The acidic and basic nature should be determined given the resulting solution of the statement. Concept introduction: Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower p H for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution. pKa: It is introduced as an index to express the acidity of weak acids, where p K a is defined as fallows, we consider the K a constant for acetic acid 1.8 × 10 − 5 ( p K a ) but p K a constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid. An acid-base reaction reaction is represented as written below. HA ( aq ) + B ( aq ) ⇌ BH + ( aq ) + A − ( aq ) ( acid ) ( base ) ( conjugate acid ) ( conjugate base ) The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants ( K a and K b ) for reactants as well as of the products. The more the value of K a for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of K b for a base, stronger will be the base and it will undergo faster ionization.

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Answer 1

Question

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

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Draw the stepwise mechanism for the reactions

Answer 2

Question

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

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Answer 3

Question

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

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Answer 4

Question

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

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Answer 5

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

Answer 6

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

Answer 7

Chapter 16.6, Problem 3RC

Interpretation Introduction

Interpretation:

The acidic and basic nature should be determined given the resulting solution of the statement.

Concept introduction:

Strong acid: Acid solutions contains hydrigen ions, the higher concentration of hydrogen ions, the lower $pH$ for example hydrochloric acid is strong acid when comapre to acetic acid it is a weakr acid. Hence srong acids are completely ionizaes but weak acids are only partly ionizaed in the solution.

pKa: It is introduced as an index to express the acidity of weak acids, where $pKa$ is defined as fallows, we consider the $Ka$ constant for acetic acid $1.8×10−5 (pKa)$ but $pKa$ constant for is 4.8 which is a simpler expression. Furthermore the smaller pKa value has strongest acid.

An acid-base reaction reaction is represented as written below.

$HA(aq)+B(aq) ⇌ BH+(aq) + A−(aq)(acid) (base) (conjugate acid) (conjugate base)$

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants $(Kaand Kb)$ for reactants as well as of the products. The more the value of $Ka$ for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of $Kb$ for a base, stronger will be the base and it will undergo faster ionization.

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Answer 11

Ch. 16.1 - 1. H3PO4 phosphoric acid, can donate two protons...Ch. 16.1 - 2. The cyanide ion, CN−, accepts a proton from...Ch. 16.1 - 3. In the following reaction, identify the acid on...Ch. 16.1 - Prob. 4RC Ch. 16.2 - What are the hydronium ion and hydroxide ion...Ch. 16.2 - What is the pH of a 0.0012 M NaOH solution at 25C?...Ch. 16.2 - The pH of a diet soda is 432 at 25C. What is the...Ch. 16.2 - If the pH of a solution containing the strong base...Ch. 16.3 - Prob. 1RC Ch. 16.3 - Which acid has the strongest conjugate base? (a)...

Solution Summary: The author explains that acidic and basic nature should be determined given the resulting solution of the statement.

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