https://file.aiquickdraw.com/mathbot/file/1729830711790u3rxl2nm.jpg

To solve this problem, we will use the dilution equation:

\[
C_1 V_1 = C_2 V_2
\]

Where:
- \(C_1\) is the initial concentration (6.0 M),
- \(V_1\) is the initial volume (25 mL),
- \(C_2\) is the final concentration (what we are trying to find),
- \(V_2\) is the final volume (750 mL).

Rearranging the equation to solve for \(C_2\):

\[
C_2 = \frac{C_1 V_1}{V_2}
\]

Substituting the values:

\[
C_2 = \frac{6.0 \, \text{M} \times 25 \, \text{mL}}{750 \, \text{mL}} = \frac{150}{750} = 0.2 \, \text{M}
\]

So, the final concentration is **0.2 M**.

Would you like more details or have any further questions?

Here are five related questions to expand this topic:
1. How does changing the final volume affect the concentration of the solution?
2. What happens to the concentration if the initial volume is doubled?
3. How would the process change if the substance is not HCl but a different acid or base?
4. Can you calculate the final concentration if the dilution involves adding more than one substance?
5. What is the difference between a molarity-based dilution and a mass-based dilution?

**Tip:** When performing dilutions, always make sure the units for volume are consistent throughout the calculation.

What is the concentration of a solution made by diluting 25 mL of 6.0 M HCl to a final volume of 750 mL?

Find the concentration of a solution made by diluting 25 mL of 6.0 M HCl to 750 mL. Learn to apply the dilution equation (C1V1 = C2V2) to calculate the final concentration of 0.2 M. Suitable for students in Grades 9-12.

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