Exams › JEE Advanced › Chemistry

A sample of K3[Fe(CN)6] is found to be 60% dissociated in aqueous solution. What is the value of the Van't Hoff factor (i) for this solution?

1. 4
2. 3.8
3. 2.8
4. 2.4

Correct answer: 2.8

Solution

K3[Fe(CN)6] dissociates into 4 ions (3 K+ and 1 [Fe(CN)6]³-), so n = 4. With alpha = 0.60, i = 1 + 3(0.60) = 2.8.

Related JEE Advanced Chemistry questions

• In which of the following cases can the pH be determined using the equilibrium constant(s) provided?
• In the equilibrium reaction NH2COONH4(s) ⇌ 2NH3(g) + CO2(g), which change will cause the partial pressure of NH3 to rise?
• For the reaction XY2(g) ⇌ XY(g) + Y(g), if the value of α (degree of dissociation) is very small compared to 1, how is α related to the pressure (P)?
• At 460°C, 0.02 g of hydrogen reacts with 2.54 g of iodine until equilibrium is reached. Upon analysis, the equilibrium mixture contains 0.0021 moles of iodine. What is the equilibrium constant (Kc) for this reaction?
• Determine the pH of a 1.0 M solution of an unidentified hydroxide compound, assuming the metal ion has a +1 charge.
• What explains the acidic nature of an aqueous solution of aluminum chloride?

⚔️ Practice JEE Advanced Chemistry free + battle 1v1 →