For the equimolal solutions, increasing order of osmotic pressure is

1. 1 m \(C_6H_5COOH\)
2. 1 m \(BaCl_2\)
3. 1 m \(KCl\)
4. 1 m glucose
5. 1 m \(H_3PO_4\)

Choose the correct answer from the options given below:

E < C < B < D < A

The correct answer is 4. E < C < B < D < A.

Osmotic pressure is a colligative property, which means that it depends on the number of particles in solution, not on the type of particles. The more particles in solution, the higher the osmotic pressure.

Equimolal solutions have the same number of moles of solute per liter of solution. However, some solutes dissociate into ions in solution, while others do not. For example, \(BaCl_2\) dissociates into three ions in solution \((Ba^{2+}, 2Cl^-)\), while glucose does not dissociate.

Therefore, the order of increasing osmotic pressure for the equimolal solutions is as follows:

1. \(H_3PO_4\) (5 ions per molecule)
2. \(BaCl_2\) (3 ions per molecule)
3. \(KCl\) (2 ions per molecule)
4. \(Glucose\) (1 molecule per molecule)
5. \(C_6H_5COOH\) (1 molecule per molecule)