(a) Interpretation: The pH value for a solution in which [H + ] = 1.0 × 10 − 3 M should be calculated at 25 ° C . Concept Introduction: To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of [H + ] in aqueous solution is small, by using the p scale in the form of pH scale, it is better way to represent acidity of solution. Thus, pH = -log [H + ] And, at 25 ° C , the actual concentrations of the products are: [H + ][OH − ]=1 × 10 − 14 The mathematical product of both [H + ] and [OH − ] concentrations are always constant known as ion product constant ( K w ) [H + ][OH − ]=1 × 10 − 14 = K w .

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Answer 1

Question

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

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Answer 2

Question

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

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Answer 3

Question

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

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Answer 4

Question

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

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Answer 5

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Answer 6

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Answer 7

Chapter 16.4, Problem 16.3SC

Interpretation Introduction

(a)

Interpretation:

The $pH$ value for a solution in which $[H+]$ = $1.0×10−3M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Answer 8

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Answer 9

Interpretation Introduction

(b)

Interpretation:

The $pH$ value for a solution in which $[OH−]$ = $5.0×10−5M$ should be calculated at $25°C$ .

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of $[H+]$ in aqueous solution is small, by using the p scale in the form of $pH$ scale, it is better way to represent acidity of solution.

Thus, $pH$ = $-log [H+]$

And, at $25°C$ , the actual concentrations of the products are:

$[H+][OH−]=1×10−14$

The mathematical product of both $[H+]$ and $[OH−]$ concentrations are always constant known as ion product constant ( $Kw$ )

$[H+][OH−]=1×10−14=Kw$ .

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 16.1 - Exercise 16.1 Which of the following represent...Ch. 16.2 - Vinegar contains acetic acid and is used in salad...Ch. 16.3 - Exercise 16.2 Calculate [H+] in a solution in...Ch. 16.4 - Prob. 16.3SC Ch. 16.4 - Prob. 1CT Ch. 16.4 - Prob. 16.4SC Ch. 16.4 - Exercise 16.5 The pH of rainwater in a polluted...Ch. 16.4 - Exercise 16.6 The pOH of a liquid drain cleaner...Ch. 16.5 - Exercise 16.7 Calculate the pH of a solution of...Ch. 16 - You are asked for the H+ concentration in a...

Solution Summary: The author explains that the value of pH for a solution in which = 1.0times.

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