If a liter of a 0.5 M solution is added to another solution to make a total of 2 liters, what will the concentration of the final solution be?

To solve this problem, we use the concept of dilution and the formula for concentration:

\[
C_1 V_1 = C_2 V_2
\]

Where:
- \( C_1 \) is the initial concentration (0.5 M),
- \( V_1 \) is the initial volume (1 liter),
- \( C_2 \) is the final concentration (what we are solving for),
- \( V_2 \) is the final volume (2 liters).

Now, rearrange the formula to solve for \( C_2 \):

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

Substitute the values:

\[
C_2 = \frac{0.5 \, \text{M} \times 1 \, \text{L}}{2 \, \text{L}} = \frac{0.5}{2} = 0.25 \, \text{M}
\]

So, the concentration of the final solution will be **0.25 M**.

Would you like more details on the solution process?

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Here are some related questions to further your understanding:

1. How would the concentration change if 3 liters were the final volume instead of 2 liters?
2. What would happen if the initial solution were 1 M instead of 0.5 M?
3. How can you calculate the mass of solute in the final solution if you know the molar mass?
4. What if a certain amount of solute is added instead of dilution by volume—how does this affect concentration?
5. How does temperature affect the molarity of a solution?

**Tip:** When diluting a solution, remember that the amount of solute remains constant—only the volume changes.

Learn how to calculate the final concentration of a solution after dilution. This problem involves the key concepts of molarity and dilution, using the formula C1 * V1 = C2 * V2. Suitable for high school students in Grades 10-12.

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