Aliquid mixture contains water (h2o, mw = 18.0), ethanol (c2h5oh, mw = 46.0) and methanol (ch3oh, mw = 32.0). using two different analytical techniques to analyze the mixture, it was determined that the water mole fraction was 0.250 while the water mass fraction was 0.134. determine the mole fraction ethanol (c2h5oh) and the mole fraction methanol (ch3oh) in the solution. report the values to the correct number of significant figures.

Mole fraction of ethanol is 0.363.

Mole fraction of methanol is 0.387.

Explanation:

Mole fraction of water =

Mole fraction of ethanol =

Mole fraction of methanol =

Moles of water =

Moles of ethanol=

Moles of methanol=

Mass of the mixture = M

Mass of water,

Fraction of water by mass = 0.134

Mass of ethanol =

Mass of methanol =

..[1]

..[2]

On solving [1] and [2]:

Mole fraction of ethanol =

Mole fraction of methanol =

c, liquids evaporate, creating a gas

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.