How many grams of copper (II) sulfate are dissolved in 247 ml of water if the concentration is 48.6% m/v?

To find the amount of copper(II) sulfate (\( \text{CuSO}_4 \)) dissolved in 247 mL of water given a 48.6% m/v (mass/volume) concentration, you can follow these steps:

### Step 1: Understanding the formula
The percentage concentration by mass/volume (\( \%\ m/v \)) is defined as:

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

Rearranging to solve for the mass of solute:

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

### Step 2: Plug in the values

Given:
- Concentration (\% m/v) = 48.6%
- Volume of solution = 247 mL

\[
\text{mass of solute (g)} = \left( \frac{48.6}{100} \right) \times 247
\]

### Step 3: Calculation

\[
\text{mass of solute (g)} = 0.486 \times 247 = 120.102 \ \text{g}
\]

Thus, **120.1 grams of copper(II) sulfate** are dissolved in 247 mL of water.

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Would you like further details on this solution or have any questions?

### Related Questions:
1. How would the amount of solute change if the volume of water is doubled?
2. What is the mass of solute in a 500 mL solution with the same concentration?
3. How do you prepare a 48.6% m/v solution of copper(II) sulfate?
4. What is the molarity of this solution if the molar mass of CuSO\(_4\) is known?
5. How do you convert between m/v and molarity?

### Tip:
When working with percentages in chemistry, always confirm whether it's a mass/volume, mass/mass, or volume/volume percentage to avoid confusion in calculations.

Find out how to calculate the grams of copper (II) sulfate dissolved in 247 mL of water with a 48.6% m/v concentration. Learn the step-by-step process, including key mass-volume calculations, suitable for students in Grades 9-11.

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