M1V1=M2V2  [ENDORSED]

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Rohan Kubba Dis 4B
Posts: 50
Joined: Sat Aug 17, 2019 12:18 am

M1V1=M2V2

Postby Rohan Kubba Dis 4B » Thu Oct 03, 2019 12:13 am

I understand that the molarity equation is M1V1=M2V2, however the molarity equation is = to M=n/V. So, basically, I am asking about the idea that shouldn’t the volume cancel out in the M1V1=M2V2. I know my thinking is wrong but I just need a plausible explanation for it.

SnehinRajkumar1L
Posts: 101
Joined: Thu Jul 11, 2019 12:15 am

Re: M1V1=M2V2  [ENDORSED]

Postby SnehinRajkumar1L » Thu Oct 03, 2019 12:18 am

This equation demonstrates that initial and final moles are always equal when diluting a solution. So, yes, when you do multiply it out, the units for volume cancel out, but you are left with the number of moles. This equation helps us calculate volume needed for dilutions or new concentrations using the idea that moles are conserved in a solution.

Junwei Sun 4I
Posts: 125
Joined: Wed Oct 02, 2019 12:16 am

Re: M1V1=M2V2

Postby Junwei Sun 4I » Thu Oct 03, 2019 12:21 am

M wouldn't cancel out here since M1V1 actually comes from manipulating the equation Molarity(M)=number of moles(n)/volume. Since we know that moles of solute remain the same when diluting a solution we manipulate M=n/v to be n=MV so that we could set up the equation M1V1=M2V2 to solve for unknowns in the dilution process. I'm not that good at explaining equation but hopefully this help!

Jasmine Fendi 1D
Posts: 108
Joined: Sat Aug 24, 2019 12:15 am

Re: M1V1=M2V2

Postby Jasmine Fendi 1D » Thu Oct 03, 2019 12:52 am

Yes! Technically the equation would cancel out and become n1=n2, which is what M1V1=M2V2 originally derived from. Sometimes the problem would only give you molarity and volume so you wouldn't use moles.


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