Can anyone rank these acids strongest to weakest: HCL, H2SO4, and H3PO4?
402204
H2SO4 - HCl - H3PO4 - HSO4(1-) - H2PO4(1-) - HPO4(2-)\n\nHCl is quite strong, but suffers the disadvantage at atmospheric pressure that it is volatile and will dissolve in water only up to 37%. It can be driven out of watery solutions by addition of less volatile but not necessarily stronger acids.\n\nH2CO3 would rank fairly high in this list too if you could prevent the CO2 from evaporating.\n\nWhen ranking H2SO4 and H3PO4 you'll have to state how far you want the protolysis to go. Taking the average of H2SO4 and HSO4(1-) makes it weaker than HCl, and worse so for H3PO4.
114804
No need to break it down to "molecular" other wise, try this: Sodium thiosulphate. Dont just use it coz they all vary in their Ph U know the basisity or acidity they concentrate.
728160
1. C, 2. Cl, 3. Se. The closer the atom is to Fluorine on the Periodic table (excluding noble gases), the stronger the electron affinity. Fluorine is the strongest.
2508
Weak acids and organic acids in water.\n\nBut remember the solution depends on what the solvent is.  In water, the seven strong acids essentially completely ionize...i.e. can be considered completely ionized.
30400
Sulfuric Acid- just learned that today... check the link for more info...\nit is a VERY strong acid!
804052
The conjugate acid of any base B: is HB.  So the answers are HF, HSO4-, NH4+, and H2S+.  (Are you sure that wasn't supposed to be HS- and H2S?)
152640
Phosphorus forms only oxy-hydroxides, like phosphoric acid (H3PO4), which could be written as PO(OH)3. There will always be one H2O less than theoretically possible.
160963
K2SO4 ---> 2K+  +  SO4-\n\nHCl ---> H+  +  Cl-\n\nNaHCO3 ---> Na+  +  HCO3-\n\nNH4OH ---> NH4+  +  OH-\n\nBaCl2 ---> Ba-2  +  2CL-\n\n(NH4)3PO4 ---> 3NH4+  +  PO4-3
747313
1) Zinc Chloride\n2) Copper (II) Sulphate\n3) there is no such thing as NH4OH, but oh well..\n    Ammonium Hydroxide\n4) Iron (III) Sulphide\n5) Aluminium Phosphate\n6) Lead (II) Nitrate\n7) Sulphur hexafluoride\n8) Sodium Sulphate\n9) Mercury (II) oxide\n10) Potassium Clorate (V)\n11) Tin (II) Choride\n12) Iron (II) hydroxide\n13) Mercury (II) Sulphate\n14) Carbon Dioxide
596849
2 - Potassium Chloride\n\nIt has, by far, the weakest covalency of all those listed, and therefore breaks apart most readily.
290781
MgSO4(s) + 2HCL(aq) ---> H2SO4(aq) + MgCl2 (aq)
271476
pH = 4.75\n\ntechnically, the pH can be anything.  But, for the most effective acetic acid buffer, the pH would be 4.75 because the pKa of acetic acid is 4.75.  When the pH = pKa, the amount of acid and base are equal, thus its resistant to pH changes is greatest.
235017
i think #5 is lactic acid
449522
http://en.wikipedia.org/wiki/Sulphuric_acid
520869
A weak acid does not dissociate fully while a strong acid dissociates completely.\n\ne.g. HCl --> H+ + Cl-\nIf you have 0.1M of HCL, you will also have 0.1M of H+.\n\ne.g. CH3COOH <==> CH3COO- + H+\nIf you have 0.1M of CH3COOH, you may only get 0.01M of H+ as some of the CH3COOH does not dissociate to form H+.\n\nAn example of a weak organic acid is propanoic acid, C2H5COOH.
866949
<--------- 7 ---------->   (pH)\nacid                base\n\nthe smaller pH the stronger acid\nthe bigger pH the stronger base\n\nso you should arrange them from the smallest pH to the biggest\nstomach content (1.6)\nsoda pop (3)\nmilk (6.5)\nfresh water (7, of course neutral)\nhuman blood (7.4)\nsea water (8.7)\ndrain cleaner (8.7)
179919
Hydroflouric acid is a strong electrolyte because of hydrogen bonding.\nI am almost positive that ammonia is a weak electrolyte.\nI think Nitric acid is a nonelectolyte. \n\nI hope this helps. Sorry if I am wrong.