3. Why is it proper to read the initial volume of the buret instead of trying to adjust the volume to a round number such as 0 mL? 4. Calculate the molarity of a NaOH solution if 23.25 mL of NaOH is titrated with 0.475 grams of KHP and 1.25 mL of 0.100 M HCI is required.
3. Why is it proper to read the initial volume of the buret instead of trying to adjust the volume to a round number such as 0 mL? 4. Calculate the molarity of a NaOH solution if 23.25 mL of NaOH is titrated with 0.475 grams of KHP and 1.25 mL of 0.100 M HCI is required.
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![### Reading Initial Volume and Molarity Calculations
#### 3. Importance of Reading Initial Volume from the Buret
When performing titration experiments, it is crucial to read the initial volume of the buret accurately, rather than trying to adjust the volume to a round number like 0 mL. This precision ensures that all calculated measurements are based on true initial readings, thereby eliminating potential inaccuracies that could arise from attempting to adjust the liquid to a specific mark. Accurate initial volume recordings contribute to the reliability and reproducibility of the experiment's results.
#### 4. Calculating Molarity of NaOH Solution
To find the molarity of a NaOH (Sodium Hydroxide) solution, follow these steps:
- The data given:
- Volume of NaOH solution: 23.25 mL
- Mass of KHP (Potassium hydrogen phthalate): 0.475 grams
- Volume of HCl (Hydrochloric acid) solution: 1.25 mL with 0.100 M concentration
- Steps:
- Convert the volume of NaOH to liters: \( 23.25 \, \text{mL} = 0.02325 \, \text{L} \)
- Convert the mass of KHP to moles using the molar mass of KHP (approximately 204.22 g/mol):
\[
\text{Moles of KHP} = \frac{0.475 \, \text{g}}{204.22 \, \text{g/mol}} \approx 0.002325 \, \text{moles}
\]
- Since HCl is fully ionized in solution, the moles of NaOH is equal to the moles of KHP in the titration reaction:
\[
\text{Moles of NaOH} = 0.002325 \, \text{moles}
\]
- Calculate molarity (M) using the formula \( M = \frac{\text{moles}}{\text{liters}} \):
\[
\text{Molarity of NaOH} = \frac{0.002325 \, \text{moles}}{0.02325 \, \text{L}} = 0.10 \, \text{M}
\]
The molarity of the Na](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6ae95cc5-a0cd-43b0-8331-9678c9dacca0%2Fc78d646f-3c1f-4d39-a684-c2e07cec00b6%2Fa95yoe8.jpeg&w=3840&q=75)
Transcribed Image Text:### Reading Initial Volume and Molarity Calculations
#### 3. Importance of Reading Initial Volume from the Buret
When performing titration experiments, it is crucial to read the initial volume of the buret accurately, rather than trying to adjust the volume to a round number like 0 mL. This precision ensures that all calculated measurements are based on true initial readings, thereby eliminating potential inaccuracies that could arise from attempting to adjust the liquid to a specific mark. Accurate initial volume recordings contribute to the reliability and reproducibility of the experiment's results.
#### 4. Calculating Molarity of NaOH Solution
To find the molarity of a NaOH (Sodium Hydroxide) solution, follow these steps:
- The data given:
- Volume of NaOH solution: 23.25 mL
- Mass of KHP (Potassium hydrogen phthalate): 0.475 grams
- Volume of HCl (Hydrochloric acid) solution: 1.25 mL with 0.100 M concentration
- Steps:
- Convert the volume of NaOH to liters: \( 23.25 \, \text{mL} = 0.02325 \, \text{L} \)
- Convert the mass of KHP to moles using the molar mass of KHP (approximately 204.22 g/mol):
\[
\text{Moles of KHP} = \frac{0.475 \, \text{g}}{204.22 \, \text{g/mol}} \approx 0.002325 \, \text{moles}
\]
- Since HCl is fully ionized in solution, the moles of NaOH is equal to the moles of KHP in the titration reaction:
\[
\text{Moles of NaOH} = 0.002325 \, \text{moles}
\]
- Calculate molarity (M) using the formula \( M = \frac{\text{moles}}{\text{liters}} \):
\[
\text{Molarity of NaOH} = \frac{0.002325 \, \text{moles}}{0.02325 \, \text{L}} = 0.10 \, \text{M}
\]
The molarity of the Na
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