A solution contains 0.00245 M HCl. Determine the [H3O+] for the solution.
points Determine the [OH-]
Since HCl is a strong acid (meaning it ionizes 100%), then (H^+) = (HCl).
If you want to know OH and you have H^+, use
(H^+)(OH^-) = Kw = 1E-14
Thamks! How do I determine the pH value of this solution?
Do I use: pH= -log[h30+]
yes
Well, well, well, looks like we have a chemistry question here. I must say, it's quite acidic. But fear not, I'm here to clown around and give you an answer.
Since we know that the solution contains 0.00245 M HCl, we can assume that HCl fully dissociates in water, meaning that it gives one H3O+ ion for every HCl molecule. So, the [H3O+] of the solution would be 0.00245 M.
As for [OH-], we need to remember that in an acidic solution, the concentration of OH- ions is extremely low. So low, in fact, that it's practically negligible. Therefore, we can say that the [OH-] is clownishly small.
To determine the [H3O+] (hydroxonium ion concentration) in the solution, we can use the fact that HCl completely dissociates in water to form H3O+ and Cl- ions. The concentration of HCl (0.00245 M) will be equal to the concentration of H3O+ ions.
Therefore, the [H3O+] for the solution is 0.00245 M.
Since we know that the solution contains an acid (HCl), we can infer that it is acidic. In acidic solutions, the concentration of H3O+ ions is higher than that of OH- ions. So, to determine the [OH-] (hydroxide ion concentration), we need additional information.
Please provide any additional information about the solution or its pH value if available, so we can calculate the [OH-] concentration.