What is the concentration in %m/v of a 0.677 M aqueous solution of acetone (MM = 58.08 g/mol)?

To find the concentration in % m/v (mass/volume percent), we use the following relationship:

\[
\text{Concentration} \, (\% m/v) = \frac{\text{mass of solute (g)}}{\text{volume of solution (mL)}} \times 100
\]

Given:
- **Molarity (M)** = 0.677 mol/L
- **Molar mass (MM) of acetone** = 58.08 g/mol
- 1 L = 1000 mL

### Step 1: Calculate the mass of acetone in 1 liter of solution.
The molarity tells us that there are 0.677 moles of acetone per liter of solution.

\[
\text{Mass of acetone (g)} = \text{Molarity (mol/L)} \times \text{Molar mass (g/mol)} = 0.677 \, \text{mol/L} \times 58.08 \, \text{g/mol} = 39.33 \, \text{g}
\]

### Step 2: Calculate the concentration in % m/v.
Now that we know there are 39.33 g of acetone in 1 L (1000 mL) of solution:

\[
\text{Concentration} \, (\% m/v) = \frac{39.33 \, \text{g}}{1000 \, \text{mL}} \times 100 = 3.933\%
\]

### Final Answer:
The concentration of the solution is **3.933% m/v**.

Would you like more details on any step?

Here are 5 related questions for practice:
1. How would the % m/v change if the molarity were doubled?
2. What is the molarity of a solution with a concentration of 5% m/v?
3. How do you convert between % m/v and molarity for any solute?
4. If the volume of solution is reduced by half, what happens to the % m/v concentration?
5. How does the density of the solution affect % m/v?

**Tip:** Always double-check your units to ensure you're calculating mass/volume percent correctly!

Learn how to calculate the % m/v concentration of a 0.677 M aqueous solution of acetone. This detailed step-by-step guide involves using molarity and molar mass to find the mass of solute, followed by calculating the mass/volume percent concentration. Suitable for high school students in Grades 10-12.

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