 # Aquarium Math

2206 Views 2 Replies 2 Participants Last post by  dennis
I thought it might be nice if we had a reference to go to with math related issues. I for one always have trouble wiht a few of the chemistry problems and equations we (or at least a dork like me) soemtimes use. For instance: How do figure out how much of a certain element is in something (ie, how much K in KNO3, or how much Ca in Kent's liquid calcium and how much does 1ml of it add to my tank)? How can there be more than 100% of something (reciently read a bag of dolomite that said 104% equivilant to Calcium carbonate by dry weight)? Is it really ok to measure things in teaspoons when some products are obvoiusly "fluffier"(contain more air) than others?

I am sure there are others but they elude me right now. Maybe someone who is good at chemesrty could post a little something helpful for those less fortunate. I would try but obviously..... :? .

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well, let me see if I can tackle this for you.

Asking how much K in KNO3 is tricky. It all depends on how you define the question. it could be 1) how many grams of K for every gram of KNO3. it could also mean how many moles of K per gram of NO3 etc etc.

lets consider the 1st more obvious possiblility. the mass of on mole of the following (rounded for easier math)
K=39g
N=14g
O=16g

so 1 mole of KNO3=39+14+16=69g. so 39/69=~57% K.

You can take the above example and apply it so many other ways using different definitions of "how much"

To answer you second part is very simple. It comes down to the following formula
M1V1=M2V2 where V=volumes in liters and M =concentrations in moles/L
alternately, it could be grams and milliliters...all depends on how things are defined in the starting values

Example. Suppose Kent is 10% Ca (10^-2 ...ppm=10^-6 so 10% Ca=10000ppm)

You want to add 1mL of 10,000 ppm Ca into your 29g tank.
we need to 1st convert 25g to L which well approximate at ~100L
M1V1=M2V2
(10,000ppm Ca)*(1ml *1L/1000mL)=M2*100L
Solve for M2 and you find out that you just added 0.1ppm Ca

(NOTE, I have rounded a lot of stuff for simplicity)

The 104% deal is kinda tricky and depends on how they define their units...which we can't tell right now.

As for the fluffy thing, recall that density has the unitys of mass/volume. as long as you know the approximate density of the material and account for it, you can measure out stuff approximately by using volumes (tsp/tbs) instead of mass (grams)

Hope this clears some stuff up

...hope I didn't make a stupid mistake in my rapid calculations too See less See more
Excellent Gomer. Thank you I see that the mass of one mole of an element is the same as the atomic mass(amu) of that element expressed in grams. I understand that. Cool I think this is a wonderful start. I would really like to continue adding info and tips to this so we can have a reference to come to wiht this sort of thing.

Thanks again
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