最早,劳伦斯·约瑟夫·亨德森在研究碳酸的缓冲能力时提出亨德森方程,后来,卡尔·阿尔伯特·哈塞尔巴尔赫将亨德森方程写为对数形式,并用于研究血液中碳酸引起的代谢性酸中毒(拓展阅读:Henderson-Hasselbalch equation and the pH of buffer solution)。
The reason the Henderson-Hasselbalch equation is an approximation is because it takes water chemistry out of the equation. This works when water is the solvent and is present in a very large proportion to the [H+] and acid-conjugate base. You shouldn't try to apply the approximation for co...
Easy Derivation of pH Is Approximately Equal To (pKa1 + pKa2) / 2 Using Autoprotolysis of HA-: Doubtful Value of the Supposedly More Rigorous Equation Easy Derivation of pH Is Approximately Equal To (pKa1 + pKa2) / 2 Using Autoprotolysis of HA-: Doubtful Value of the Supposedly More...
首先 例题里的酸 都是一元弱酸 当弱酸与其共轭碱共存时，电离平衡受同离子效应的影响 溶液中[H3O+]的浓度由弱酸与其共轭碱的浓度比决定 这里没有牵涉到平衡移动的问题 因为这个是标准的缓冲溶液 里面没有加入其他任何的酸或者碱 来调节PH 故不存在平衡移动的问题 况且弱酸的电离都很小 自身的电离...
[HA]eq=c(1−α);[A−]=cα; Hence:log[A−]eq[HA]eq=pH−pKa The above equation is extremely practical as pH is easily measured and pKavalues are predefined. View chapter Explore book
pH and pKa are related through the Henderson-Hasselbalch equation, pH = pKa + log(base/acid). If there is more of the basic form, the pH will be higher than the pKa, and the opposite for more acidic forms. What does pKa of a functional group mean? Each functional group's pKa can ...
Aqueous buffer solutions with pHs ranging from 3.83 to 10.85 were mixed. Four methods—two graphical and two mathematical— were used to estimate the acid dissociation constant (pKa) and isosbestic point using absorbance measurements. The equation for the dependence of the absorbance on pH at λ ...
the henderson-hasselbalch equation is used to calculate the relationship between pka and ph ph is equal to the sum of the pka value and the log of the conjugate base concentration divided by the weak acid concentration. q2 what happens if the ph falls below pka? the group is in the ...
pH = 14 – pOH = 9.3 I used notes and the internet for the equations, which seemed to work fine until I googled the pH of the acids and it makes my answers completely wrong. I originally thought the pH could be worked out by doing the -log of Ka, but then M concentration was in...
The equation may be rewritten as: Ka/[H+] = [A-]/[AH] This shows that pKa and pH are equal when half of the acid has dissociated. The buffering capacity of a species or its ability to maintain pH of a solution is highest when the pKa and pH values are close. So, when selecting...