Answer :
Certainly! Let's interpret and analyze the data on the pH readings of various solutions. Here is a detailed, step-by-step solution:
### Step-by-Step Analysis:
1. Understanding pH Scale:
- The pH scale measures the acidity or basicity of a solution.
- A pH of 7 is considered neutral.
- Values less than 7 indicate acidity, while values greater than 7 indicate basicity.
2. Identifying the Solutions:
- Acids have pH values less than 7.
- Bases have pH values greater than 7.
- Salts can have varying pH depending on their composition.
3. Interpreting the Data:
- We will list each solution and its corresponding pH reading to determine if it's acidic, neutral, or basic.
### Data Analysis:
1. [tex]$0.1 M HCl$[/tex]:
- pH reading: 0.1
- This is significantly less than 7, indicating a very strong acid.
2. [tex]$0.01 M HCl$[/tex]:
- pH reading: 1.1
- This is also much less than 7, indicating a strong acid, though less concentrated than the [tex]$0.1 M HCl$[/tex].
3. [tex]$0.1 M Na_2CO_3$[/tex]:
- pH reading: 10.3
- This reading is greater than 7, indicating that [tex]$Na_2CO_3$[/tex] is a basic solution.
4. [tex]$0.1 M NaOH$[/tex]:
- pH reading: 13.0
- This reading is much greater than 7, indicating a very strong base.
5. [tex]$0.1 M HC_2H_3O_2$[/tex] (Acetic Acid):
- pH reading: 2.8
- This is less than 7, indicating that [tex]$HC_2H_3O_2$[/tex] is an acid, though it is a weak acid compared to HCl.
6. [tex]$0.01 M HC_2H_3O_2$[/tex] (Acetic Acid):
- pH reading: 3.6
- This reading is also less than 7, indicating it remains acidic but is weaker due to lower concentration.
7. [tex]$0.1 M NaHCO_3$[/tex]:
- pH reading: 8.2
- This reading is slightly greater than 7, indicating [tex]$NaHCO_3$[/tex] is a basic solution, but not as strong as [tex]$NaOH$[/tex] or [tex]$Na_2CO_3$[/tex].
Here's a concise summary of the pH readings:
- Acidic Solutions (pH < 7):
- [tex]$0.1 M HCl$[/tex]: pH = 0.1
- [tex]$0.01 M HCl$[/tex]: pH = 1.1
- [tex]$0.1 M HC_2H_3O_2$[/tex]: pH = 2.8
- [tex]$0.01 M HC_2H_3O_2$[/tex]: pH = 3.6
- Basic Solutions (pH > 7):
- [tex]$0.1 M Na_2CO_3$[/tex]: pH = 10.3
- [tex]$0.1 M NaOH$[/tex]: pH = 13.0
- [tex]$0.1 M NaHCO_3$[/tex]: pH = 8.2
### Conclusion:
- The data shows a range of acidic and basic solutions, with [tex]$HCl$[/tex] being the strongest acid and [tex]$NaOH$[/tex] being the strongest base among the given solutions.
- Acidity and basicity are also affected by the concentration of the solution, as seen in the difference between [tex]$0.1 M$[/tex] and [tex]$0.01 M$[/tex] acetic acid solutions.
This analysis allows us to categorize and better understand the chemical nature of each solution based on their pH readings.
### Step-by-Step Analysis:
1. Understanding pH Scale:
- The pH scale measures the acidity or basicity of a solution.
- A pH of 7 is considered neutral.
- Values less than 7 indicate acidity, while values greater than 7 indicate basicity.
2. Identifying the Solutions:
- Acids have pH values less than 7.
- Bases have pH values greater than 7.
- Salts can have varying pH depending on their composition.
3. Interpreting the Data:
- We will list each solution and its corresponding pH reading to determine if it's acidic, neutral, or basic.
### Data Analysis:
1. [tex]$0.1 M HCl$[/tex]:
- pH reading: 0.1
- This is significantly less than 7, indicating a very strong acid.
2. [tex]$0.01 M HCl$[/tex]:
- pH reading: 1.1
- This is also much less than 7, indicating a strong acid, though less concentrated than the [tex]$0.1 M HCl$[/tex].
3. [tex]$0.1 M Na_2CO_3$[/tex]:
- pH reading: 10.3
- This reading is greater than 7, indicating that [tex]$Na_2CO_3$[/tex] is a basic solution.
4. [tex]$0.1 M NaOH$[/tex]:
- pH reading: 13.0
- This reading is much greater than 7, indicating a very strong base.
5. [tex]$0.1 M HC_2H_3O_2$[/tex] (Acetic Acid):
- pH reading: 2.8
- This is less than 7, indicating that [tex]$HC_2H_3O_2$[/tex] is an acid, though it is a weak acid compared to HCl.
6. [tex]$0.01 M HC_2H_3O_2$[/tex] (Acetic Acid):
- pH reading: 3.6
- This reading is also less than 7, indicating it remains acidic but is weaker due to lower concentration.
7. [tex]$0.1 M NaHCO_3$[/tex]:
- pH reading: 8.2
- This reading is slightly greater than 7, indicating [tex]$NaHCO_3$[/tex] is a basic solution, but not as strong as [tex]$NaOH$[/tex] or [tex]$Na_2CO_3$[/tex].
Here's a concise summary of the pH readings:
- Acidic Solutions (pH < 7):
- [tex]$0.1 M HCl$[/tex]: pH = 0.1
- [tex]$0.01 M HCl$[/tex]: pH = 1.1
- [tex]$0.1 M HC_2H_3O_2$[/tex]: pH = 2.8
- [tex]$0.01 M HC_2H_3O_2$[/tex]: pH = 3.6
- Basic Solutions (pH > 7):
- [tex]$0.1 M Na_2CO_3$[/tex]: pH = 10.3
- [tex]$0.1 M NaOH$[/tex]: pH = 13.0
- [tex]$0.1 M NaHCO_3$[/tex]: pH = 8.2
### Conclusion:
- The data shows a range of acidic and basic solutions, with [tex]$HCl$[/tex] being the strongest acid and [tex]$NaOH$[/tex] being the strongest base among the given solutions.
- Acidity and basicity are also affected by the concentration of the solution, as seen in the difference between [tex]$0.1 M$[/tex] and [tex]$0.01 M$[/tex] acetic acid solutions.
This analysis allows us to categorize and better understand the chemical nature of each solution based on their pH readings.
