A solution is prepared by dissolving 1.928 g of KNO3 into enough water to make 651 mL. What is the molarity of the solution?

To find the molarity of the solution, we need to use the formula:

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

### Step 1: Calculate the moles of \( \text{KNO}_3 \)
1. **Molar mass of \( \text{KNO}_3 \)**:
   - Potassium (K): 39.10 g/mol
   - Nitrogen (N): 14.01 g/mol
   - Oxygen (O): 16.00 g/mol (there are 3 oxygen atoms)

\[
\text{Molar mass of } \text{KNO}_3 = 39.10 + 14.01 + (3 \times 16.00) = 101.11 \text{ g/mol}
\]

2. **Moles of \( \text{KNO}_3 \)**:

\[
\text{Moles of } \text{KNO}_3 = \frac{1.928 \text{ g}}{101.11 \text{ g/mol}} = 0.01907 \text{ moles}
\]

### Step 2: Convert the volume of the solution from mL to L
\[
\text{Volume in liters} = \frac{651 \text{ mL}}{1000} = 0.651 \text{ L}
\]

### Step 3: Calculate the molarity
\[
\text{Molarity (M)} = \frac{0.01907 \text{ moles}}{0.651 \text{ L}} \approx 0.02928 \text{ M}
\]

The molarity of the \( \text{KNO}_3 \) solution is approximately **0.0293 M**.

Would you like more details or have any questions about this calculation?

Here are five related questions you might find helpful:
1. How do you prepare a solution with a specific molarity?
2. What is the molarity of a solution if you have different amounts of solute?
3. How do you convert molarity to molality?
4. What is the difference between molarity and molality?
5. How does temperature affect the molarity of a solution?

**Tip:** Always ensure that the volume of the solution is in liters when calculating molarity.

Learn how to calculate the molarity of a potassium nitrate (KNO3) solution with 1.928 g dissolved in 651 mL of water. This problem involves calculating molar mass, converting volume from milliliters to liters, and applying the molarity formula. Suitable for high school chemistry students.

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