2019年1月25日 · This practice is valid for Cl- ions (pKb ≈ 20) because it is a much weaker base than water is. But is this practice valid for the Na+ ion, which has a pKa = 13.9? If we were to take the pKa of water to be 15.7, the Na+ ion would be over …

2014年4月9日 · $\begingroup$ So it sounds like the origin of the -1.76 value arises from a simplified definition of pKa often used in introductory courses. In any case, what implications does this have, if the pKa is really 1.0 instead of -1.76? Does the pKa of protonated methanol differ significantly? $\endgroup$ –

2015年12月21日 · Methanol is more acidic than water because its conjugate base that is methoxide is weaket than waters conjugate base that is hydroxide and now we can say that weaker is the conjugate base more is its acidic character . or we can say that due to the presence of methyl group in CH3 bond between O and H become weak and it can easily release ...

2018年1月19日 · $\begingroup$ I can't post an answer with definite reasoning, because I don't know the Pka values, and so, I can't examine the trends in them. I think the OP's reasoning behind the acidity order is right, so the only confusion is in the Pka values. I can't comment due to lack of reputation, otherwise I would've done that $\endgroup$ –

2015年11月26日 · As for why the $\ce{D2O}$ is less dissociated than $\ce{H2O}$, The ionization constant of heavy water ($\ce{D2O}$) in the temperature range 298 to 523 K Canadian Journal of Chemistry, 1976, 54(22): 3553-3558 breaks the differences down in to enthalpy and entropy components, which both favor ionization of $\ce{H2O}$ and states that $\ce{D2O}$ is ...

HOCl is a weak acid (pKa=7.5) that can be protonated on oxygen by HCl to give H2OCl+ (+ charge on oxygen) and Cl-. Have Cl- displace H2O from H2OCl+ to afford Cl2 (think SN2 rxn.) $\endgroup$ – user55119

Including water on both side of the equation is a bit of a mistake here. For hydronium: $$\ce{K_a = \frac{[H^+][H_2O]}{[H_3O^+]}}$$

2023年1月14日 · Consider the reaction between ammonia and acetic acid: if ammonia acts as a base, then the reaction is shifted to the right, since NH4+ is a weaker acid than CH3COOH [pKa(NH4+)= 9.8; pKa(CH3COOH)=4]. Conversely, if acetic acid were to act as a base, the equilibrium would be enormously shifted to the left, this because NH3 is an extremely weaker ...

What is the pKa Range for weak acids and bases? Bases don't have a $\mathrm{p}K_\mathrm{a}$. To discuss the strength of a base, you can look at the $\mathrm{p}K_\mathrm{a}$ of the conjugate acid, though. Am I correct in assuming that the following is true? $\mathrm pK_\mathrm a < 3$ is for a …

2015年4月17日 · Now if we evaporate solvent we will get glycine hydrochloride salt, which has a pKa is 2.3 for first deprotonation and a pKa of 9.6 for the second deprotonation. Chloroacetic acid's pKa is 2.87, which means that glycine hydrochloride is more acidic.