Answer:
The false statement is b.
The boiling point of a water sample from the Salt Lake is lower than the boiling point of pure water
Explanation:
This excersise refers to colligative properties.
Boiling point refers to the property of boiling point elevation. In a solution of ions, as water sea or water from lakes, the boiling point will be higher than water pure.
It is logical to say that, because these sort of water have ions. Remember that colligative properties depends on the solute particles.
T° boiling solution - T° pure solvent = Kb . m . i
In the freezing point depression, we have the oppossite of boiling point elevation. Freezing point of solution is lower than pure solvent, according to this:
T° freezing pure solvent - T° freezing solution = Kc . m . i
We have to always consider the i, which means Van't Hoff factor, number of ions dissolved in solution. As the i is higher, the freezing point of solution will be lower, and the boiling point of solution will be higher.
They are true statement a and c.
In solution of., [NaCl] = 0.1M, as it is a higher concentration, the molality is also higher than a solution of [NaCl] = 0.05.
As water sample form Salt Lake has certain ions, it is logical to say that the boiling point of this water is higher than boiling point of pure water.
and 
in an acid solution, can be written as :-
