The molarity of solution obtained by dissolving 0.01 moles of NaCl in 500ml of solution is:

Explanation

To find the molarity of a solution obtained by dissolving 0.01 moles of NaCl in 500 mL of solution, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the number of moles of solute**:
The problem states that we have 0.01 moles of NaCl.

\[ \text{Moles of NaCl} = 0.01 \text{ moles} \]

2. **Convert the volume from mL to L**:
The volume of the solution is given as 500 mL. To convert this to liters, we divide by 1000 (since 1 L = 1000 mL).

\[ \text{Volume in liters} = \frac{500 \text{ mL}}{1000} = 0.5 \text{ L} \]

3. **Use the molarity formula**:
Molarity (M) is defined as the number of moles of solute divided by the volume of the solution in liters.

\[ \text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Volume of solution in L}} \]

Plugging in the values we have:

\[ \text{Molarity} = \frac{0.01 \text{ moles}}{0.5 \text{ L}} \]

4. **Calculate the molarity**:
Performing the division gives us:

\[ \text{Molarity} = 0.02 \text{ M} \]

### Final Answer:
The molarity of the solution obtained by dissolving 0.01 moles of NaCl in 500 mL of solution is **0.02 M**.

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