The osmotic pressure of a dilute solution of a compound XY in water is four times that of a solution of 0.01 M `BaCl_(2)` in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in `"mol" L^(-1)`) in solution is:

Options

A. `4xx10^(-4)`
B. `4xx10^(-2)`
C. `6xx10^(-2)`
D. `16xx10^(-4)`

Explanation

To solve the problem, we need to find the concentration of the compound XY in a solution based on its osmotic pressure compared to a known solution of BaCl₂. Here’s a step-by-step breakdown of the solution:

### Step 1: Understand the relationship between osmotic pressure and concentration
The osmotic pressure (π) of a solution can be expressed using the formula:
\[ \pi = iCRT \]
where:
...