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

Options

A. 0.01 M
B. 0.005 M
C. 0.02 M
D. 0.1 M

Explanation

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

### Step 1: Understand the formula for molarity
Molarity (M) is defined as the number of moles of solute divided by the volume of the solution in liters. The formula is:
\[ \text{Molarity (M)} = \frac{\text{Number of moles of solute}}{\text{Volume of solution in liters}} \]

### Step 2: Identify the number of moles of solute
From the question, we know that the number of moles of NaCl (solute) is:
\[ \text{Number of moles of NaCl} = 0.01 \text{ moles} \]

### Step 3: Convert the volume of the solution from milliliters to liters
The volume of the solution is given as 500 ml. To convert this to liters, we use the conversion factor that 1 liter = 1000 ml:
\[ \text{Volume in liters} = \frac{500 \text{ ml}}{1000} = 0.5 \text{ liters} \]

### Step 4: Substitute the values into the molarity formula
Now, we can substitute the values we have into the molarity formula:
\[ \text{Molarity (M)} = \frac{0.01 \text{ moles}}{0.5 \text{ liters}} \]

### Step 5: Calculate the molarity
Now, we perform the calculation:
\[ \text{Molarity (M)} = \frac{0.01}{0.5} = 0.02 \text{ M} \]

### Final Answer
The molarity of the solution is:
\[ 0.02 \text{ M} \]

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