A metal chloride contains 25.26% metal. Its equivalent weight is

Options

A. 12
B. 24
C. 36
D. 48

Explanation

To find the equivalent weight of the metal in the metal chloride that contains 25.26% metal, we can follow these steps:

### Step 1: Determine the mass of the metal and chlorine in 100 g of the metal chloride.
Given that the metal chloride contains 25.26% metal, in 100 g of the metal chloride, the mass of the metal (M) is:
\[ \text{Mass of Metal} = 25.26 \, \text{g} \]
The remaining mass will be chlorine (Cl):
\[ \text{Mass of Chlorine} = 100 \, \text{g} - 25.26 \, \text{g} = 74.74 \, \text{g} \]

### Step 2: Find the equivalent weight of chlorine.
The atomic weight of chlorine (Cl) is approximately 35.5 g/mol. The equivalent weight of chlorine, which is the weight that reacts with one mole of metal, is equal to its atomic weight since chlorine typically forms one bond in metal chlorides:
\[ \text{Equivalent weight of Cl} = 35.5 \, \text{g} \]

### Step 3: Set up the relationship between metal and chlorine.
From the information given, we know that 25.26 g of metal reacts with 74.74 g of chlorine. We can set up a proportion to find out how much metal would react with 35.5 g of chlorine:
\[ \frac{25.26 \, \text{g of metal}}{74.74 \, \text{g of Cl}} = \frac{x \, \text{g of metal}}{35.5 \, \text{g of Cl}} \]

### Step 4: Solve for x (the equivalent weight of the metal).
Cross-multiplying gives:
\[ 25.26 \times 35.5 = 74.74 \times x \]
Calculating the left side:
\[ 25.26 \times 35.5 = 897.63 \]
Now, we can solve for x:
\[ x = \frac{897.63}{74.74} \]
Calculating this gives:
\[ x \approx 12 \, \text{g} \]

### Conclusion:
The equivalent weight of the metal is approximately 12 g.