(i) Write the colligative property which is used to find the molecular mass of macromolecules.
(ii) In non-ideal solution, what type of deviation shows the formation of minimum boiling azeotropes?
(ii) In non-ideal solution, what type of deviation shows the formation of minimum boiling azeotropes?
(i) Osmotic pressure is the colligative property which is used to find the molecular mass of macromolecules.
(ii) In non-ideal solution, positive deviation shows the formation of minimum boiling azeotropes.
(ii) In non-ideal solution, positive deviation shows the formation of minimum boiling azeotropes.
(i) Gas (A) is more soluble in water than Gas (B) at the same temperature. Which one of the two gases will have the higher value of KH (Henry’s constant) and why ?
(ii) In non-ideal solution, what type of deviation shows the formation of maximum boiling azeotropes ?
What are colligative properties? Write the colligative property which is used to find the molecular mass of macromolecules.
What type of intermolecular attractive interaction exists in the pair of methanol and acetone ?
Define the following terms :
(i) Mole fraction
(ii) Isotonic solutions
(iii) Van’t Hoff factor
(iv) Ideal solution
Why a mixture of Carbon disulphide and acetone shows positive deviation from Raoult’s law? What type of azeotrope is formed by this mixture?
Explain the solubility rule “like dissolves like” in terms of intermolecular forces that exist in solutions.
Define azeotropes. What type of azeotrope is formed by positive deviation from Raoult’s law ?
Give an example.
Describe the preparation of potassium permanganate. How does the acidified permanganate solution react with oxalic acid ?
Write the ionic equations for the reactions.
State Raoult’s law for a solution containing nonvolatile solute. What type of deviation from Raoult’s law is shown by a solution of chloroform and acetone and why?
State Raoult’s law. How is it formulated for solutions of non-volatile solutes ?
Calculate the degree of dissociation (α) of acetic acid if its molar conductivity () is 39.05 Scm² mol⁻¹. Given (H⁺) = 349.6 Scm² mol⁻¹ and (CH₃COO⁻) = 40.9 Scm² mol⁻¹..
A 1.00 molar aqueous solution of trichloroacetic acid (CCl₃COOH) is heated to its boiling point. The solution has the boiling point of 100.18 °C. Determine the van’t Hoff factor for trichloroacetic acid. ( for water = 0.512 K kg mol⁻¹).
Explain why on addition of 1 mol of NaCl to 1 litre of water, the boiling point of water increases, while addition of 1 mol of methyl alcohol to one litre of water decreases its boiling point.