Which of the following is a weak acid?
959167
HNO2...all others are strong acids.
703155
No surprise at all, the transition does not take place at an pH of exactly 7 but already before. Take a look here for a graph:\n\nhttp://antoine.frostburg.edu/chem/senese/101/acidbase/faq/indicating-strong-or-weak.shtml
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
771216
weak bases only dissociate a very small amount, while strong bases dissociate almost fully.
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...............
774155
This dissociates into Cl- and\n(CH3)2NH2+\n\nCl- is an extremely weak base, so weak in fact that it is neutral\n\n(CH3)2NH2+ on the other hand is a regular weak acid that will make the solution acidic.
628182
HCl would work best.  Sulfamic acid is a weak acid that although easier to handle is more expensive and less effective.  HCl is cheap, but when concentrated can fume, and is more likely to produce Chlorine gas if you acidify something chlorinated with it.
62342
Acidity is when an excess of H+ binds H2O as H3O+.  Strong acids are ones like HCl, which in solution will ionize completely--Cl-, being very soluble, will let go of H+ to make the solution acidic.  Other "weak" bases are ones that do not necessarily ionize completely.  Excess H+ will bind to sites in the weak acid molecule rather than binding to H20, meaning that the pH will not be as low (low pH < 7 = acidic).  In this way, a weak acid can act as a buffer--in pure water, it will ionize to a certain extent, but with excess H+, it will bind more H+, but the free H+ in solution will only change very little, and the pH remains rather stable.
117085
Buffering, in chemical terms, is a weak acid and its cooresponding salt or a weak base and its cooresponding salt.  The idea is that the weak acid will go to an equilibrium like the following example.  Suppose that I have a weak acid HA and the salt with the anion A-.  The acid will go into equilibrium:\nHA <---> H+ + A-\nWhat will happen is that if you add H+ ions to the buffer solution (acids will add H+ ions), they will be consumed into the reaction to become more HA.  If you add a base (adding OH- ions), it will react away H+ to form water and force more A- to form.  Either way, this buffer system will resist a change in pH.  That's what buffers do. \nBuffers are essential in our body because even though we consume all of these orange juices and sodas, which are both acidic, our body needs to maintain a very precise slightly basic pH, or else we could die.  This is done with CO2 in solution in our bodies.
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)
357070
The equivalence point is where all the reactants have reacted.  Since you have a strong base and a weak acid, the pH of the base pulls it over to the basic side of the scale rather than neutral.  Simply, there are more OH- ions than H+ ions total.  All the H+ ions are reacted so you are left with extra OH- ions.  Also works vice-versa.
449522
http://en.wikipedia.org/wiki/Sulphuric_acid
30400
Sulfuric Acid- just learned that today... check the link for more info...\nit is a VERY strong 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.
829401
Basically, water in pure water the water molecules will undergo autoionisation which will produce to types of ions namely H+ and OH- ions. Anyway it is a reversible reaction where H2O exist in equilibrium with H+ and OH- ions. \n\nWhen a strong acid is dissolved in water, it will disscociate completely to produce H+ ions and the anions. This is a forward and non-reversible reaction. Whereas when a weak acid is dissolve in water only part of it will dissociate and the degree of dissociation depends on is solubility constant. This is a reversible reaction.\n\nWhen an acid is mix with water both the acid and the water will contribute its proton. ( acid dissociate completely and water partially.) But the proton from water is so little and can be neglected so normally the concentration of the H+ ions of the acid is used for calculation.\n\nHope this helps.... Good luck..
152537
Citric acid is a weak acid, while sodium hydroxide is a strong base. The sodium would fall off the hydroxide (because it's strong), so the reaction would be:\n\nHC6H7O7 + OH- --> H2O + C6H7O7
819664
The lone pair of electrons on the Nitrogen atom of Ammonia, is available for donation. That is why ammonia is considered as a base. \nBut it not as readily available as it is From OH- radical or other basic radicals. So it is much weaker than them.\nIn aq. soln, NH3 combines with water to form a very weak electrolyte NH4OH, which gets dissociated to a very small extent furnishing only a few OH- ions. So the aq. soln. of NH3 is also mild basic.\n\n Ammonia acts both as a weak base in the Brernsted-Lowry sense\nNH3 + H2O = NH4(+) + OH(-)and\nas a complexing agent (Lewis acid) with some metal ions\nZn(2+)+ 4NH 3 + Zn(NH3)4(2+)\nBoth weak and strong bases produce hydroxide ion in solution which precipitates some metal ions, e.g.\nA13(+) + 30H- + Al(OH)3(s)\nand Zn92+) + 20H- + Zn(OH)2(s).\nThese precipitates appear as flocculent white solids which settle slowly from solution. In higher\nconcentrations hydroxide ion acts as a complexing agent for amphoteric cations, e.g.\nZn(OH)2(s) + 2OH- -+ Zn(OH),2-\nAl(OH)3(s) + OH- -+ A1(OH)4-\nThis experiment demonstrates the action of OH- and NH3 on Al”(aq) and Zn*‘(aq) ions.\n\nAlthough ammonia is well-known as a base, it can also act as an extremely weak acid. It is a protic substance, and is capable of dissociation into the amide (NH2−) ion, for example when solid lithium nitride is added to liquid ammonia, forming a lithium amide solution:\n\n        Li3N(s)+ 2 NH3 (l) → 3 Li+(am) + 3 NH2−(am)\n\nThis is a Brønsted-Lowry acid-base reaction in which ammonia is acting as an acid.\n\nI think you are interested about dry ammonia.