Make a solution of one-tenth normal nitric acid one liter

To prepare a 0.1 N (one-tenth normal) solution of nitric acid (HNO₃), we'll need to calculate the amount of concentrated nitric acid required and then dilute it to 1 liter with distilled water.

### Step-by-Step Solution:

1. **Determine the Molecular Weight and Normality**:
   - The molecular weight of HNO₃ is approximately 63 g/mol.
   - For nitric acid, normality (N) is equivalent to molarity (M) because it donates one proton (H⁺) per molecule.

2. **Calculate the Amount for 0.1 N Solution**:
   - For a 1 N solution, we would need 63 grams of HNO₃ per liter.
   - For a 0.1 N solution, we need 6.3 grams of HNO₃ per liter.

3. **Determine the Volume of Concentrated Nitric Acid**:
   - Concentrated nitric acid is typically around 68% HNO₃ by weight with a density of approximately 1.42 g/mL.
   - Therefore, 1 mL of concentrated HNO₃ contains \(1.42 \, \text{g/mL} \times 0.68 = 0.9656 \, \text{g}\) of HNO₃.

   - To obtain 6.3 grams of HNO₃:
     \[
     \text{Required Volume} = \frac{6.3 \, \text{g}}{0.9656 \, \text{g/mL}} \approx 6.52 \, \text{mL}
     \]

4. **Preparation Steps**:
   - Measure approximately 6.52 mL of concentrated nitric acid using a pipette or a volumetric cylinder.
   - Carefully add the nitric acid to a container with about 500 mL of distilled water (never add water to acid as it can cause splashing or an exothermic reaction).
   - Mix the solution and then add more distilled water until the total volume reaches 1 liter.

5. **Final Solution**:
   - You now have 1 liter of 0.1 N nitric acid solution.

Would you like additional details on the preparation steps or clarifications?

### Related Questions
1. How do you calculate the normality of other acids?
2. What precautions should be taken when diluting acids?
3. How does normality differ from molarity for diprotic and triprotic acids?
4. Can this method be adapted for bases, such as NaOH?
5. How does temperature affect the concentration of solutions?

#### Tip
Always add acid to water, not water to acid, to minimize the risk of an exothermic reaction and splattering.

Make a solution of one-tenth normal nitric acid one liter.

Learn how to prepare a 0.1 N nitric acid solution in a 1-liter volume using calculations for dilution, density, and normality. This solution requires calculating the mass of HNO₃ needed and the volume of concentrated nitric acid. Suitable for high school chemistry students.

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