the Osmotic pressure of 0.010 M solution of kI and sucrose our 0.432 atm and 0.24 atm respectively. the van't Hoff factor for KI is
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GIven:
The molarity of KI and sucrose solutions, C = 0.01 M
The osmotic pressure of KI solution, Π (KI) = 0.432 atm
The osmotic pressure of sucrose solution, Π (sucrose) = 0.24 atm
To Find:
The Van’t Hoff factor, i.e., 'i' for Potassium Iodide.
Calculation:
- Sucrose is a non - electrolyte compound, so it does not dissociate in water.
- The osmotic pressure of sucrose is given as:
Π(sucrose) = C × R × T
⇒ 0.24 = 0.1 × R × T
⇒ R × T = 2.4 ....(i)
- As KI dissociates in water to form K⁺ and I⁻.
- The osmotic pressure of KI can be given as:
Π (KI) = i × C × R × T
⇒ 0.432 = i × 0.1 × 2.4 {from (i)}
⇒ i = 0.432/0.24
⇒ i = 1.8
- So, the Van’t Hoff factor for KI is 1.8.
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