What is the strongest acid known?
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well this question was asked two days before.\nsearch for this question u'll get all the knowledge\nstrongest oxo-acid-- HClO4\nstrongest protonic acid--H2SO4\nstrongest lewis acid----SBF5\n btw HF is not consider very strong bcoz F is very small atom and it does not loose H+ very easily.\n\nEDIT: Question(very odd name) there has been acids with negative pH and 0 pH( 0pH is more stronger than 1)
856196
Phosphoric acid, monobasic is a stronger acid (pKa ~ 7) compared to hydrogen cyanide (pKa ~9).  The hydrogen from HCN just doesn't want to dissociate as quickly.\n\nIt is true that phosphoric acid, monobasic once dissociated will then be HPO4(--), but this has a pKa of about 12, which is three orders of magnitude weaker than HCN.
910938
Na+ and K+ (both group 1)\nCa2+ and Mg2+ (both group 2).\nNa+ and Mg2+ have the electron arrangement of neon, and the other two that of argon.\nIonic radius decreases from left to right, and increases top to bottom, so K+ is the largest of all these.\nElectronegativity increases upwards and to the right of the Periodic Table, so Mg has the highest value of these four.
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<--------- 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)
83361
It's not really a valid question. The only diprotic strong acid is sulfuric acid (H2SO4) with the loss of its second proton being weak. Otherwise, diprotic acids are weak.\n\nIf you're asking for a comparison between something like HCl or HNO3 and H2SO4, you'd have to consult chemical literature.
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acid\ngas naphtha\noxygen  and hydrogen\nacid\nacid
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The greater the Kb value is, the stronger the base.  Just think about what Kb means.  On the left side of the equilibrium is the base, on the right side is the conjugate acid, meaning the base has reacted.  The stronger the base, the more it will react, the more the reaction will proceed to the right, the greater Kb will be.\n\nSo.....\n\nC > E > B > A > D
556259
strong acids have a high tendency to donate protons (hydrogen ions) and strong bases have a high tendency to receive them.  \nstrong acids have a very low pH, 1-3\nweak acids have a ph of about 3-6\npH 7 - neutral solution\nweak bases have phs of about 8-11\nstrong bases - ph 11-14
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d. 100% of the max number of hydroxide ions.\n\nIn chemistry, strong base or strong acid is not a degree of how much it would eat you alive if you got it on you, but the degree in which it disassociates in water.
732674
HBr is a strong acid because of Bromine's electronegativity.
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Triangles I did a project like that. Triangles are the strongest.
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KOH, potassium hydroxide, is a strong BASE.\nHNO3, nitric acid, is a strong ACID.\nNH3, ammonia, is a weak BASE.\nMg(OH)2, magnesium hydroxide, is considered a weak BASE due to it's limited solubility in water.\n\nTherefore, only HNO3, nitric acid, is NOT a base.
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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.
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Hydrogen has the highest known specific heat of 1.43 x 10^4  J/kg*K at a temperature of 25°C.
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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.
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Milk, bleach, Maalox, Tums, chalk...anything that neutralizes an acid.
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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.