A solution is composed of 1.15 mL of diethyl ether (C4H10O, density=0.7134 g/mL) dissolved in 78.85 mL of dichloromethane (CH2Cl2, density=1.3266 g/mL). What is the molarity of the solution?

Molarityof the solution is 0.1375 M.

Explanation:

We will first find the number of moles of diethyl ether (C4H10O)  by finding its molar mass and measured mass.

Molar mass of diethyl ether (C4H10O) = 74.12 g.

Now, volume of diethyl ether (C4H10O) = 1.15 mL and its density = 0.7134 g/mL.

Therefore,  measured mass of diethyl ether (C4H10O) = volume x  density = 1.15 mL x 0.7134 g/mL = 0.82 g.

Now, number of moles of diethyl ether (C4H10O) =

= 0.011 Moles.

Volume of the solution = volume of diethyl ether + volume of dichloromethane = 1.15 mL + 78.85 mL = 80 mL.

Now, molarity of the solution = Number of moles of diethyl ether / Volume of the solution( in  mL) x 1000 =  

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

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