G13???

[Jocelynn Franco 1L]

To prepare a fertilizer solution, a florist dilutes 1.0 L of 0.20 M NH4NO3 (aq)by adding 3.0 L of water. The florist then adds 100. mL of the diluted solution to each plant. How many moles of nitrogen atoms will each plant receive? Solve this exercise without using a calculator.

So I solved for mols of NH4NO3 and got 0.8 mol but now I'm stuck and not really sure what to do.

[Jennifer Huynh 3I]

First I used M1V1 = M2V2 to solve for the molarity of the new solution after adding 3.0 L of water.

M1V1 = M2V2
(0.2)(1) = M2(4)
M2 = 0.05

Then, I multiplied the resulting molarity by the amount of solution added to each plant to obtain the number of moles of NH4NO3 added to each plant.

ML = n
(0.05)(0.1) = 0.005 mol NH4NO3

Because there are 2 N atoms in each NH4NO3 molecule, we multiply the moles of NH4NO3 by the ratio (2/1).

0.005 mol NH4NO3 (2 mol N/1 mol NH4NO3) = 0.01 mol N

[Ellie Fox 2K]

The first thing to start with is the dilution. To do this you want to use m1v1=m2v2. This will give you the molarity of your new solution. Then, since molarity is moles of solute by the volume of the solution in liters, to get moles you can just multiply the molarity by the amount of solution added. Lastly, looking at the molecular formula of the fertilizer, there are 2 moles of nitrogen, so multiply the moles by 2 to get your answer!