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Calculate the mass of ammonium sulfide (nh4)2s in 3.00 l of a 0.0200 m solution. g (nh4)2s

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CintiaSalazar

Taking into account the definition of molarity, 4.08 grams of ammonium sulfide are present in 3.00 L of a 0.0200 M solution.

Definition of molarity

Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.

The molarity of a solution is calculated by dividing the moles of solute by the volume of the solution:

[tex]Molarity=\frac{number of moles}{volume}[/tex]

Molarity is expressed in units [tex]\frac{moles}{liter}[/tex].

Mass of ammonium sulfide

In this case, you know:

  • Molarity: 0.0200 M
  • number of moles: ?
  • volume: 3 L

Replacing in the definition of molarity:

[tex]0.0200 \frac{moles}{liter}=\frac{number of moles}{3 L}[/tex]

Solving:

0.0200  [tex]\frac{moles}{liter}[/tex]× 3 L= number of moles

0.06 moles= number of moles

On the other side, the molar mass is the amount of mass that a substance contains in one mole. In this case, the molar mass of ammonium sulfide is 68 g/mole.

Then, the amount of mass contained in 0.06 moles is calculated as:

0.06 moles×[tex]\frac{68 grams}{1 mole}[/tex]= 4.08 grams

Finally, 4.08 grams of ammonium sulfide are present in 3.00 L of a 0.0200 M solution.

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