▼ ▼ Submit Part B A solution has [H3O+] = 1.6x10-5 M. Use the ion product constant of water Kw= [H3O+][OH-] to find the [OH-] of the solution. Express your answer to two significant figures. View Available Hint(s) [OH-] = Submit Part C ΑΣΦ 1 to find the [H3O+] of the solution. Express your answer to two significant figures. View Available Hint(s) [H3O+] = A solution has [OH-] = 1.3x10-2 M. Use the ion product constant of water Kw= = [H3O+][OH-] ? —| ΑΣΦ M ? M
▼ ▼ Submit Part B A solution has [H3O+] = 1.6x10-5 M. Use the ion product constant of water Kw= [H3O+][OH-] to find the [OH-] of the solution. Express your answer to two significant figures. View Available Hint(s) [OH-] = Submit Part C ΑΣΦ 1 to find the [H3O+] of the solution. Express your answer to two significant figures. View Available Hint(s) [H3O+] = A solution has [OH-] = 1.3x10-2 M. Use the ion product constant of water Kw= = [H3O+][OH-] ? —| ΑΣΦ M ? M
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![**Part B**
A solution has \([H_3O^+] = 1.6 \times 10^{-5}\ M\). Use the ion product constant of water:
\[ K_w = [H_3O^+][OH^-] \]
to find the \([OH^-]\) of the solution.
Express your answer to two significant figures.
[Input Box for OH- concentration] M
**Part C**
A solution has \([OH^-] = 1.3 \times 10^{-2}\ M\). Use the ion product constant of water:
\[ K_w = [H_3O^+][OH^-] \]
to find the \([H_3O^+]\) of the solution.
Express your answer to two significant figures.
[Input Box for H3O+ concentration] M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3%2F94799fc4-dbf4-4869-ba7f-5f0f66fadc4c%2Fmmu7l7g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Part B**
A solution has \([H_3O^+] = 1.6 \times 10^{-5}\ M\). Use the ion product constant of water:
\[ K_w = [H_3O^+][OH^-] \]
to find the \([OH^-]\) of the solution.
Express your answer to two significant figures.
[Input Box for OH- concentration] M
**Part C**
A solution has \([OH^-] = 1.3 \times 10^{-2}\ M\). Use the ion product constant of water:
\[ K_w = [H_3O^+][OH^-] \]
to find the \([H_3O^+]\) of the solution.
Express your answer to two significant figures.
[Input Box for H3O+ concentration] M
![# Calculating \([H_3O^+]\) and \([OH^-]\) in Solutions
## Overview
The ion product constant of water reveals that a solution's concentrations of hydronium ion \([H_3O^+]\) and hydroxide ion \([OH^-]\) are inversely proportional since they are on the same side of the equation. If a solution's concentration of \([H_3O^+]\) increases, then its concentration of \([OH^-]\) decreases. Similarly, if a solution's concentration of \([H_3O^+]\) decreases, then its concentration of \([OH^-]\) increases. This section also reveals that if the concentration of either the hydronium ion or the hydroxide ion is known, then the concentration of the other can be calculated using the ion product constant of water.
## Part A
Determine whether the following hydroxide ion concentrations \([OH^-]\) correspond to acidic, basic, or neutral solutions by estimating their corresponding hydronium ion concentrations \([H_3O^+]\) using the ion product constant of water \((K_w)\).
### Table: Relationship between Hydronium Ion Concentration and Solution Condition
| Hydronium ion concentration \([H_3O^+]\) | Solution condition |
|------------------------------------------|--------------------|
| Greater than \(1 \times 10^{-7} M\) | Acidic |
| Equal to \(1 \times 10^{-7} M\) | Neutral |
| Less than \(1 \times 10^{-7} M\) | Basic |
### Task
Place the hydroxide ion concentrations into the correct categories based on the solution condition:
- \([OH^-] = 4 \times 10^{-12} M\)
- \([OH^-] = 3 \times 10^{-9} M\)
- \([OH^-] = 8 \times 10^{-10} M\)
- \([OH^-] = 4 \times 10^{-13} M\)
- \([OH^-] = 2 \times 10^{-2} M\)
- \([OH^-] = 7 \times 10^{-4} M\)
- \([OH^-] = 5 \times 10^{-5} M\)
- \([OH^-]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3%2F94799fc4-dbf4-4869-ba7f-5f0f66fadc4c%2F9xewfme_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Calculating \([H_3O^+]\) and \([OH^-]\) in Solutions
## Overview
The ion product constant of water reveals that a solution's concentrations of hydronium ion \([H_3O^+]\) and hydroxide ion \([OH^-]\) are inversely proportional since they are on the same side of the equation. If a solution's concentration of \([H_3O^+]\) increases, then its concentration of \([OH^-]\) decreases. Similarly, if a solution's concentration of \([H_3O^+]\) decreases, then its concentration of \([OH^-]\) increases. This section also reveals that if the concentration of either the hydronium ion or the hydroxide ion is known, then the concentration of the other can be calculated using the ion product constant of water.
## Part A
Determine whether the following hydroxide ion concentrations \([OH^-]\) correspond to acidic, basic, or neutral solutions by estimating their corresponding hydronium ion concentrations \([H_3O^+]\) using the ion product constant of water \((K_w)\).
### Table: Relationship between Hydronium Ion Concentration and Solution Condition
| Hydronium ion concentration \([H_3O^+]\) | Solution condition |
|------------------------------------------|--------------------|
| Greater than \(1 \times 10^{-7} M\) | Acidic |
| Equal to \(1 \times 10^{-7} M\) | Neutral |
| Less than \(1 \times 10^{-7} M\) | Basic |
### Task
Place the hydroxide ion concentrations into the correct categories based on the solution condition:
- \([OH^-] = 4 \times 10^{-12} M\)
- \([OH^-] = 3 \times 10^{-9} M\)
- \([OH^-] = 8 \times 10^{-10} M\)
- \([OH^-] = 4 \times 10^{-13} M\)
- \([OH^-] = 2 \times 10^{-2} M\)
- \([OH^-] = 7 \times 10^{-4} M\)
- \([OH^-] = 5 \times 10^{-5} M\)
- \([OH^-]
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