What is the boiling point of an aqueuous solution of
anonelectrolyte that has an osmotic pressure of 10.50 atm at 25c?
kbof water is 0.52c/m. assume its density is the same as
purewater.

100.223°C is the boiling point of an aqueous solution.

Explanation:

Osmotic pressure of the solution = π = 10.50 atm

Temperature of the solution =T= 25 °C = 298 .15 K

Concentration of the solution = c

van'y Hoff factor = i = 1 (non electrolyte)

c = 0.429 mol/L = 0.429 mol/kg = m

(density of solution is the same as  pure water)

m = molality of the solution

Elevation in boiling point =

T = Boiling point of the pure solvent

= boiling point of the solution

= Molal elevation constant

We have :

(given)

m = 0.429 mol/kg

T = 100° C (water)

100.223°C is the boiling point of an aqueous solution.

c. 75.7

i think that is the right

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

if you need further assistance, let me know: )

~ trueboss72