How do balance calcium hydoxide with phosphoric acid?
812798
3Ca(OH)2+2H3PO4>Ca3(PO4)2+6H2O
869137
2H3PO4 + 3Ba(OH)2 ---> 6H2O + Ba (PO4)2 +  2Ba
874983
1. Molarity = concentration and it expressed as mol per dm^3\n    Change the mass to mole and the 851 ml to dm^3. Then find   \n    the ratio of the number of moles to volume in dm^3\n\n2. Soluble ionic compounds breaks up the water molecules in H^+ ions and OH^- ions. Sodium carbonate give Na^+ ions and CO3^2- ions......Other ions that are present are HCO3^- ions called hydrogen carbonate ions. I have found that a solution of sodium carbonate is alkaline: implying that there are more OH^- ions to H^+ ions, due to the formation of HCO^- ions.\n3. OH^- (aq) + H^+(aq) ----> H2O (l)\n4. H^+ ions (ie. hydrogen ions), OH^- ions (ie. hydroxyl ions),\n   Ca^2+ calcium ions and Cl^- chloride ions\n5. Hydrogen ions, hydroxyl ions. ammonium ions and sulphate ions.\n6. Actually the calcium metal reacts with water to give hydrogen gas and calcium hydroxide. At the same time, calcium reacts with nitric acid to give calcium nitrate, water and brown nitrogen dioxide gas.\nHence there is no simple ionic equation for your question\nYou may want to consider this one:\nCa^0  +  2H^+   + 2OH^-  -----> H2(g)  + Ca^2+  + 2OH^-\n7. Hydrogen ions, hydroxyl ions, iron (III) ions Fe^3+  and sulphate ion SO4^2-
898270
Calcium Phosphate is insoluble, so it will precipitate.\n\nThere is no all the time rules, just trends\nNa, Li, K, are almost always soluble.\nCL, F, I, Br, NO3 are almost always.\n\nAs you move towards the middle of the periodic table, it becomes less soluble
383957
if you want a pH 7 buffer use potassium dihydrogen phosphate and disodium hydrogen phosphate in equal quantities.
1175708
It is Calcium and phosphrus.
458904
Well,if CaCO3 + 2H20 = Ca(OH)2 + H2CO3\n\nthen the products of chalk in water are:\n\n(1) Calcium hydroxide (Ca(OH)2) and carbonic acid (H2CO3)\n\nThis is an exothermic reaction: it gives off heat.\n\nFurther reaction between Calcium hydroxide and the carbonic acid produces Calcium bi-carbonate (Ca(HCO3)2) and water (H2O). \n\nCa(OH)2 + 2H2CO3 = Ca(HCO3)2 + 2H2O.\n\nCalcium bicarbonate is baking powder, and it is safe, and even medicinal as an antacid.\n\nThe feasibility or otherwise of the above chemical reactions is now left to chemical thermodynamicists to confirm, while the speed or sluggishness of the reactions is for kineticists to compute.
814262
H2SO4 + H20 -> H2SO4:H2O (water decreased)\nHNO2 + H2O-->NH3 + O2   (you balance it)\nNaHSO3 + H2O-->H2SO3 + NaOH(you balance it)
248591
CaO + H2O => Ca(OH)2\n\ncalcium oxide + water => calcium hydroxide\n\nThis is a great site for this - the reaction between CaO and water is an exothermic reaction (1)\n\nthe second reference is even better - not simply a diagram but a torn apart "self-heating" can\n\ngood luck!\n\nSomething else you might want to looking - MRE's (meals ready to eat)
795289
If the solution contains a diprotic acid, there are two hydrogen atoms available for the acid to lose (such as H2SO4).\n\nA solution of 50mL of a 1.012 M solution would contain 0.0506mol of diprotic acid which would then dissociate to give you 0.1012mol of H+ ions. \n\nThen you must have as much hydroxyl anions (OH-) as you do hydrogen ions (H+), so you must have 0.1012mol of OH-. Using the formula 2H+ + 2OH- -----> 2H2O.\n\nTo convert 0.1012mol OH- into grams of Mg(OH)2, you divide the OH- concentration in half because of the equation\nMg2+ + 2OH- -----> Mg(OH)2\n\nwhich would give you the 0.0506mol Mg(OH)2.\n\nFinally you would convert the 0.0506mol Mg(OH)2 into grams Mg(OH)2 by multiplying the number of mol by the molecular weight of magnesium (II) hydroxide--the calculation is shown below:\n\n0.0506mol x 58.31g/mol = 2.95 g Mg(OH)2\n\nSo you would need 2.95 grams of Mg(OH)2 to neutralize the solution. \n\nHope this helps!!
957775
Ca(OH)2 + CO2 --> C(OH) + CaO\n\nIs unbalanced..
972791
HCl + NH4OH → H2O + NH4Cl.\nThere would be heat given off, so you could verify that a reaction took place.\n\n2HCl + Ca(OH)2 → 2H2O + CaCl2\n\nedit: The steps for balanacing the reaction:\n1)We know the salt produced is CaCl2, so an acid with Cl is HCl and a base with Ca is Ca(OH)2. \n2) write the skeleton reaction:\nHCl + Ca(OH)2 → H2O + CaCl2\n3) there are 2 Cl's on the right side, but only 1 on the left. To balance this, place a 2 in front of HCl\n2HCl + Ca(OH)2 → H2O + CaCl2\n4) Now there are 4 H on the left and only 2 on the right, so, place a 2 in front of H2O.\n2HCl + Ca(OH)2 → 2H2O + CaCl2\n5) check with the other elements, each side has one Ca, and 2 O. It all works out ☺
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.
779355
make a mixture of half baking soda and half water. then apply it to where the acid is. This is great for when you have to clean the prongs on the battery. Be careful not to touch the acid.
356281
MgCO3 + 2HCl ---> MgCl2 + CO2 + H2O\n\n2HCl + MgO ---> H2O + MgCl2\n\nBarium hydroxide is a base so can be neutralised with any acid.  An example being HCl.\n\nBa(OH)2 + 2HCl ---> BaCl2 + 2H2O\n\nor H2SO4\n\nBa(OH)2 + H2SO4 ---> BaSO4 + 2H2O
73319
the earlier equation is not balanced.\nCaO + 2HCl --------> CaCl2 + H2O
371226
Calcium(Ca+²) and Magnesium(Mg+²)