Choose the correct balanced chemical equations to show the reactions of the following:
Aluminium and caustic potash solution.

Options

A. `2Al + 2KOH + 2H_(2)O rarr 2KAl + 3H_(2)O`
B. `2Al + 2KOH + 2H_(2)O rarr 2KAlO_(2) + 3H_(2)`
C. `2Al + 2KOH + 2H_(2)O rarr KAlO_(2) + 3H_(2)`
D. `2Al + 2KOH + 2H_(2)O rarr 2KAlO + 3H_(2)`

Explanation

To solve the problem of writing the balanced chemical equation for the reaction between aluminum and caustic potash (potassium hydroxide, KOH), we can follow these steps:

### Step 1: Identify the Reactants and Products
- **Reactants**: Aluminum (Al) and caustic potash (KOH).
- **Products**: The reaction of aluminum with a strong base like KOH typically produces potassium aluminate (KAlO2) and hydrogen gas (H2).

### Step 2: Write the Unbalanced Equation
The unbalanced equation for the reaction can be written as:
\[ \text{Al} + \text{KOH} \rightarrow \text{KAlO}_2 + \text{H}_2 \]

### Step 3: Determine the Oxidation States
- Aluminum (Al) in its elemental form has an oxidation state of 0.
- In potassium aluminate (KAlO2), aluminum has an oxidation state of +3.
- Potassium (K) has an oxidation state of +1, and oxygen (O) has an oxidation state of -2.

### Step 4: Balance the Equation
1. **Balance Aluminum**: There is 1 aluminum atom on both sides.
2. **Balance Potassium**: Since there is 1 potassium in KAlO2, we need 1 KOH.
3. **Balance Oxygen**: KAlO2 has 2 oxygen atoms, so we need to account for that.
4. **Balance Hydrogen**: The reaction produces hydrogen gas (H2).

The balanced equation can be written as:
\[ 2 \text{Al} + 2 \text{KOH} \rightarrow 2 \text{KAlO}_2 + 3 \text{H}_2 \]

### Step 5: Final Check
- Count the number of each type of atom on both sides:
- Aluminum: 2 on both sides.
- Potassium: 2 on both sides.
- Oxygen: 4 on both sides (2 from KAlO2).
- Hydrogen: 6 on the product side (3 H2) and 6 on the reactant side (2 KOH).

The equation is balanced correctly.

### Final Balanced Equation
\[ 2 \text{Al} + 2 \text{KOH} \rightarrow 2 \text{KAlO}_2 + 3 \text{H}_2 \]

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