what is the chemical equation between Potassium Permanganate and Oxalic Acid?
830133
One must have to use acid (sulfuric, usually) for this reaction to proceed so the equation becomes\n2 KMnO4 + 5 H2C2O4 + 3 H2SO4 = 10 CO2 + 2 MnSO4 + 8 H2O\nIf you still dont want the acid in the equation then at least you have to leave the H ions there or you'll never be able to solve it.\n\nthe equation without acid is \n2 MnO4\n(-1) + 5 H2C2O4 + 6 H(+1) =  10 CO2 + 2 Mn(+2) + 8 H2O\n\nNote that the parantheses indicate the charge on the ion.
819244
a) Acid +H2O -> H3O(+)+ Basis\n\nKa1 =  x²/(0.1-x) = 10-4\nx<< 0.1 so x = 10-3\n\nso pH = 3\n\n2) second dissociation\nKa2 = y (10^-3 + y) / (10^-3 -y)\ny << 10¨-3\ny = Ka2 = 10^-8
651011
H2O2 + OC(NH2)2 -> HCOOH + NH4OH -> NH4(HCOO)
164971
BaCl2 + Na2SO4 --> BaSO4 + 2NaCl is the chemical reaction. \nNet ionic equation: Ba(2+) + SO4(2-) --> BaSO4 \nTotal ionic equation: Ba2+ 2Cl- + Na+ + 2SO4(2-) --> BaSO4(s) + 2Na+ + Cl-\nBarium sulfate is a classic precipitate.  \n\nAll of the masses of these compounds can be calculated by adding the individual ions' masses together, which is the same as atomic masses on a periodic table.   \nBarium chloride: 208.25 g/mol\nSodium sulfate: 142.04 g/mol (anhydrous)\nBarium sulfate: 233.43 g/mol \nSodium chloride: 58.4 g/mol
91741
What are the states of each of the substances?\n\n\nammonium chloride(aq)+potassium hydroxide(aq)---->ammonium hydroxide(aq)+potassium chloride(aq)\n\n   Complete ionic equation\nNH4+(aq)+Cl-(aq)+K+(aq)+OH-(aq)------->\nNH4+(aq)+OH-(aq)+K+(aq)+Cl-(aq)\n\n     Net Ionic Equation\nSame as complete ionic equation, every ion is a spectator ion, OR it doesn't exist.\n\nI don't think both substances are in aqueous solution.
562872
Potassium manganate or potassium permanganate?  And I'm assuming a solution of iron(II).\n\nBeyond the corrosivity of the sulfuric acid, and the oxidizing capability of the manganese species, as well as its ability to stain EVERYTHING, there are no additional hazards.  Permanganate stains can be removed by addition of an hydroxylamine solution (either the sulfate or the chloride).
620217
HOCl <==========>  H+  + OCl-\n\nthe pKa of hypochlorous acid, HClO, is 7.4 at 25°C, so:\n\npKa = -log [Ka] = 7.4, therefore\n\nKa = 3.98 x 10^-8\n\nKa = [H+]*[OCl-]/[HOCl] = 3.98 x 10^-8\n\nfrom your problem, you state that you have 1.0M HOCl, and since the only source for ions is the HOCl dissociating;\n\n[H+] = [OCl-] = y, and [HOCl] = 1.0-y\n\nsubstituting this back into the Ka equation, we get:\n\n3.98 x 10^-8 = y^2/(1.0-y)\n\nwhich converts into the quadratic equation:\n\n0 = y^2 + (3.98x10^-8)y - 3.98x10^-8\n\nI leave it to you to solve the quadratic equation to get y = [H+], and then calculate the pH of the starting solution
764101
In all reactions one uses that 2 OH -> H2O + O, the split of oxygen goes to create the ion. Finally balance the equation:\n \nSO3 + 2 NaOH -> Na2SO4 + H2O\n\nCO2 + 2 KOH -> K2CO3 + H2O \n\nSO2 + Ba(OH)2 -> BaSO3 + H2O
706351
KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
803319
Potassium Permanganate dissolves easily in water.  Iodine is only slightly soluble in water, but it dissolves really well in non-polar solvents such as ethanol, dichoromethane, etc.
917456
With hydrochloric acid the equation is:\n\n16HCl  +  2KMnO4  =  2KCl  +  2MnCl2  +  8H2O  +  5Cl2\n\nand with sulphuric acid :-\n\n2KMnO4  +  3H2SO4  =  K2SO4  +  2MnSO4  +  O2
948592
Kc=2 = conc products / conc reactants\n\nKc = 2 = [CO][H2O]/[CO2][H2]\n\nStarting concs\n[CO] and [H2O] = 0\n\n[CO2] and [H2] = 0.7 moles/10L = 0.07M\n\nEquilibrium concs\n\nFrom the balanced equation, if x CO2 reacts, it reacts with x H2 to form x H2O and x CO\n\n[CO] and [H2O] = x\n\n[CO2] and [H2] = 0.7 moles/10L = 0.07M-x\n\n\nKc=2=(x)(x) / (0.07-x)(0.07-x)\n\nsolve for x and plug back into the final concentration equations.
782974
Potassium permanganate (KMnO4) stains fabrics, fingers, and paper a dark brown color. The coffee-colored stains often can't be scrubbed off, and they may persist until the outer layer of stained skin wears off (in a day or two). It's more than just a nuisance for students and laboratory workers. Municipal water supplies are sometimes overtreated with permanganate ion to kill microbes and parasites, and when that water is chlorinated, swimming pools and porcelain can be badly stained.\nPermanganate itself is a deep purple color (almost black). The brown stain develops when permanganate decomposes into crystalline manganese dioxide on the skin or fabric surface:\n\n4 MnO4-(aq) + 4 H+(aq) = 3 O2(g) + 2 H2O() + 4 MnO2(s)\n\nThe tiny crystals of MnO2 become trapped in the pores and complex surfaces of the skin. The crystals are insoluble, and washing with water will only dislodge a few loose crystals. If the stain is on a nonliving surface, try treating it with a weak hydrochloric acid solution. Hydrochloric acid can reduce the MnO2 to water-soluble Mn2+:\n\nMnO2(s) + 4 HCl(aq) = MnCl2(aq) + Cl2(aq) + 2 H2O()\n\nCuriously, permanganate's oxidizing power makes it very useful for removing stains. Permanganate oxidation breaks the molecules of large, highly colored substances into smaller pieces. The excess permanganate is then removed chemically or by quickly rinsing.\n\nFor example, book collectors remove stains from old paper by washing the paper with a weak solution of permanganate; a rinse of sulfurous acid is used to remove the permanganate before it locks into the paper fibers and turns it brown. The same trick can be used to remove indelible inks from concrete. Photographers use permanganate to bleach stains caused by certain developing chemicals.\n\nHope that helps!!!
708721
Here is the right equation for nitric acid and sodium bicarbonate\n\n\nHNO3 + NaHCO3 ---> NaNO3 + H2O + CO2\n\nIf you do not like the sodium:\n\nHNO3 + HCO3(-) --> NO3(-) + H2O + CO2
752218
2KOH + Cl2 ----> KCl + KClO + H2O\n6KOH + 3Cl2 ----> 5KCl + KClO3 + 3H2O
455269
H2SO4 + Mg(OH)2 -> 2H2O + MgSO4
81025
alkaline potassium permanganate test