hat is the molarity of a solution that contains 0.505 mol KCl (molar mass = 74.55 g/mol) in 7.98 L of solution?

To find the molarity (M) of a solution, you can use the formula:

\[
M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}
\]

Given:
- Moles of KCl = 0.505 mol
- Volume of solution = 7.98 L

Now, applying the values to the formula:

\[
M = \frac{0.505 \, \text{mol}}{7.98 \, \text{L}} = 0.0633 \, \text{M}
\]

So, the molarity of the solution is **0.0633 M**.

Would you like further details or have any questions about this process?

Here are five related questions for further exploration:
1. How does temperature affect the molarity of a solution?
2. How do you prepare a solution with a specific molarity?
3. What is the relationship between molarity and concentration?
4. How does the concept of molality differ from molarity?
5. How would you calculate the molarity of a diluted solution?

**Tip:** Always ensure that the volume used in molarity calculations is in liters (L), not milliliters (mL).

What is the molarity of a solution that contains 0.505 mol KCl (molar mass = 74.55 g/mol) in 7.98 L of solution?

Find out how to calculate the molarity of a solution containing 0.505 mol KCl in 7.98 L of solution. This example demonstrates the key concepts of molarity and concentration calculations, suitable for high school chemistry students (Grades 9-12).

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