A solution is prepared by dissolving 3.6 g of methanol  (CH3OH,  Molar mass = 32.04g/mol) into water and form 100 mL solution.  Calculate the **molarity** of Methanol in this solution

To calculate the **molarity** of methanol in the solution, we use the formula:

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

### Step 1: Calculate the moles of methanol
The moles of methanol can be calculated using its mass and molar mass:

\[
\text{moles of methanol} = \frac{\text{mass of methanol}}{\text{molar mass of methanol}} = \frac{3.6\text{ g}}{32.04\text{ g/mol}}
\]

\[
\text{moles of methanol} \approx 0.1123 \text{ mol}
\]

### Step 2: Convert the volume of the solution to liters
Since the solution is 100 mL, we convert it to liters:

\[
\text{volume in liters} = \frac{100}{1000} = 0.100 \text{ L}
\]

### Step 3: Calculate the molarity
Now, substitute the moles of methanol and the volume of the solution into the molarity formula:

\[
\text{Molarity} = \frac{0.1123 \text{ mol}}{0.100 \text{ L}} = 1.123 \text{ M}
\]

Thus, the molarity of methanol in the solution is **1.123 M**.

Would you like further details or explanations on any step? Here are five related questions you might find helpful:

1. What is the difference between molarity and molality?
2. How would you calculate the molarity if the volume of the solution changes?
3. What are other methods to express concentration besides molarity?
4. How do temperature changes affect molarity?
5. What is the significance of molar mass in chemical calculations?

**Tip:** Always make sure the volume is in liters when calculating molarity, as this unit ensures consistency.

A solution is prepared by dissolving 3.6 g of methanol (CH3OH, Molar mass = 32.04 g/mol) into water and form 100 mL solution. Calculate the molarity of Methanol in this solution.

Learn how to calculate the molarity of methanol (CH3OH) in a 100 mL solution by applying stoichiometry and unit conversion. This example includes step-by-step calculations using the molar mass of methanol and the volume of solution. Suitable for high school students in Grades 10-12.

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