how to find the pH of " 100 molar H Cl " ???????????????

Answer 1

It's impossible, there wouldn't be enough water for the bonds to be solvated. The HCL bond needs many more water molecules to be in a liquid phase, that is why higher concentrations are impossible.

Answer 2

HCl, being a gas, must dissolve in water to give you a 100 M HCl solution. The most concentrated "solution" in water is water! The molarity of water is:

Molarity = moles solute / 1 L solution

1 L H2O = 1 kg H2O = 1000 g H2O

1000 g H2O / (18.015 g / mol H2O) = 55.5 moles H2O

Therefore, molarity of water = 55.5 moles / L

You cannot have anything more concentrated than that. 100 moles per liter is not theoretically possible.

Now, if we are just trying to figure out the problem in an academic sense, just take the - log of 100 and the pH is -2 (again, an impossible reality).

Answer 3

As mentioned, you just can't get to 100M HCl. Practical maximum is about 38 - 39% HCl by weight. At concentrations above that , you have fuming hydrochloric, with the HCl gas coming off. At that max concentration, Molarity is 12.4 and pH is -1.1.

Yes, you can have negative pH. In the strong acids, the H ionization is so great the logarithm is positive in high concentrations, giving a negative pH.

Answer 4

Am I misunderstanding one of the answers? The log of 100 is 2, but then the negative of that would be -2. You cannot have a pH of -2.

As stated before, there is absolutely no way to have [H+] of 100M
And by the way, molarity is moles solute/ Liters solution (not mL as one answer said).

Answer 5

100 molar HCl means that the concentration of [H+] ions is 100 mol/mL. You simply just take this number and do the -log of it. so the answer is -log[100]. which is 2.

the pH is 2.0

Answer 6

How the heck do you get 100 molar of anything?