why do acid's have to have one or more hydrogen ion?
605960
That's the definition of an acid. Something which has the Hyrogen ion.
708448
This deals with Bronsted-Lowry (B-L) acids and bases, and conjugate-base pairs \n\nB-L acids: donate H+ ions: STRONG ACIDS dissociate into ions\nH20 + HCl --> Cl- + H+  (H+ is the same as hydronium [H3O+])\nso it can be written as H20 + HCl --> Cl- + H3O+ \nThis looks like it donates a H+ ion, but it dissociates because it is a STRONG acid.  \n\nwk acid: HA= wk acid; A- = conjugate base\nHA + H2O ---> H3O+ + A-\n\nB-L bases: accept H+ ions: STRONG bases dissociate\nNaOH + H2O --> H2O + Na+ + OH-\n\nwk base: B = wk base; HB = conjugate acid\nB- + H2O --> HB + OH-\n\nThat's all you need to know to write all eqns.
292346
26 electrons. If it's an electrically neutral atom, then the number of protons must equal the number of electrons.
853143
A stabilizer is often necessary when using H2O2, because that compound tends to decompose, especially in the presence of trace amounts of many metallic ions.  In fact, if even a minute amount of, say, Cu++ is present, the decomposition can be violent.
175315
our stomach has acid in it, HCl so the sodium Bicarbonate neutralizes the acidic protons or hydrogen, B, Cl is just a harmless salt
716161
Well if it's stable, there will be the same amount of protons as electrons. If it has a charge add or subtract. \n(If you have a plus charge, that means there's 1 more proton than electron... if you have a -2 there are two more electrons than protons etc.)
117330
acidity has three different definations.\nLewis Acids - a substance capable of accepting as=n unshared electron from a base to form a dative covalent bond.\nArrhenius Acid - a Hydrogen containing compound that ionises and releases protons, [H+] in an aquous solution,\nBronsted Acid - a substances consisting of molecules or ions which donates protons, [H+].\nif any substances adhere to any of the three conditions, it is an acid. \nthe common theory is the Bronsted theory. this is where the term pH is introduced, where pH means 'potential of H+'. a solution with more H+ ions then OH- ions is an acidic solution. the pH is generally <7. however, this standard varies with temperature, and the concentration of the solute(water). \na general apparatus to determined is the blue litmus paper. it'll turn red on contact with acidic solutions.
573222
Once a solution of HCl hits pH 7, it is considered neutralized (or in other words it'll basically be water.) After a pH of 7, a solution has to be alkaline (or basic,) which an acid cannot be.
750517
if a soln is acidic it will be the OH anions which will be less.....for a soln 2 b acidic it has to hav H- ions...............
682358
basically, we call it an acid if the compound can be resolved into existing H+ and OH- ions. if this can be resolved then it is called acid and base. \n\nThis is pH. amount of H+ ions and amound of OH- ions. more the amount of free H+ ions in the compund more the acidic nature.\nmore the OH more the basic nature and less is the acidic nature.\n\nIt also depends on the medium in which the compound is present. some act as acids in aqueous medium. and so on....\n hope it was helpful. \nAny doubts u can ask further.
204256
The number always comes after the element, so two hydrogen and one oxygen.\n\neg if you have a more complex compound like Sulphuric Acid,\nH2SO4 that would be 2 hydrogen, one sulphur (or Sulfur in the USA) and 4 Oxygen
279663
Well, Sulfuric acid is a diprotic acid. The first proton is a strong acid, and the second proton is a fairly strong weak acid.\n\nBecause it's a strong acid, there will be 18 M of H3O+ ions.\n\n-log(18) = -1.255\n\nTo the correct number of significant figures, the pH is -1.26.\n\nEDIT: dr_futuredentist is very wrong. The second hydrogen\ndoes not dissociate fully at all.
332944
The ability to be a proton donor is the Bronsted-Lowry definition of acids.  The Lewis definition of an acid is an electron pair acceptor, which covers molecules like BF3.  (Exactly what kind of chemistry do they teach at NIU?)\n\nThe ability to accept a pair of electrons is what is common to all acids, not the ability to be a proton donor.
30128
I takes a bit of familiarity.  You need to know which ones will ionize in solution, and how they'll ionize.  Anything that releases a H ion is an acid.\n\nIf you have a specific list, I can try to help; elsewise you're best to look them up individually or study a bunch of inorganic and organic chemistry until you can spot the ionization trends.  In biochemistry, anything with the "-COOH" motif is a carboxylic acid, and is colloquially called an acid.\n\nThere's alos a tendency--though it isn't rock-solid--to write  ionizing substances in a conjugate acid/conjugate base manner.  Generally, things that have H as the first element listed will be acids (H3PO4, HCl, HBr, HI, HF, HNO3, H2SO4, HClO4, H3BO3, H2CO3, and HClO3 are all acids).  Organic acids are not necessarily going to fit into this scheme.
1180433
No.  Any salt has a pH of 7.  Any acid has a pH of less than seven.  They're contradictory.  If you mixed some acid and some salt, I wouldn't call it salt any more.  I'd call it acid.
260820
Binary acids are composed of only two elements: H and some non-metal.  For example - HCl, H2S.  They are named with the prefix "hydro", then the root of the nonmetal's name, then the suffix "ic", then the word "acid".  For the two examples above, these are "hydrochloric acid" and "hydrosulfuric acid".\n\nOxyacids have three elements: H, O, and some nonmetal.  For example - HClO2, H2SO4.  They are named according to the oxidation state of the nonmetal.  Where there are only two stable oxidation states, for example H2SO4 and H2SO3, the higher is named by the root of the nonmetal's name, followed by the suffix "ic" (H2SO4 = "sulfuric acid") and the lower has the suffix "ous" (H2SO3 - "sulfurous acid").  Those with more oxidation states are named similarly to the chlorine series: HClO = "hypochlorous acid", HClO2 = "chlorous acid", HClO3 = "chloric acid", and HClO4 = "perchloric acid", where the prefixes "hypo" and "per" distinguish additional oxidation states below and above, respectively.
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