Using the formulas provided in the image, fill in the missing areas in the table: pH: pOH: 8.5 [H+]: [OH-]: pH: 3.7 pOH: [H+]: [OH-]: pH: pOH: [H+]: [OH-]: 3.2 x 10-8 pH: pOH: [H+]: 1.7 x 10-3 [OH-]:
Using the formulas provided in the image, fill in the missing areas in the table: pH: pOH: 8.5 [H+]: [OH-]: pH: 3.7 pOH: [H+]: [OH-]: pH: pOH: [H+]: [OH-]: 3.2 x 10-8 pH: pOH: [H+]: 1.7 x 10-3 [OH-]:
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
Using the formulas provided in the image, fill in the missing areas in the table:
pH:
pOH: 8.5
[H+]:
[OH-]:
pH: 3.7
pOH:
[H+]:
[OH-]:
pH:
pOH:
[H+]:
[OH-]: 3.2 x 10-8
pH:
pOH:
[H+]: 1.7 x 10-3
[OH-]:
![**Transcription with Diagram Explanation**
---
### Text:
When the solution turns ~neutral, using an indicator, the concentration in molarity of the unknown acid or base can be calculated using the formula:
\[ M = \text{molarity}, V = \text{volume and } a = \text{acid and } b = \text{base} \]
The value is either Ma (if the unknown is an acid) or Mb (if the unknown is a base).
The unknown can then be used to calculate either pH or pOH. From either H⁺ or OH⁻ is known, pH/pOH can be calculated using the box below:
### Diagram Explanation:
The diagram visually represents the relationships and conversions between pH, pOH, [H⁺], and [OH⁻].
- **Left Side**:
- Shows the relationship between [H⁺] concentration and pH.
- The equation \([H^+] = \frac{1 \times 10^{-14}}{[OH^-]}\) is used to calculate [H⁺].
- An arrow indicates that \(pH = -\log[H^+]\).
- **Right Side**:
- Shows the relationship between [OH⁻] concentration and pOH.
- The equation \([OH^-] = \frac{1 \times 10^{-14}}{[H^+]}\) is used to calculate [OH⁻].
- An arrow indicates that \(pOH = -\log[OH^-]\).
- **Bottom Arrows**:
- Indicate that \(pOH = 14 - pH\) and \(pH = 14 - pOH\).
**Summary**:
The dissociation of the acid or base in water must be considered. For example, a 0.2 M NaOH solution has an effective basic concentration of 0.4 M, because the base dissociates fully. A 0.2 M H₃PO₄ solution has an effective acid concentration of 0.6 M, because the acid dissociates partially. An alternative base/acid concentration, only used in titrations, where the M of either \(H^+\) or \(OH^-\) ions, is called Normality (covered in the Solutions worksheet).
### Equipment Table:
| Flask | Burette and B](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9c9a1d07-5dae-4ff1-9545-cf26beba5570%2Fe6be967b-d53a-4317-ab6b-a786739cc225%2F8ezqj5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription with Diagram Explanation**
---
### Text:
When the solution turns ~neutral, using an indicator, the concentration in molarity of the unknown acid or base can be calculated using the formula:
\[ M = \text{molarity}, V = \text{volume and } a = \text{acid and } b = \text{base} \]
The value is either Ma (if the unknown is an acid) or Mb (if the unknown is a base).
The unknown can then be used to calculate either pH or pOH. From either H⁺ or OH⁻ is known, pH/pOH can be calculated using the box below:
### Diagram Explanation:
The diagram visually represents the relationships and conversions between pH, pOH, [H⁺], and [OH⁻].
- **Left Side**:
- Shows the relationship between [H⁺] concentration and pH.
- The equation \([H^+] = \frac{1 \times 10^{-14}}{[OH^-]}\) is used to calculate [H⁺].
- An arrow indicates that \(pH = -\log[H^+]\).
- **Right Side**:
- Shows the relationship between [OH⁻] concentration and pOH.
- The equation \([OH^-] = \frac{1 \times 10^{-14}}{[H^+]}\) is used to calculate [OH⁻].
- An arrow indicates that \(pOH = -\log[OH^-]\).
- **Bottom Arrows**:
- Indicate that \(pOH = 14 - pH\) and \(pH = 14 - pOH\).
**Summary**:
The dissociation of the acid or base in water must be considered. For example, a 0.2 M NaOH solution has an effective basic concentration of 0.4 M, because the base dissociates fully. A 0.2 M H₃PO₄ solution has an effective acid concentration of 0.6 M, because the acid dissociates partially. An alternative base/acid concentration, only used in titrations, where the M of either \(H^+\) or \(OH^-\) ions, is called Normality (covered in the Solutions worksheet).
### Equipment Table:
| Flask | Burette and B
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