15. The elevation of boiling point can be given by
kb is constant, C is molality of the solution, and i is the van 't Hoff factor.
For molecular (non-ionic) solute, i=1
For ionic solute, i>1.
So, the presence of ionic solute raises the boiling point.
16. The freezing point of the solution will be lowered compared to a pure substance (according to freezing point depression).
17. (i) strong electrolyte
strong acid, e.g: HCl
strong base, e.g: NaOH
salt, e.g: NaCl
(ii) weak electrolyte
weak acid, e.g: H2CO3
weak base, e.g: NH3
(iii) Non-electrolyte
sugar, fats, etc.
18. Properties of acids:
i. It gives H3O+ ion in water or it is a lone-pair acceptor (Lewis acid). Mostly electrolyte in aqueous solution.
ii. forms salt by reacting with a base.
iii. releases hydrogen gas while reacting with the metal.
iv. changes the color of a pH indicator.
v. taste: sour
Properties of bases:
i. It gives OH- ion in water or it is a lone-pair donar (Lewis base).
ii. forms salt by reacting with acid.
iii. taste: bitter.
iv. it conducts electricity.
19. Strong acid or base is fully dissociated in an aqueous solution.
e.g: HCl+H2O ----> H3O+ +Cl-
Weak acid or base is partially dissociated.
20. pH=-log10[ H3O+]
For acid: pH: 0-7
For base: pH: 7-14
21. Properties of salts:
i. ionic in nature.
ii. mostly water-soluble.
iii. usually insulator. But in an aqueous medium, it carries charges.
iv. mostly, salty in taste.
v. it has a high melting point.
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