A solution made by mixing 50 .0 m L of 0.050 M NaHCO 3 and 0.10 mL of 0.10 M sodium hydroxide p H has to be calculated. Concept Introduction: pH definition: The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion [H 3 O + ] concentration. pH = -log[H 3 O + ] Henderson-Hasselbalch equation: The pH at an intermediate stage of the titration is calculated by using the following equation, pH = pK a + log [ base ] [ acid ] where, pH = - log [ H + ] pK a = - log K a ( K a - acid dissociation constant ) This equation is known as Henderson-Hasselbalch equation.

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Answer 1

Question

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

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Answer 2

Question

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

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Answer 3

Question

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

Expert Solution & Answer

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Answer 4

Question

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

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Answer 5

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

Answer 6

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

Answer 7

Chapter 19, Problem 19.33P

(a)

Interpretation Introduction

Interpretation:

A solution made by mixing $50.0 mL$ of $0.050 M NaHCO3$ and $0.10 mL$ of $0.10 M$ sodium hydroxide $pH$ has to be calculated.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Henderson-Hasselbalch equation:

The $pH$ at an intermediate stage of the titration is calculated by using the following equation,

$pH = pKa + log [base][acid]where, pH = - log [H+] pKa = - log Ka (Ka - acid dissociation constant)$

This equation is known as Henderson-Hasselbalch equation.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The amount of $HCl$ must be added to $25.0 mL$ of the buffer change the $pH$ by $0.07$ units has to be identified.

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion $[H3O+]$ concentration.

$pH = -log[H3O+]$

Buffer solution:

Buffer solution is defined as a solution that oppose changes in $pH$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $pH$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 19.1 - Calculate the pH of a buffer consisting of 0.50 M...Ch. 19.1 - Prob. 19.1BFP Ch. 19.1 - Prob. 19.2AFP Ch. 19.1 - The molecular scenes below show three samples of a...Ch. 19.1 - Prob. 19.3AFP Ch. 19.1 - What is the component concentration ratio, [NH3]/...Ch. 19.2 - A chemist titrates 20.00 mL of 0.2000 M HBrO (Ka =...Ch. 19.2 - For the titration of 30.00 mL of 0.1000 M benzoic...Ch. 19.3 - Write the ion-product expression at equilibrium...Ch. 19.3 - Prob. 19.5BFP

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