.

Similarly,

A+H+HA

Here, A is a base as it accepts a proton to from HA which is a conjugate acid.

Interpretation Introduction

(f)

Interpretation:

The equation to show the basic nature of the given species in water according to the Bronsted-Lowry model should be written.

Concept introduction:

According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form conjugate base and bases are substances which accepts protons to from conjugate acid.

For example:

HAH++A

Here, HA is an acid as it donates a proton to form A a conjugate base.

Similarly,

A+H+HA

Here, A is a base as it accepts a proton to from HA which is a conjugate acid.

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Chapter 13 Solutions

Chemistry: Principles and Reactions
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Ch. 13 - Using the Brønsted-Lowry model, write an equation...Ch. 13 - Follow the directions of Question 11 for the...Ch. 13 - Find the pH of solutions with the following[ H+ ]....Ch. 13 - Find the pH of solutions with the following[ H+ ]....Ch. 13 - Calculate H+ and OH- and in solutions with the...Ch. 13 - Calculate [H+] and [OH-] in solutions with the...Ch. 13 - Complete the following table for solutions at 25C.Ch. 13 - Complete the following table for solutions at 25C.Ch. 13 - Solution 1 has [ H+ ]=1.7102 M. Solution 2 has [...Ch. 13 - Solution R has pH 13.42. Solution Q has [ OH...Ch. 13 - Consider three solutions, R, Z, and Q. •...Ch. 13 - Solution A has a pH of 12.32. Solution B has [H+]...Ch. 13 - Unpolluted rain water has a pH of about 5.5. Acid...Ch. 13 - Most cola soft drinks have a pH of 3.1. 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It is...Ch. 13 - Selenious acid, H2SeO3, is primarily used to...Ch. 13 - Write the ionization expression and the Kb...Ch. 13 - Follow the instructions for Question 63 for the...Ch. 13 - Using the equilibrium constants in Table 13.2,...Ch. 13 - Follow the directions of Question 65 for the...Ch. 13 - Using the equilibrium constants listed in Table...Ch. 13 - Using the equilibrium constants listed in Table...Ch. 13 - Find the value of Kb for the conjugate base of the...Ch. 13 - Find the values of Kb for the conjugate bases of...Ch. 13 - Determine [OH-], pOH and pH of a 0.28 M aqueous...Ch. 13 - Determine the [OH-] and pH of a 0.72 M solution of...Ch. 13 - Codeine (Cod), a powerful and addictive...Ch. 13 - Consider pyridine, C5H5N, a pesticide and deer...Ch. 13 - A solution of baking soda, NaHCO3, has a pH of...Ch. 13 - A solution of sodium cyanide, NaCN, has a pH of...Ch. 13 - Write formulas for two salts that (a) contain Ni3+...Ch. 13 - Write formulas for two salts that (a) contain NH4+...Ch. 13 - State whether 1 M solutions of the following salts...Ch. 13 - State whether 1 M solutions of the following salts...Ch. 13 - Write net ionic equations to explain the acidity...Ch. 13 - Write net ionic equations to explain the acidity...Ch. 13 - Arrange the following aqueous 0.1 M solutions in...Ch. 13 - Arrange the following aqueous 0.1 M solutions in...Ch. 13 - Unclassified At 25C, a 0.20 M solution of...Ch. 13 - Ammonium chloride is mixed with sodium nitrite. 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