How to make 100 ml of 1000 ppm sulfur solution from sulfuric acid?

To prepare 100 mL of a 1000 ppm sulfur solution from sulfuric acid, we need to calculate the amount of sulfuric acid required based on its sulfur content. Here’s the step-by-step process:

### 1. Understanding ppm and the Composition of Sulfuric Acid
- **1000 ppm** means 1000 mg of sulfur per liter of solution, or equivalently, 100 mg per 100 mL.
- Sulfuric acid (H₂SO₄) has a molar mass of 98.08 g/mol, with sulfur (S) contributing 32.07 g/mol to this mass.
- Therefore, the percentage of sulfur by mass in H₂SO₄ is:
  \[
  \text{Percent Sulfur} = \frac{32.07}{98.08} \approx 0.327 \text{ or } 32.7\%
  \]

### 2. Calculating the Mass of Sulfuric Acid Required
- For 100 mL of solution at 1000 ppm, we need 100 mg of sulfur.
- To find the mass of sulfuric acid required to get 100 mg of sulfur:
  \[
  \text{Mass of } H_2SO_4 = \frac{\text{Required mass of Sulfur}}{\text{Percent Sulfur}}
  \]
  \[
  \text{Mass of } H_2SO_4 = \frac{100 \text{ mg}}{0.327} \approx 305.2 \text{ mg}
  \]

### 3. Converting to Volume of Sulfuric Acid
- The density of concentrated sulfuric acid (approx. 98% purity) is about 1.84 g/mL.
- To find the volume of concentrated sulfuric acid needed:
  \[
  \text{Volume of } H_2SO_4 = \frac{\text{Mass of } H_2SO_4}{\text{Density}}
  \]
  \[
  \text{Volume of } H_2SO_4 = \frac{305.2 \text{ mg}}{1.84 \text{ g/mL}} = \frac{305.2 \times 10^{-3} \text{ g}}{1.84 \text{ g/mL}} \approx 0.166 \text{ mL}
  \]

### 4. Dilution Procedure
1. Measure 0.166 mL of concentrated sulfuric acid using a pipette.
2. Add this to a volumetric flask or a container containing some distilled water.
3. Add more distilled water to bring the total volume to 100 mL.
4. Mix thoroughly.

### Important Safety Note
- Always add acid to water, not water to acid, to prevent exothermic reactions that can cause splashing.
- Wear appropriate safety gear such as gloves and goggles.

Would you like more details on any step or have any other questions? Here are some related questions for further exploration:

1. How do you calculate the ppm of a solution from a given concentration?
2. What is the procedure for diluting strong acids safely?
3. How do you convert between molarity and ppm?
4. What is the relationship between density and concentration for solutions?
5. How does the concentration of sulfuric acid affect its reactivity?

**Tip:** When working with strong acids, always add the acid to water slowly to prevent splashing and heat release.

Step-by-step guide on preparing 100 mL of a 1000 ppm sulfur solution from sulfuric acid. Includes concentration and dilution calculations, as well as relevant chemical principles such as density and percentage composition of sulfur in sulfuric acid. Suitable for high school chemistry students.

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