The osmotic pressure of equimolar solutions of glucose, KCI, MgC12 follows the order

Options

A. `MgCl_2 gt KCI gt Glucose`
B. `Glucose gt KCI gt MgCl_2`
C. `KCI_MgCl_2 Glucose`
D. `MgCl_2 gt Glucose gtKCl`

Answer

To determine the order of osmotic pressure for equimolar solutions of glucose, KCl, and MgCl2, we can follow these steps:

### Step 1: Understand the formula for osmotic pressure
The osmotic pressure (π) of a solution can be calculated using the formula:
\[ \pi = C \cdot R \cdot T \cdot i \]
Where:
- \(C\) = concentration of the solution (which is equal for all three in this case)
- \(R\) = gas constant (constant for all)
- \(T\) = temperature (constant for all)
- \(i\) = Van't Hoff factor (number of particles the solute dissociates into)

### Step 2: Identify the Van't Hoff factor for each solute
1. **Glucose**: Glucose does not dissociate in solution, so its Van't Hoff factor \(i\) is:
\[ i_{\text{glucose}} = 1 \]

2. **KCl**: KCl dissociates into two ions (K⁺ and Cl⁻) when dissolved in water, so its Van't Hoff factor \(i\) is:
\[ i_{\text{KCl}} = 2 \]

3. **MgCl2**: MgCl2 dissociates into three ions (Mg²⁺ and 2 Cl⁻) when dissolved in water, so its Van't Hoff factor \(i\) is:
\[ i_{\text{MgCl2}} = 3 \]

### Step 3: Compare the Van't Hoff factors
Now we can compare the Van't Hoff factors:
- \(i_{\text{glucose}} = 1\)
- \(i_{\text{KCl}} = 2\)
- \(i_{\text{MgCl2}} = 3\)

### Step 4: Determine the order of osmotic pressure
Since osmotic pressure is directly proportional to the Van't Hoff factor, we can conclude:
- The osmotic pressure of MgCl2 is the highest due to its Van't Hoff factor of 3.
- The osmotic pressure of KCl is next with a Van't Hoff factor of 2.
- The osmotic pressure of glucose is the lowest with a Van't Hoff factor of 1.

Thus, the order of osmotic pressure for equimolar solutions of glucose, KCl, and MgCl2 is:
\[ \text{MgCl2} > \text{KCl} > \text{Glucose} \]

### Final Answer
The osmotic pressure of equimolar solutions of glucose, KCl, and MgCl2 follows the order:
\[ \text{MgCl2} > \text{KCl} > \text{Glucose} \]

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