You measure out 1.8 mL of an aqueous ethylenediamine (H2NCH2CH2NH2) solution. This aqueous solution has a density of 0.950 g/mL and is 25.0% by mass ethylenediamine. How many moles of ethylenediamine are in the 1.8 mL?

To find the answer we need to convert the volume to mass using density, the mass to mass of ethylenediamine using the concentration of the solu and to moles using its molar mass (Molar mass ethylendiamine: 60.1g/mol):

Mass:

1.8mL * (0.950g/mL) = 1.71g

Mass ethylenediamine:

1.71g * 25.0% = 0.4275g ethylenediamine.

Moles:

0.4275g * (1mol / 60.1g) =

7.11x10⁻³ moles ethylenediamine

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ConcepcionPetillo ConcepcionPetillo · Answer 2 · 2022-03-26T08:57:47+01:00

There are 7.11x10⁻³ moles of ethylenediamine in 1.8mL

Calculating the number of moles:

We have to convert the volume to mass first:

Mass = volume × density

1.8mL × (0.950g/mL) = 1.71g

Now, the mass of ethylenediamine is:

1.71g × 25.0% = 0.4275g of ethylenediamine.

The molar mass of ethylenediamine is: 60.1g/mol

So, the number of moles of ethylenediamine :

0.4275g × (1mol / 60.1g) = 7.11x10⁻³ moles of ethylenediamine

Learn more about moles conversion:

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