@rolnor, your tough love was effective despite my lack of appreciation. My use of "lowblow" and "no cookie" was meant to express my distaste somewhat in jest too. I am embarrassed as well for my laziness, naivety, and manner of handling your response. My motivation remains.
@Borek, thank you for the additional education. I was lazy in my notation and, similar to students looking for shortcuts, I admit that I am in the forums looking to be spoon fed as well.
I want to express my heartfelt gratitude that everyone even took the time to read and reply. The consequent rabbit holes I have traveled are going to take some time to organize and think more critically about before I am ready return with a well researched inquiry that is considerate to everyone's time here.
I think that we can conclude this thread with the following as a solution:
from @rolnor - the answer to my question is no
from @billnotgates - https://www.britannica.com/science/chemical-reaction/The-Bronsted-Lowry-theory
shows that the reaction is dynamic (
), albeit a product favored reaction, and that the Cl-
in the product is the weak base and aqueous. That H2
O is the base reactant in the Bronsted-Lowry reaction and that HCl is the strong acid reactant.
from @Borek - charges matter, and that https://en.m.wikipedia.org/wiki/Acid
indicates that what makes HCl qualify as an arrhenius bronsted-lowry acid is that it readily donates a proton in the form of H+(aka protonation, protolysis). Since H2
O is present, the H+
donated by the HCl, bonds with the H20 to form H3
)+ and leaves Cl-
in aqueous form, or as a solvent in the solution. Since HCl is a "strong acid" it readily dissociates in water. Since there is a 1:1 relationship between protonation of the HCl and H2
O, HCl also falls into the category of monoprotic acid.
A link within the wiki recommendation from @Borek (https://en.m.wikipedia.org/wiki/Hydrochloric_acid
) immediately reveals that H3
(hydronium) in fact constitutes the HCl with Cl-
and they will likely form other hydrogen bonds with neighboring H2
O molecules in a variety of ways. In the presence of enough H20 however, it is likely to entirely dissociate into H3O+ and Cl-. The wiki page also indicates that the mass fraction of the HCl effects physical properties such as boiling point. For example it indicates that the mixture will act as an azeotrope if the mass fraction 20.2% and this means that at the corresponding boiling point that the vapor will be maintain the same proportions that existed in the mixture. This point is somewhat related to my asking if I can just boil off the Cl- since the product of the Bronsted-Lowry reaction is favored and Cl- boiling point is significantly lower than H2O, but perhaps not so low that H30+ would not be denatured in the process. However, I consider the boiling point of H3O+ to likely be similar to H2O and well above that of Cl- since the bonds of the hydrogen and H+
are covalent with the O (not positive this point though). Certainly need to keep top of mind eutectic and azeotropic properties based on mass fraction it appears. It does not look like hydrogen bonds between H3O+
require much attention.
Other research makes it look like the most efficient way to remove Cl- ions is with Silver Nitrate to form precipitates and then filter. I would like to avoid introduction of more elements as it feels like steps away from the final product rather than towards. such is the game i guess.
ultimately the reaction i am trying to perform here I have attached an image of. My initial question was because I was trying to figure out how to make sure my reactants are combined in the presence of H+
additional answers I will need to discover is how to get rid of the diethyl ether in one of my reactants and where the heck the MgBr went.
Thanks again everyone.