carbonate to 1ppm ammonia
Here's my math:
Here is the formula to determine ppm
From: Lesson 8: The Chemistry of Solutions
So what I want to know is, what g/L for 1ppm. So our variable in the equation is "mass of solute (g)". So I first rewrite the equation to put all instances of g on one side.
g = variable to solve for
mass of solvent = 1000 (water)
This gives us 1 = (g/(1000+g)) * (1,000,000/1)
1 = (g/(1000+g)) * 1,000,000
1/1,000,000 = g/(1000+g)
.000001 = g/(1000+g)
.001 + .000001g = g
.001 = g - .000001g
.001 = .999999g
g/L=.001 to make 1 ppm
or, 1.000001 mg
/L to make 1 ppm
Here it is rewritten as a single equation, using water weight as a constant for solvent, and adding in ppm
as a changeable variable:
is a variable that one can enter to solve for any ppm
that I specify.
Or of course you can just multiply your g value from the simplified version by your ppm
This is not the full answer of course. If you enter in 10ppm (for the 10:1 ratio), you'll be given 10mg/L. So we're not done because not all of that 10mg is carbonate.
So my molecule is NaHCO3, but I only care about the atom CO3.
Molar mass of CO3 is 60.01
Molar mass of the entire molecule is 84.0075
So CO3 is 60.01/84.0075 = .71434098 of the molecule
So to determine how much total solvent to put in, we solve for:
total solvent = mg
of atom to make x ppm
[from our previous equation] / (molar mass of desired atom / molar mass of molecule)
So in the specific case of our molecule with carbonate, this equation is:
I'm not that good at showing my work with math problems so if this requires clarification I will try to look over it and expand it