Question

The following NLC system which shows equilibrium between solute and solvent is

1 mL H2O & 3 mL ethanol

1 g KNO3 & 100 mL H2O

1 g I2 & 100 mL H2O

2 M CaCl2

Answer 1

Answer :1 g I₂ & 100 mL H2O

When iodine is added to water, the following equilibrium is established

I₂(s) + H₂O(l) = OI^-(aq) + 2H⁺(aq) + I^-(aq)

I^-(aq) = Iodide ion

OI^-(aq) = hypoiodite ion

2 M CaCl2 and 1 g KNO3 & 100 mL H2O are solutions of strong electrlytes in water .The strong electrolytes are almost completely dissociated in aqueous solutions and there exists NO equilibrium between solute and solvent

1 mL H2O & 3 mL ethanol : Ethanol and water are miscible with each other in all proportions. Hence there will be No equilibrium between solute and solvent