2006-10-10 04:02:56 · 5 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
As you properly stated, you can identify the conjugate acid in a reaction as the species more protonated (that is why they are able to donate protons), and the conjugate base as the chemical species desprotonated.
For example:
H3O+ is the conjugate acid of H2O in a reaction (you can see that hydronium ion is more "willing" to donate its proton than water)
Cl- is the conjugate base of HCl in a reaction (you can see that Chloride ion is more "willing" to accept a proton rather than HCl)
Here you are with a list of examples found in wikipedia:
Acid..................................................................................... Base
HFSbF5 Fluoroantimonic acid .......SbF6 − Antimony pentaflouride ion
HCl Hydrochloric acid ...........................Cl- Chloride ion
H2SO4 Sulfuric acid ........................HSO4− Hydrogen sulfate ion
HNO3 Nitric acid ..............................NO3− Nitrate ion
H3O+ Hydronium ion........................H2O Water
HSO4− Hydrogen sulfate ion ...........SO42− Sulfate ion
H3PO4 Phosphoric acid.................. H2PO4− Dihydrogen phosphate ion
HC2H3O2 Acetic acid ......................C2H3O2- Acetate ion
H2CO3 Carbonic acid ......................HCO3− Hydrogen carbonate ion
H2S Hydrosulfuric acid .....................HS− Hydrogen sulfide ion
H2PO4− Dihydrogen phosphate ion ...HPO42− Hydrogen phosphate ion
NH4+ Ammonium ion .........................NH3 Ammonia
HCO3− Hydrogen carbonate ion ........CO32− Carbonate ion
HPO42− Hydrogen phosphate ion ......PO43− Phosphate ion
H2O Water (neutral, pH7) ...................OH− Hydroxide ion
Maybe you can see a pattern in the list above.
Hope it helps!
Good luck!
2006-10-10 04:25:26 · answer #1 · answered by CHESSLARUS 7 · 0⤊ 0⤋
It depends on the equations that you have:
Model:
HX + H2O ⇌ X− + H3O+
HX would be the conjugate acid here because it donated a proton and because X - (thus the negative charge).
X - , the base produced, would be the conjugate base.
Example:
CH3COOH + H2O ⇌ CH3COO- + H3O+
CH3COOH is the conjugate acid and CH3COO- is the conjugate base.
2006-10-10 04:17:45 · answer #2 · answered by surgicalgod123 2 · 0⤊ 0⤋
Take any acid
Remove a hydrogen ion (H+)
What's left over is the conjugate base.
ie HCl --> H+ + Cl-
acid Base
2006-10-10 04:31:52 · answer #3 · answered by The Cheminator 5 · 0⤊ 0⤋
a) CH3COOH(aq) + H2O(l) <--> H3O+(aq) + CH3COO-(aq) CH3COOH(aq) - acid, CH3COO-(aq) - conjugate base H2O(l) - base, H3O+(aq) - conjugate acid b) HCO3-(aq) + H2O(l) <--> H2CO3(aq) + OH-(aq) HCO3-(aq) - base, H2CO3(aq) - conjugate acid H2O(l) acid, OH-(aq) - conjugate base c) HNO3(aq) + SO4-2(aq)----> HSO4-(aq) + NO3-(aq) HNO3(aq) - acid, NO3-(aq) - conjugate base SO4-2(aq) - base, HSO4-(aq) - conjugate acid
2016-12-13 05:41:23 · answer #4 · answered by Anonymous · 0⤊ 0⤋
extremely tough stuff. look from a search engine. that can help!
2014-11-13 15:01:06 · answer #5 · answered by ? 3 · 0⤊ 1⤋