Equivalent mass of `NH_(3)` is -
`( NH_(3) + H^(+) rarr NH_(4)^(+))`

Options

A. 17
B. `17//2`
C. 1.7
D. `17//3`

Answer

To find the equivalent mass of ammonia (NH₃) in the reaction:

\[ \text{NH}_3 + \text{H}^+ \rightarrow \text{NH}_4^+ \]

we will follow these steps:

### Step 1: Identify the reaction
In this reaction, ammonia (NH₃) acts as a base and accepts a proton (H⁺) to form ammonium ion (NH₄⁺).

### Step 2: Determine the n-factor
The n-factor is defined as the number of moles of protons (H⁺) that one mole of the substance can accept or donate. In this case, NH₃ accepts one proton (H⁺), so the n-factor is 1.

### Step 3: Calculate the molecular mass of NH₃
The molecular mass of NH₃ can be calculated as follows:
- Nitrogen (N) has an atomic mass of approximately 14 g/mol.
- Hydrogen (H) has an atomic mass of approximately 1 g/mol, and there are 3 hydrogen atoms in NH₃.

Thus, the molecular mass of NH₃ is:
\[ \text{Molecular mass of NH}_3 = 14 + (3 \times 1) = 14 + 3 = 17 \, \text{g/mol} \]

### Step 4: Calculate the equivalent mass
The equivalent mass can be calculated using the formula:
\[ \text{Equivalent mass} = \frac{\text{Molecular mass}}{\text{n-factor}} \]

Substituting the values we have:
\[ \text{Equivalent mass} = \frac{17 \, \text{g/mol}}{1} = 17 \, \text{g/equiv} \]

### Conclusion
The equivalent mass of NH₃ is 17 g/equiv.

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