G. 13

Moderators: Chem_Mod, Chem_Admin

Mansi_1D
Posts: 50
Joined: Fri Aug 02, 2019 12:15 am

G. 13

Postby Mansi_1D » Sun Oct 06, 2019 1:01 pm

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?

Can some walk me through the steps to find the moles of nitrogen atoms please.

405318478
Posts: 90
Joined: Sat Jul 20, 2019 12:16 am

Re: G. 13

Postby 405318478 » Sun Oct 06, 2019 1:05 pm

You would first find the molarity of the new solution using the equation M1V1=M2V2, then using the equation Molarity = (Moles)/(Volume) find the moles in 100mL.

Malia Shitabata 1F
Posts: 127
Joined: Sat Aug 17, 2019 12:17 am

Re: G. 13

Postby Malia Shitabata 1F » Sun Oct 06, 2019 4:04 pm

405318478 wrote:You would first find the molarity of the new solution using the equation M1V1=M2V2, then using the equation Molarity = (Moles)/(Volume) find the moles in 100mL.


I followed this but I'm not sure it gave the right answer since the solution manual said the concentration should be 0.050 and I got 0.067 and I feel like that's too far off to just be a sig fig or rounding error. And then my final answer for moles was 0.013 but it should be 0.010 or is my answer acceptable?

Bradley Whitworth 4B
Posts: 54
Joined: Sat Jul 20, 2019 12:17 am

Re: G. 13

Postby Bradley Whitworth 4B » Sun Oct 06, 2019 5:56 pm

To start you would use m1v1=m2v2 to figure out m2 in this problem taking careful note that the v2 is NOT the second volume they give you because it is being ADDED to the first volume in this instance so the actual v2 would be v1 plus the amount being added. Once you find the m2 we know that molarity=moles/volume so with the found m2 we can plug that in as molarity and plug in the 100ml given by the problem (converted to liters) to solve for the amount of moles of nitrogen each plant gets

Bradley Whitworth 4B
Posts: 54
Joined: Sat Jul 20, 2019 12:17 am

Re: G. 13

Postby Bradley Whitworth 4B » Sun Oct 06, 2019 5:58 pm

To start you would use m1v1=m2v2 to figure out m2 in this problem taking careful note that the v2 is NOT the second volume they give you because it is being ADDED to the first volume in this instance so the actual v2 would be v1 plus the amount being added. Once you find the m2 we know that molarity=moles/volume so with the found m2 we can plug that in as molarity and plug in the 100ml given by the problem (converted to liters) to solve for the amount of moles of nitrogen each plant gets

Miriam Villarreal 1J
Posts: 105
Joined: Sat Aug 17, 2019 12:16 am

Re: G. 13

Postby Miriam Villarreal 1J » Sun Oct 06, 2019 6:02 pm

Dilution Formula: M1V1=M2V2
Therefore, (0.20NH4No3)(1.0L)=M2(4.0L) - you add the 3.0L and 1.0L
=.05 mol NH4NO3


Return to “Molarity, Solutions, Dilutions”

Who is online

Users browsing this forum: No registered users and 2 guests