whats the balanced chemical formula of  potassium permanganate & hydrochloric acid?
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
264737
Dissolve the following in 800ml distilled H2O.\n8g of NaCl\n0.2g of KCl\n1.44g of Na2HPO4\n0.24g of KH2PO4\nAdjust pH to 7.4 or 7.6 with HCl.\nAdjust volume to 1L with additional distilled 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)
821226
1. sodium hypochlorite\n2. hydrogen chloride\n3. concentrated sulphuric acid\n4. oxidising it, for example with potassium manganate(VII).\n\nIf you've done the other 96, well done!
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.
906651
2KOH=>K(2)O+H(2)O\n\nFeO+C=>CO+Fe\n\nCa+2AlCl=>CaCl(2)+2Al\n\nP(2)O(5)+3H(2)O=>2H(3)PO(4)\n\n2KI+Pb(NO3)2=>2KNO(3)+PbI(2)
713170
K2CrO4 +Pb(NO3)2 ---> PbCrO4(s)  + 2KNO3\n\nNice yellow ppt.
262227
any oxidative substance (potassium permanganate), ultraviolet rays, sun, air, hydrogen peroxide, etc
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.
746627
Cl2 + 2KI --> 2KCl + I2\n\nsingle replacement
866145
HCl + AgNO3-----> AgCl +HNO3\nPb(OOC-CH3)2  + 2LiCl -------> PbCl2  + 2Li(OOC-CH3)\nNa3PO4 + CrCl3 -------> Cr(PO4) + 3NaCl\nH2SO4 + BaCl2 ----------> BaSO4 + 2HCl\nAl2(SO4)3  + 6NH4OH ------> 2Al(OH)3  + 3(NH4)2SO4\n2AgNO3 + H2S -------> Ag2S  + 2HNO3\nCaCl2   + Pb(NO3)2 -------> Ca(NO3)2  + PbCl2\nCa(NO3)2 + Na2CO3 ------>CaCO3  + 2 NaNO3
212037
I think you are talking about Aluminum zirconium tetrachlorohydrex gly (used in anti perspirants). the molecular formula is\n\nAlyZr(OH)3y+4-xClxmGlynH2O
251148
Assume we have 100g hydroxylamine hydrochloride. Then we would have 5.80 g H, 20.16 g N, 23.02 g O and 51.02 g Cl.\n\nFind the moles of each element in the compound: \n\n5.80 g H / 1.008 g/mol H = 5.75 mol H\n\n20.16 g N / 14.01 g/mol N = 1.44 mol N\n\n23.02 g O / 16.00 g/mol O = 1.44 mol O\n\n51.02 g Cl / 35.45 g/mol Cl = 1.44 mol Cl\n\nSo the formula is: N1.44 H5.75 O1.44 Cl1.44\n\nNow divide by the smallest number: N1.44/1.44 H5.75/1.44 O1.44/1.44 Cl1.44/1.44\n\nSo the empirical formula is: NH4OCl
724799
Aluminium is Al3+\n Chlorine is CL1-\n Potassium is K1+ \n\nHahaz, I think should be correct. Hahaz, I did your homework.
43725
Bleach\nsodium hyporchlorite has HCL in it\nMuritic acid
498295
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+: \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 [1]. The same trick can be used to remove indelible inks from concrete [2]. Photographers use permanganate to bleach stains caused by certain developing chemicals. \n\nReferences\nBookbinding and the Conservation of Books, D. Etherington and M. T. Roberts. URL: http://palimpsest.stanford.edu/don/dt/dt2556.html, viewed 10/06/99 \nCBD-153. Removal of Stains from Concrete Surfaces,V.S. Ramachandran, J.J. Beaudoin, National Research Council Canada (1972). URL:http://www.nrc.ca/irc/cbd/cbd153e.html, viewed 10/06/99
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!!!