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# Convert the following pH values into both [ H + ] and [ OH − ] values: a. pH = 3 .95 b. pH = 4 .00 c. pH = 11 .86

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### Chemistry for Today: General, Orga...

9th Edition
Spencer L. Seager + 2 others
Publisher: Cengage Learning
ISBN: 9781305960060

#### Solutions

Chapter
Section
BuyFindarrow_forward

### Chemistry for Today: General, Orga...

9th Edition
Spencer L. Seager + 2 others
Publisher: Cengage Learning
ISBN: 9781305960060
Chapter 9, Problem 9.42E
Textbook Problem
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## Convert the following pH values into both [ H + ] and [ OH − ] values:a. pH = 3 .95 b. pH = 4 .00 c. pH = 11 .86

Interpretation Introduction

(a)

Interpretation:

The given pH values are to be converted into both [H+] and [OH].

Concept introduction:

pH of a solution is represented as the negative logarithm of the concentration of protons.

pH=log[H+]

This scale is defined from 1 to 14. It helps to determine whether the given solution is acidic, basic or neutral. The solutions with pH<7 are acidic in nature, with pH=7 are neutral in nature and with pH>7 are basic in nature.

### Explanation of Solution

pH is used to calculate the concentrations of H3O+ and OH.

pH=log[H+][H+]=1×10pH

The pH of the given solution is 3.95.

[H+]=1×103.95mol/L[H+]=1.1×104mol/L

Thus, the [H+] value for the given solution is 1.1×104mol/L.

The concentration of OH is calculated by,

Kw=[H3O+][OH]

Substitute the value of ionization constant and concentration of H3O+ in the given formula

Interpretation Introduction

(b)

Interpretation:

The given pH values are to be converted into both [H+] and [OH].

Concept introduction:

pH of a solution is represented as the negative logarithm of the concentration of protons.

pH=log[H+]

This scale is defined from 1 to 14. It helps to determine whether the given solution is acidic, basic or neutral. The solutions with pH<7 are acidic in nature, with pH=7 are neutral in nature and with pH>7 are basic in nature.

Interpretation Introduction

(c)

Interpretation:

The given pH values are to be converted into both [H+] and [OH].

Concept introduction:

pH of a solution is represented as the negative logarithm of the concentration of protons.

pH=log[H+]

This scale is defined from 1 to 14. It helps to determine whether the given solution is acidic, basic or neutral. The solutions with pH<7 are acidic in nature, with pH=7 are neutral in nature and with pH>7 are basic in nature.

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