H2CO3 is stronger, meaning that the 1st H+ is easier to remove.
HCO3- is weaker because the 2nd H+ must be removed from a negative ion (which attracts the H+).
When HCO3- acts as a Bronsted base, it accepts a proton (H+) to form H2CO3 (carbonic acid).
The conjugate base of H2CO3 is HCO3-. When H2CO3 donates a proton, it forms the bicarbonate ion (HCO3-), resulting in the conjugate base of the acid.
You mean,HCO3 - = bicarbonateH2CO3 = carbonic acid and the conjugate of the above base.
H2CO3 is atype of ionization which depend on two steps as following :H2CO3 H+ + HCO3- HCO3- H+ + CO3-2
In blood at pH 7.4, there is more bicarbonate (HCO3-) because the pKa of carbonic acid (H2CO3) is lower than the blood pH, favoring the dissociation of H2CO3 into HCO3-. The bicarbonate acts as a buffer to help maintain blood pH within a normal range.
When HCO3- acts as a Bronsted base, it accepts a proton (H+) to form H2CO3 (carbonic acid).
The conjugate base of H2CO3 is HCO3-. When H2CO3 donates a proton, it forms the bicarbonate ion (HCO3-), resulting in the conjugate base of the acid.
You mean,HCO3 - = bicarbonateH2CO3 = carbonic acid and the conjugate of the above base.
H2CO3 is atype of ionization which depend on two steps as following :H2CO3 H+ + HCO3- HCO3- H+ + CO3-2
In blood at pH 7.4, there is more bicarbonate (HCO3-) because the pKa of carbonic acid (H2CO3) is lower than the blood pH, favoring the dissociation of H2CO3 into HCO3-. The bicarbonate acts as a buffer to help maintain blood pH within a normal range.
Ka= [h+][HCO3-]/[H2CO3]
The conjugated acid of HCO3- is: H2CO3, carbonic acid.Conjugated pairs of acid and base always differ ONE (1) proton (H+): The acid WITH and the base WITHOUT it.So, on the other hand the conjugated base of HCO3- is: CO32-, carbonate.
I think you mean H+ + HCO3- --> H2CO3
NaHCO3 ---> Na+(aq) + HCO3-(aq) CH3COOH <--> H+(aq) + CH3COO-(aq) H+ + HCO3- ---> H2CO3 H2CO3 ---> H2O + CO2
The conjugate base of HCO3- (bicarbonate ion) is CO32- (carbonate ion) The conjugate acid of HCO3- (bicarbonate ion) is H2CO3 (carbonic acid)
H2CO3 is Carbonic Acid or HCO3- is Bicarbonate
HCO3 acts as a Brønsted-Lowry base in the bicarbonate buffer system, which consists of the equilibrium between carbonic acid (H2CO3) and bicarbonate ion (HCO3-) in aqueous solution. In this system, HCO3- accepts a proton (H+) to form carbonic acid (H2CO3).