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IRISSAK [1]
3 years ago
14

A student dissolves 7.9 g of stilbene (C14H12) in 475. mL of a solvent with a density of 1.03 g/mL. The student notices that the

volume of the solvent does not change when the stilbene dissolves in it. Calculate the molarity and morality of the students solution. Round both of your answers to 2 significant digits.
Chemistry
1 answer:
andrey2020 [161]3 years ago
6 0

Answer:

Molarity: 0.092M

Molality: 0.090m

Explanation:

Molarity, M, is defined as the moles of solute (In this case, C14H12 -Molar mass: 180.25g/mol-) in 1L of solution.

The molality, m, are moles of solute per kg of solvent.

<em>Molarity:</em>

<em>Moles solute: </em>

7.9g * (1mol/180.25g) = 0.04383 moles

<em>Liters solution:</em>

475mL = 0.475L

Molarity: 0.04383 moles / 0.475L = 0.092M

<em />

<em>Molality:</em>

<em>kg solvent:</em>

475mL * (1.03g/mL) = 489.25g = 0.48925kg

Molality:

0.04383 moles / 0.48925kg = 0.090m

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An aqueous solution is 0.467 m in hcl. what is the molality of the solution if the density is 1.23 g/ml?
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Answer:
molarity = 0.385 moles/kg

Explanation:
Assume that the volume of the aqueous solution given is 1 liter = 1000 ml
Now, density can be calculated using the following rule:
density = mass / volume
Therefore:
mass = density * volume = 1.23 * 1000 = 1230 grams
Now, 0.467 m/L * 1L = 0.467 moles of HCl
We will get the mass of the 0.467 moles of HCl as follows:
mass = molar mass * number of moles = (1+35.5)*0.467 = 17.0455 grams
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To calculate the molar solubility, we use the equation given by Henry's law, which is:

C_{C_2H_4}=K_H\times p_{C_2H_4}

where,

K_H = Henry's constant = 4.78\times 10^{-3}mol/L.atm

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p_{C_2H_4} = partial pressure of ethylene gas = 0.684 atm

Putting values in above equation, we get:

C_{C_2H_4}=4.78\times 10^{-3}mol/L.atm\times 0.684atm\\\\C_{C_2H_4}=3.27\times 10^{-3}mol/L

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