A mixture containing one mole of `BaF_(2)` and two mole of `H_(2)SO_(4)` will be neutralised by:

Options

A. 1 mole `KOH`
B. 4 mole `KOH`
C. 2 mole `KOH`
D. 2 mole `Ca(OH)_(2)`

Answer

To solve the problem of neutralizing a mixture containing one mole of BaF₂ and two moles of H₂SO₄, we need to follow these steps:

### Step 1: Write the Reaction
First, we need to understand the reaction that occurs between BaF₂ and H₂SO₄. Barium fluoride (BaF₂) reacts with sulfuric acid (H₂SO₄) to form barium sulfate (BaSO₄) and hydrofluoric acid (HF):

\[ \text{BaF}_2 + \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{HF} \]

### Step 2: Determine the Moles of Products
From the balanced equation, we see that one mole of BaF₂ reacts with one mole of H₂SO₄ to produce one mole of BaSO₄ and two moles of HF. Since we have two moles of H₂SO₄, only one mole will react with BaF₂, leaving one mole of H₂SO₄ unreacted.

### Step 3: Identify the Neutralization Requirement
To neutralize the remaining unreacted sulfuric acid (H₂SO₄), we need a base. H₂SO₄ is a strong acid that can release two protons (H⁺ ions), so we need two hydroxide ions (OH⁻) to neutralize one mole of H₂SO₄.

### Step 4: Choose the Base
The bases that can provide the required hydroxide ions are:
- Calcium hydroxide (Ca(OH)₂), which provides two OH⁻ ions per mole.
- Potassium hydroxide (KOH), which provides one OH⁻ ion per mole.

### Step 5: Calculate the Required Moles of Base
To neutralize one mole of the remaining H₂SO₄:
- If we use Ca(OH)₂, we need 1 mole of Ca(OH)₂ (since it provides 2 OH⁻ ions).
- If we use KOH, we need 2 moles of KOH (since it provides 1 OH⁻ ion per mole).

### Conclusion
Thus, to neutralize the mixture, we can use either:
- 1 mole of Ca(OH)₂, or
- 2 moles of KOH.

### Final Answer
The mixture can be neutralized by either **1 mole of Ca(OH)₂ or 2 moles of KOH**.

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