If I add water to 250 mL of a 0.4 M Tang solution until the final volume is 500 mL, what will the molarity of the diluted solution be?

To determine the new molarity of the Tang solution after dilution, we can use the formula for dilution:

\[
M_1 V_1 = M_2 V_2
\]

where:
- \( M_1 \) is the initial molarity (0.4 M),
- \( V_1 \) is the initial volume (250 mL),
- \( M_2 \) is the final molarity (what we are trying to find),
- \( V_2 \) is the final volume (500 mL).

Plugging in the values:

\[
0.4 \, \text{M} \times 250 \, \text{mL} = M_2 \times 500 \, \text{mL}
\]

Solving for \( M_2 \):

\[
M_2 = \frac{0.4 \times 250}{500} = \frac{100}{500} = 0.2 \, \text{M}
\]

So, the molarity of the diluted solution is **0.2 M**.

Would you like a deeper explanation or have any other questions?

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1. How does changing the volume affect molarity in a solution?
2. What would the final molarity be if the volume was increased to 750 mL instead?
3. How does the dilution formula \(M_1V_1 = M_2V_2\) apply to real-world chemical solutions?
4. How would you calculate the amount of Tang needed to create a solution of a specific molarity?
5. What are some common applications of dilutions in chemistry?

**Tip:** Always double-check your units, especially when working with different volumes and concentrations.

Learn how to determine the molarity of a diluted Tang solution. This step-by-step guide uses the dilution formula (M1 * V1 = M2 * V2) to solve a real-world chemistry problem involving initial and final volumes of 250 mL and 500 mL. Perfect for high school students studying chemistry.

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