How many liters of a 3.89 M K2SO4 solution are needed to provide 99.8 g of K2SO4 (molar mass 174.01 g/mol)

Explanation:

anor277

Nov 17, 2017

Well, by definition,

Molarity

≡

Moles of solute

Volume of solution

Explanation:

And thus...

moles of solute

=

molarity

×

volume

We use a molar quantity of

80.3

⋅

g

174.01

⋅

g

⋅

m

o

l

−

1

=

0.461

⋅

m

o

l

with respect to

potassium sulfate

And thus

volume

=

moles of solute

molarity

80.3

⋅

g

174.01

⋅

g

⋅

m

o

l

−

1

3.12

⋅

m

o

l

⋅

L

−

1

=

0.148

⋅

L

.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

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