There is no such acid which is both strong and weak. An acid is either weak or it is strong.
However, sulfuric acid as a diprotic acid is a strong acid in its first dissociation.
H2SO4 --> H+ + HSO4-
and is a weak acid in its second dissociation
HSO4- --> H+ + SO42-
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It is a strong acid only for the first hydrogen ion that is produced.
(1) H2SO4 --> H+ + HSO4^-
The remaining bisulfate ion, HSO4^-, is a weak acid and only partially dissociates.
(2) HSO4^- <==> H+ + SO4^2-
A misconception is that since sulfuric acid is a strong acid, that it dissociates like this:
(3) H2SO4 --> 2H+ + SO4^2-
That simply isn't the case except for extremely dilute solutions. As the concentration of the acid decreases, the acid behaves more and more like a strong diporotic acid. At "infinite dilution" it is accurate to write the dissociation as equation (3).
Read more: http://wiki.answers.com/Q/Is H2SO4 a strong acid or weak acid#ixzz2TQB85UJp
A strong acid disassociates completely or nearly completely when diluted with water. A weak acid will not disassociate completely, or even hardly at all.
For example, if you have a strong acid solution, such as hydrochloric acid (HCl - a strong acid) and add baking soda, (sodium carbonate), the free hydrogen ions (the H in the HCl) in the solution will bind with the carbonate portion of the sodium carbonate to make Carbonic Acid - a weak acid. Carbonic Acid is weak, so it binds the ions, and lowers the acidity of the solution. The Sodium and Chlorine form table salt, if the solution is dried.
The idea here is that the carbonic acid does not completely disassociate in the water - in other words, the hydrogen ion does not separate from the carbonate in water - maybe only 10% will disassociate. HCl is another matter - it's a very strong acid, where 100% of the molecules dissassociate.
PHP, THC, XanX, LFP
No. Many strong electrolytes are bases or neutral salts.
Buffer systems. They convert strong acids or bases into weak acids or bases.
yes
Strong acids are acids that dissociate readily from their hydrogen ion(s). Examples include: Strong acids HCl, hydrochloric acid HNO3, nitric acid HI, hydroiodic acid H2SO4, sulfuric acid HBr, hydrobromic acid HClO4, perchloric acid HClO3, chloric acid Weak acids do not dissociate readily from their hydrogen ions. They, therefore, act weakly as an acid. All edible acids are, naturally enough, weak acids. Examples include: Weak acids HCN, hydrocyanic acid (COOH)3C3OH, citric acid tartaric acid, lactic acid, oxalic acid ...
This is based on acids. HNO3 is a strong acid.
Weak acids have a larger value of pKa than strong acids
True organic acids are weak acids but alpha substituted acids may be strong as 'trichloric acetic acid is a very strong acid.
Lowest pH, strong acids, then weak acids, then salts of strong acids and strong bases, then salts of weak acids and strong bases, then weak bases, then strong bases. All very confusing!
acids are of types.....concentrated acids are strong.
Weak Acids
The acids ability to disassociate completely in solution. Strong acids do and weak acids do not.
strong acid
Mineral acids are strong acids.
The acids ability to disassociate completely in solution. Strong acids do and weak acids do not.
it is weak and strong because it neutralises acids. So its strong not weak but weak not strong.
strong acids
Strong acids dissociate completely in aqueous solution; weak acids do not.