1000Ppm Fluoride Ion Solution

How to Prepare 100ppm Solution of Fluoride Ion?

Answer:
I'm going to assume you want 100ppm by mass, since this is really the only way that makes sense with a solid and liquid.

First, youneed to get a fluoride salt. I will use sodium fluoride as an example - it may or may not matter which salt depending on what you're trying to do. Be careful, fluoride compounds can be toxic.

Second,you need to figure out what percentage of the salt is actually fluoride. To do this in our example, first look up the molecular weights of sodium and fluorine on a periodic table (the numbers at thebottom of the squares). Sodium (Na) has a molecular weight of 22.989, Fluorine (F) weighs 18.998. Add these to get the total molecular weight of sodium fluoride:
22.989 + 18.998 = 41.987

Now,divide the total weight by the weight of fluorine to get a conversion factor (units of NaF / units of F):
41.987 / 18.998 = 2.21

Third, you need to weigh out your fluorine and water - 100 partsfluorine for every (million - 100) parts water. This reduces to 1 part fluorine per 9,999 parts water (I'll round to 10,000). This is a big difference, so you may need two different scales withdifferent ranges, and it's going to make a bunch of solution.

I'm going to measure in grams, but you could use any measure of weight. First, weight out 10,000 g (10 kg) of water and set it aside. Rememberto subtract out the weight of the container when weighing! Next, we need 1 g of fluoride. However, we have sodium fluoride, not fluorine, so we need to use the conversion factor from before:
1 g(F) * 2.21 (NaF / F) = 2.21 g NaF

Weigh out 2.21 g of your salt, add it to the water, and you're done!!!

A problem with this method is you'll end up with a huge amount of solution, and it may bemore water than you can easily deal with. To avoid the issue, make the initial solution more concentrated, then dilute it again in a second step. For example, use only 1 / 10th the amount of water,...