`6.02xx10^(23)` molecules of urea are present in `100 ml` of its solution. The concentration of urea solution is -

Options

A. `0.001 M`
B. `0.01 M`
C. `0.02 M`
D. `10 M`

Answer

To find the concentration of urea solution in terms of molarity, we can follow these steps:

### Step 1: Determine the number of moles of urea
We know that:
- The number of molecules of urea = \( 6.02 \times 10^{23} \) molecules.
- According to Avogadro's number, \( 1 \) mole of any substance contains \( 6.022 \times 10^{23} \) molecules.

Using this information, we can calculate the number of moles of urea:

\[ \text{Number of moles of urea} = \frac{\text{Number of molecules}}{\text{Avogadro's number}} = \frac{6.02 \times 10^{23}}{6.022 \times 10^{23}} \approx 1 \text{ mole} \]

### Step 2: Convert the volume of the solution to liters
The volume of the solution is given as \( 100 \) ml. We need to convert this to liters:

\[ \text{Volume in liters} = \frac{100 \text{ ml}}{1000} = 0.1 \text{ L} \]

### Step 3: Calculate the molarity (concentration) of the solution
Molarity (M) is defined as the number of moles of solute per liter of solution. We can use the formula:

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

Substituting the values we have:

\[ \text{Molarity} = \frac{1 \text{ mole}}{0.1 \text{ L}} = 10 \text{ M} \]

### Conclusion
The concentration of the urea solution is \( 10 \text{ M} \).

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