When 100 ml of 10M solution of `H_(2)SO_(4)` and `100ml` of 1M solution of `NaOH` are mixed the resulting solution will be

Options

A. Acidic
B. Basic
C. Neutral
D. Can not predicted

Explanation

To solve the problem of mixing 100 ml of a 10 M solution of \( H_2SO_4 \) with 100 ml of a 1 M solution of \( NaOH \), we will follow these steps:

### Step 1: Calculate the number of moles of \( H_2SO_4 \)
The formula to calculate the number of moles is:
\[ \text{Number of moles} = \text{Molarity} \times \text{Volume (in liters)} \]
Given:
- Molarity of \( H_2SO_4 = 10 \, M \)
- Volume of \( H_2SO_4 = 100 \, ml = 0.1 \, L \)

Calculating the number of moles:
\[ \text{Number of moles of } H_2SO_4 = 10 \, M \times 0.1 \, L = 1 \, \text{mole} \]

### Step 2: Calculate the number of moles of \( NaOH \)
Using the same formula:
Given:
- Molarity of \( NaOH = 1 \, M \)
- Volume of \( NaOH = 100 \, ml = 0.1 \, L \)

Calculating the number of moles:
\[ \text{Number of moles of } NaOH = 1 \, M \times 0.1 \, L = 0.1 \, \text{mole} \]

### Step 3: Write the balanced chemical equation
The balanced reaction between sulfuric acid and sodium hydroxide is:
\[ H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O \]
From the equation, 1 mole of \( H_2SO_4 \) reacts with 2 moles of \( NaOH \).

### Step 4: Determine the limiting reagent
From the moles calculated:
- We have 1 mole of \( H_2SO_4 \)
- We have 0.1 mole of \( NaOH \)

To completely react with 0.1 mole of \( NaOH \), we need:
\[ \text{Moles of } H_2SO_4 \text{ required} = \frac{0.1}{2} = 0.05 \, \text{mole} \]
Since we have 1 mole of \( H_2SO_4 \), it is in excess, and \( NaOH \) is the limiting reagent.

### Step 5: Calculate the remaining moles after the reaction
After the reaction:
- Moles of \( NaOH \) that reacted = 0.1 mole
- Moles of \( H_2SO_4 \) that reacted = 0.05 mole

Remaining moles of \( H_2SO_4 \):
\[ \text{Remaining } H_2SO_4 = 1 - 0.05 = 0.95 \, \text{mole} \]

### Step 6: Determine the nature of the resulting solution
Since there are remaining moles of \( H_2SO_4 \) (which is an acid), the resulting solution will be acidic.

### Final Conclusion
The resulting solution after mixing 100 ml of 10 M \( H_2SO_4 \) and 100 ml of 1 M \( NaOH \) will be acidic due to the excess \( H_2SO_4 \).

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