A sample of the unknown solution is now diluted from an initial volume of 2.00 mL to a final volume of 25.00  mL. If the diluted solution has an absorbance of 0.73 x 10^3 then the concentration of A in the initial solution is

To find the concentration of substance \( A \) in the initial solution, we can apply the concept of dilution. The dilution formula is:

\[
C_1 V_1 = C_2 V_2
\]

where:
- \( C_1 \) is the concentration of the initial solution,
- \( V_1 \) is the initial volume,
- \( C_2 \) is the concentration of the diluted solution,
- \( V_2 \) is the final volume.

Since we know the volumes \( V_1 = 2.00 \, \text{mL} \) and \( V_2 = 25.00 \, \text{mL} \), we need to find \( C_1 \), the initial concentration.

The absorbance value given (0.73 x \(10^3\)) is related to concentration by Beer-Lambert’s Law:

\[
A = \epsilon \cdot c \cdot l
\]

where:
- \( A \) is absorbance,
- \( \epsilon \) is the molar absorptivity (or extinction coefficient),
- \( c \) is the concentration of the solution,
- \( l \) is the path length of the sample cell.

To proceed, we need the molar absorptivity (\( \epsilon \)) and the path length (\( l \)) to find \( C_2 \). Once \( C_2 \) is known, we can use the dilution formula to determine \( C_1 \).

Could you provide the values for \( \epsilon \) and \( l \) or confirm that they are standard values? 

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Would you like a breakdown of the Beer-Lambert Law or more help with these calculations? 

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**Follow-up Questions:**
1. What is Beer-Lambert’s Law, and how does it relate absorbance to concentration?
2. How would changes in the path length \( l \) affect the concentration calculation?
3. What steps are involved in calculating the concentration when only volumes and absorbance are given?
4. How can one experimentally determine the molar absorptivity \( \epsilon \)?
5. What is the significance of dilution in determining the concentration of a solution?

**Tip:** Always ensure units are consistent when using the dilution formula.

A sample of the unknown solution is now diluted from an initial volume of 2.00 mL to a final volume of 25.00 mL. If the diluted solution has an absorbance of 0.73 x 10^3, then the concentration of A in the initial solution is

Learn how to calculate the initial concentration of a solution using the dilution formula and Beer-Lambert Law. This problem involves diluting a solution from 2.00 mL to 25.00 mL and using an absorbance of 0.73 x 10^3 to find the initial concentration. Suitable for students in Grades 10-12.

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