I need a substance that will change hydroxyapatite, Ca5(PO4)3OH, to fluorapatite, Ca5(PO4)3F. Can anyone help?
488406
I'm guessing HF, but be very cautious because it's a nasty acid\nI found something new,fluoridated water, which will allow exchange in the teeth of hydroxyl ions for fluoride ions, slightly strengthens the teeth(from wikipedia).Maybe you don't need too use HF after all :)
177902
Well, it's not easy. Phosphoric acid is H3PO4. Phosphorus is at an oxidation state of +5. If you want it to reduce to plain phosphorus (ox. state of 0), you'll need something to oxidize. If you're not a professional chemist, it'd be much, much, much easier just to buy some phosphorus.
328050
NaPO3F is also a reintegrator of phosphate (PO4---) so it can be useful not only for teeth.
634218
There really is not a set formula, as the -ite anions don't have a set formula themselves (PO3 2- for phosphite, NO2- for nitrite, SO3 2- for sulfite, Cl02- for chlorite, etc.)
861843
Start with the Ca then balance the number of PO4 ions, then balance the Oxygen and the hydrogens should balance themselves out.  Its just trial and error. Monkey with it until it works.
494638
P3O10 does not exist; it's P4O10.\n\nBalanced equation is:\n\nP4O10 + 6H2O --->  4H3PO4
869137
2H3PO4 + 3Ba(OH)2 ---> 6H2O + Ba (PO4)2 +  2Ba
161218
Calcium hypclorite (sp) The combination oxidizes, the coloring agents, kills the bacteria by providing a very acid inviroment
1101513
Your question is not very clear, however I am attempting it.\n1:  1 mol of Na3PO4 will have 3 mol of Na and 1 mol of PO4 ions.\n2:  2.5 mol of Na2SO4 will have 5 mol of Na and 2.5 mol of SO4 ions.\n3: 3 mol of CaSO4 will have 3 mol of Ca and 3 mol of SO4 ions.\n4: 4 mol of NH4NO3 will have 4 mol of NH4 and 4 mol of NO3 ions.
986414
Start by balancing the equation:\n2Ca3(PO4)2 (s) + 6H2SO4 (aq)-----> 6CaSO4 (s) + 4H3PO4(aq)\n\nThen figure out the molar masses of each of the reactants:\nCa3(PO4)2 = 3(40.078) + 2(30.973762) + 8(15.9994) = 310.176724\n\nH2SO4 = 2(1.00794) + 32.065 + 4(15.9994) = 98.07848\n\nDivide each of your known masses of reactants by its respective molar mass to determine how many moles of each you have, and divide this number by the coefficient (the number in front) of the reactant to determine how many "parts" of each you have:\n(1000/310.176724)/2 = 1.612 parts 2Ca3(PO4)2\n(980/98.07848)/6 = 1.665 parts 6H2SO4\n\nTake the smaller number (since once you run out of one reactant, the reaction is over) and figure out how many moles of calcium sulfate and phosphoric acid you'll produce:\n(1.612)(6)(40.078 + 32.065 + 4(15.9994)) = 1316.7518832g CaSO4\n\n(1.612)(4)(3(1.00794) + 30.973762 + 4(15.9994)) = 631.872933536g H3PO4\n\nSince the total mass of reactants and products needs to be the same, you can check your (er, my) work by totalling up both sides:\n(1.612)(2)(310.176724) + (1.612)(6)(98.07848) = 1948.625g\n1316.7518832 + 631.872933536 = 1948.625g
753910
CaF2 is calcium fluoride. Sorry I messed up before.
911306
Aluminium carbonate does not exist, and has never been prepared as the pure compound. All attempts to prepare it result in aluminium hydroxide.
1043803
The chemical mixes are called phosphate eliminators and can be gotten from you pool supply store.  You can't make the mixtures yourself cheaper than you can buy them.\n\nYou can find many web pages on the subject by a simple web search such as\n\nhttp://www.rainbowpoolsinc.com/help/phosphate.htm
495941
We have no idea what data you [we] have to work with here.\n\nWhat did you do in your lab?\n\nI assume you had a saturated solution of Ca(OH)2 which you then titrated with a stron acid like HCl.  You then should have recored the volume and concentration of the acid required to neutralize the Calcium Hydroxide.\n\nWrite out the chemical reaction between Ca(OH)2 and your acid, find the mole ratio between the moles of acid used and the moles of OH- in solution, and solve.
204385
H3PO3\n\nnot H3PO4, which is PhosphoRIC acid
812798
3Ca(OH)2+2H3PO4>Ca3(PO4)2+6H2O
47432
3AgC2H3O2 + Na3PO4 -----> Ag3PO4 + 3NaC2H3O2