  # NotYou

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## Profile Information

• Location
Australia Somewhere
• Interests
Pools
• Favorite Area of Science
Pools
• Occupation
Pool Technician

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## NotYou's Achievements 1

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1. Thanks for this extra info, Studiot. I haven't got there yet, but that is what I am looking to learn (and more).
2. It can also be written as: 1 = Vreverse Vforward Which becomes: Kequilibrium = [A][ B] = kreverse [C][D] kforward How will that change the rest of the proof?
3. I found it as PDF's at analysischamp.com/links2.html
4. Are these dissociation constants available for everything? Where would I find a list of them?? (Please don't say "Google it") So that would mean that these dissociation constants are dependant on temperature and pressure? Is there a formula for that/them?? What happens when either are pure? Can they be pure??
5. Again: So it's impossible to find the pH of a solution given only the molecular concentrations!
6. This is where I get confused. Given: [H+][OH−]/[H2O]=1.8x10−16 [H+]=[OH−]=1.0x10−7 And: [H] = 992.1 m/l [HO] = 58.8 m/l [H2O] = 55.5 m/l How can: (992.1*58.8)/55.5 = 1.8x10−16 ? 992.1 = 58.8 = 1.0x10−7 ?
7. So it's impossible to find the pH of a solution given only the molecular concentrations?
8. Hi All, This should be easy, but I can't seem to find it on the 'net. I'm trying to get my head around calculating the pH of a solution given its chemical makeup. I had hoped that starting with something easy, like water, would help me. But all the research and attempted calculations don't add up. The equilibrium equation of water is Kw mol2 dm-6 = [H3O+]mol dm-3 [OH-]mol dm-3 I'm told that Kw is 1.0 x 10-14. (Why? Where did this come from? Was it just made up because the pH scale only goes to 14??) I've calculated [H3O+] to be 19.02322 g/mol or 0.01902332 mol dm-3 and [OH-] is 17.00734 g/mol or 0.01700734 mol dm-3 First, do I have the correct values for [H3O+] and [OH-]? Secondly, I can't balance the the equation as 10-14 ≠ 0.0003235360711688! Where am I going wrong?
9. Can anyone provide the calculations to compensate for the Boron?
10. Thanks for the link exchemist, However I know what Boron is used for. I just don't know if the Boron levels affects the amount of Hydrochloric Acid I require.
11. Hi All, One of the pH adjustment programs I use takes the amount of Boron in the water into account. I'm not sure it matters - So I'd like to know if the Boron concentration in pool water affects the amount of Hydrochloric Acid required. If so, how? Is there a formula I can use to adjust for the amount of Boron? Thanks in advance, Buddy.
12. I, too, suspect that it's iron stains. The stains sometimes appear at the spot where I pour the salt into the pools. The salt I use is highly refined pool salt - ultra-fine pure white crystalline salt. However I don't think they remove all the contaminants, too costly. Here's what Fishel Pools says about pool salt: I think you're right about the chelation, here's what I found at PubMed: Amazing stuff, hey?
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