H2CO3 «  H+ + HCO3-   Now visualize a small amount of acid added to the solution. Describe what will happen?
98553
it will start to bubble and produce heat.
804535
Neutralization Reaction:\nHC2H3O2(aq) + KOH(aq) -->H2O(l) + KC2H3O2(aq)\nThe equation is already balanced.\n\na. False KC2H3O2(aq) and H2O are products.\nb. True\nc. False, some ions will cancel out but some will remain.\n\nThe ionic equation is as follows:\n(H^+)(aq) + (C2H3O2^-)(aq) + (K^+)(aq) + (OH^-)(aq) -->H2O(l) + (K^+)(aq) + (C2H3O2^-)(aq)\nRepeated ions are crossed off from both sides and the net ionic equation is:\n(H^+)(aq) + (OH^-)(aq) -->H2O(l)\n\nd. True\ne. False\n\nNote: the + and - signs were written with ^ to indicate that they were raised up (like a power).  Sorry if this notation is confusing.  Good luck and I hope that this helps!
826050
Depends on the acid.  Fuming sulfuric acid, for example, actually forms such a strong hydration with water that it will yank out oxygen and hydrogen from your hydrocarbon based tissue, leaving carbon, which looks like a 3rd degree burn.
163386
The time necessary to diffuse H+ ions in the base. Thats it, when u add the necessary amount of acid at once.\n\nUsually when neutralization is carried out the conical flask (or whatever where the base is kept) is kept shaking to increase individual molecular motion. The more motion, the greater chance of H+ ion meeting OH- ion and neutralize each other in a given time interval\n\nH+(aq) + OH-(aq) --> H2O(l)
839133
H2CO2 is better written as HCO(OH).\n\nThe dissociation equation is:\n\nHCO(OH) ---> HCOO(-) + H(+)\n\nYou can see from the reaction that it can give only one proton (The other H, bound to the C is not acidic).\n\nSo monoacid.
205870
CaCO3(s) + 2HC2H3O2(aq)-> Ca(C2H3O2)2(aq) + H2O(l) + CO2(g)
757438
CaC2 + 2 H2O ---> Ca(OH)2 + HCCH
684663
Maybe I'm wrong but I don't see a solution.  Not enough oxygen to complete that reaction.  Dod you have a typo somewhere?\nIf water is on the left then:\n  CH3COOH + 2 H2O + 8 NaCO3  =  8 NaHCO3 + 2 CO2
802465
carboxylic acid, as represented by -(C=O)-OH. For more info, check the source.
924773
(1) NaHCO3    --->  Na(+) + HCO3-\n(2) Ca(NO3)2  ---> Ca2(+) + 2NO3-\n(3) Al2(CO3)3  ---> 2Al(3+) + 3CO3(2-)\n\nThis is all taking place in water (ideally), so you should consider that too.
901715
h3o+ is for hydronium ion, an acid.
608403
NaOH (aq) + HCl (aq) --> NaCl (aq) + H2O (l)
739795
Bicarbonate Ion.  HCO3-  Will combine with H+ (acid) to form H2CO3 or carbonic acid which has less effecto on pH.  Hemoglobin in RBC's is also an example of a protien buffer.  A buffer is anything that will receive or donate a hydrogen to swing the pH either way.
1044128
increase in acidity....\n\nread your textbook, PLZ
551370
Well, the equation is..\nCH3COOH + NaHCO3 ----> CH3COONa (Sodium Acetate) + H2CO3 (Carbonic Acid) \n(or)\nCH3COOH + NaHCO3 ----> CH3COONa (Sodium Acetate) + H2O (Water) + CO2 (Carbon-dioxide)\n\nSo you might have noticed the equation is already balanced. It is a double-displacement reaction. So the sides are already balanced.\nHope this helps.\n\nOne small note...I don't think there is a compound such as NaCO3. The valency of CO3(^-2) ion is 2, so it has to combine with two Sodiums (two positive charges to neutralise its two negative charges) unless the compound one of the above users mentioned is NaCO3-.\n\nrule wid style n luv@vinny
624341
A solution that contains an equivalent amount of an acid and its conjugate base.
877634
Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+