If 100mL of `1.0M NaOH` solution is diluted to 1.0L, the resulting solution contains

Options

A. 1 mole of `NaOH`
B. `0.1` mole of `NaOH`
C. `10.0` mole of `NaOH`
D. `0.05` mole of `NaOH`

Explanation

To solve the problem, we will use the concept of dilution and the formula that relates the concentrations and volumes before and after dilution.

### Step-by-Step Solution:

1. **Identify the given values:**
- Initial concentration (M1) of NaOH = 1.0 M
- Initial volume (V1) of NaOH = 100 mL = 0.1 L (since 1000 mL = 1 L)
- Final volume (V2) after dilution = 1.0 L

2. **Use the dilution formula:**
The dilution formula is given by:
\[ M_1 \times V_1 = M_2 \times V_2 \]
where:
- \(M_1\) = initial molarity
- \(V_1\) = initial volume
- \(M_2\) = final molarity
- \(V_2\) = final volume

3. **Substitute the known values into the formula:**
\[ 1.0 \, \text{M} \times 0.1 \, \text{L} = M_2 \times 1.0 \, \text{L} \]

4. **Calculate \(M_2\):**
\[ M_2 = \frac{1.0 \, \text{M} \times 0.1 \, \text{L}}{1.0 \, \text{L}} = 0.1 \, \text{M} \]

5. **Calculate the number of moles of NaOH in the final solution:**
The number of moles (n) can be calculated using the formula:
\[ n = M_2 \times V_2 \]
Substituting the values we have:
\[ n = 0.1 \, \text{M} \times 1.0 \, \text{L} = 0.1 \, \text{moles} \]

### Final Answer:
The resulting solution contains **0.1 mole of NaOH**.