The pKa for HCO3- ----> CO3-2 + H+ is 10.33
I assume you would have a reaction such as
K+ HCO3- + H2O ------> K+CO3-2 + H3O+
In which the potassium acts as a neutral ion.
The pKa value for sodium octanesulfonate is typically around 2.0 to 2.5.
The conjugate acid is Hydrogen (H2), the pKa of which is 35.
Sodium hydroxide is a strong base and does not have a pKa value. Instead, it dissociates completely in water to form hydroxide ions (OH-) and sodium ions (Na+).
From this salt the benzoate ion C6H5-COO- is a base ( the other part Na+ is neutral).This base has a pKB value of 9.80 (benzoate)The pKacid value of its conjugated benzoic acid ( C6H5-COOH) however ispKbenzoic-acid = 4.20 = pKa(which is (not surprisingly) equal to 14.0-pKbase = 14.0-9.80)
The effective pH range for a sodium phosphate buffer with a pKa value of 2.15 is typically 1.15 to 3.15. This range is optimal for buffering capacity at pH levels around the pKa value, ensuring stability and effectiveness for biological or chemical processes requiring a specific pH environment. Beyond this range, the buffer may not efficiently maintain the desired pH.
The pKa value of sodium borohydride is approximately 13.
There are two answers: bicarbonate has two pKa's - because bicarbonate can gain a proton to become carbonic acid or lose a proton to become carbonate. Two reactions; two pKa's. The pKa for bicarbonate carbonic acid reaction is 6.4 The pKa for bicarbonate carbonate reaction is 10.3 Both pKa's are temperature sensitive.
The pKa value for sodium octanesulfonate is typically around 2.0 to 2.5.
The pKa value of ceftriaxone is approximately 3.8.
The conjugate acid is Hydrogen (H2), the pKa of which is 35.
Sodium hydrogensulfate contains the HSO4- ion therfore it can function as an acid. It's pKa value is 1.9.
Sodium hydroxide is a strong base and does not have a pKa value. Instead, it dissociates completely in water to form hydroxide ions (OH-) and sodium ions (Na+).
The pKa value for sodium bicarbonate (NaHCO3) is 10.3. This provides a measure of the acid strength of bicarbonate. People often make the mistake of reporting the pKa value of 6.3 for bicarbonate. However, that is the pKa value of carbonic acid (not bicarbonate). It relates to the ease of the first deprotonation of carbonic acid to form bicarbonate. The pKa of bicarbonate relates to the deportation of bicarbonate to form carbonate. This distinction is important, since carbonic acid has two pKa's, the higher of which represents that second deprotonation.
The pKa value of Doxofylline is approximately 4.22.
In order of increasing pH: (calculated 'pH about'-values are given for 1.0 M solutions)sodium bisulfate Na+(HSO4)- is weak acidic, pKa= 1.92, (pH about 1.0)acetic acid H(OOCCH3) is weakly acidic, pKa= 4.77, (pH about 2.4)neutral: water pKa= 14, pKb= 14 so pH= 7.0sodium acetate Na+(OOCCH3)- is weakly basic, pKb= 9.23, (pH about 9.4)sodium carbonate (Na+)2(CO3)2- is weakly basic, pKb=3.75, (pH about 12.1)
From this salt the benzoate ion C6H5-COO- is a base ( the other part Na+ is neutral).This base has a pKB value of 9.80 (benzoate)The pKacid value of its conjugated benzoic acid ( C6H5-COOH) however ispKbenzoic-acid = 4.20 = pKa(which is (not surprisingly) equal to 14.0-pKbase = 14.0-9.80)
sodium hydroxide