2014年9月13日 · Since the pull of all the water molecules surrounds the Cl- ions, equilibrium tends to the right. The HCl covalent bond is also quite weak so it is much easier to pull the HCl apart than it is to reform it. This is why almost 100% of HCl is ionized. Note that all the compounds in your equation have octets.

2017年2月26日 · No. $\ce{HCl}$ is a gas at STP (standard pressure and atmosphere). As such, you can store it in pressurized cylinders, but commonly it is stored as a concentrated aqueous solution $\ce{HCl(aq)}$. In the gas phase, $\ce{HCl}$ is composed of covalently bonded molecules, H bonded to Cl.

2016年4月19日 · In case you are unfamiliar, the $\mathrm{p}K_\mathrm{a}$ is a way of expressing how much an acid dissociates in water, and a drop in $\mathrm{p}K_\mathrm{a}$ by $1$ means an acid releases $10$ times as many $\ce{H+}$ ions. $\ce{HCl}$ releases $10^{11.75}$ times as many $\ce{H+}$ ions as $\ce{CH3COOH}$, but when acetic acid's $\ce{C-H}$ …

2016年6月28日 · The electron that you think of as originally being on the hydrogen in HCl is left behind on the Cl atom, making the hydrogen atom become the H+ ion and the chlorine atom become the Cl- ion. Look at the image on this Wikipedia article about acid dissocation for a helpful graphic using acetic acid as an example. $\endgroup$

2018年5月1日 · I think that the initial step forms a tertiary amine, which then in the presence of the ketone and trace acid undergoes nucleophilic addition. But then, for the $\\ce{HCl/H2O}$ in the last step, whi...

2015年5月17日 · Seeing that both oxygen and chlorine have a small difference in their electronegativity (oxygen being roughly 3.5 and chlorine being roughly 3.0), why does chlorine in a hydrogen chloride molecule ($\ce{HCl}$) have a dipole-dipole interaction, while the oxygen in a water molecule ($\ce{H2O}$) causes the water molecule to have a stronger form of ...

2008年11月16日 · The problem says: Enthalpy is always reported with respect to a reactant. Calculate the enthalpy change, DeltaH, for each reaction in terms of kJ/mol for one of the reactants. (i.e either HCL or NaOH). I had three reactions: 1. NaOH + HCL---->H20 +NaCl 2.NH4Cl +NaOH---->H20 +NH3 +NaCl 3...

2013年6月23日 · I want to know why HCl is a much stronger acid than H2O.They have similar bond energies (H-Cl = 427 kJ/mol, O-H = 467 kJ/mol), so there should be easy to ionize both. Besides, O is more electronegative than Cl, so it should "steal" the electron easier. Why is HCl Ka so superior than water Kw?

2019年1月5日 · Consider simply aqueous solutions of $\ce{H2S}$ and $\ce{HCl}$. It is pretty much known that $\ce{HCl}$ is stronger than $\ce{H2S}$ in water. The reason behind that first is the electronegativity of $\ce{Cl}$ is higher than $\ce{S}$, so, in a polar medium, it becomes easier for the $\ce{H-Cl}$ bond to break than the other one.

2016年7月15日 · I know as a fact that HCl is a stronger acid than H3O+, but I want to know the reason behind it. The definition of an acid is a substance which dissociates to give H3O+ ions. In that case H3O+ should be the strongest acid available because it does not even need to dissociate it give itself!!