what is the [h3o+] in a 9.93 x 10^-6 M Ba(OH)2 solution?
(this is all that's given)
I understand the basics of the question. however does [OH]= 9.93x10^-6 squared?
No, but you're on the right track. Ba(OH)2 = 9.93E-6 from the problem. Since there are two OH ions in 1 Ba(OH)2, then OH = 2*9.93E-6. Then (H3O^+)(OH^-) = 1 x 10^-14
To determine the [H3O+] in a solution of Ba(OH)2, we need to consider the ionization of water and the dissociation of Ba(OH)2.
Ba(OH)2 is a strong base, meaning it dissociates completely in water. The balanced chemical equation for the dissociation of Ba(OH)2 is:
Ba(OH)2 -> Ba2+ + 2OH-
In this case, the concentration of Ba(OH)2 is given as 9.93 x 10^-6 M.
Since Ba(OH)2 dissociates into two OH- ions, the concentration of OH- ions in the solution will be twice the concentration of Ba(OH)2. Thus, the concentration of OH- ions is calculated as:
[OH-] = 2 × (9.93 x 10^-6 M) = 1.986 x 10^-5 M
Water also has a tendency to ionize into H+ and OH- ions. However, in pure water, the concentration of H+ ions from self-ionization is usually very low, around 1.0 x 10^-7 M.
H2O -> H+ + OH-
Since Ba(OH)2 is a strong base, it will react with water to consume OH- ions and produce more H+ ions. For every two OH- ions consumed, two H+ ions are produced. This means the increase in the concentration of H+ ions will also be twice the decrease in OH- ions concentration.
Therefore, the [H3O+] concentration is:
[H3O+] = 2 × (1.0 x 10^-7 M - 1.986 x 10^-5 M)
= 2 × (-1.976 x 10^-5 M)
= -3.95 x 10^-5 M
Thus, the [H3O+] in a 9.93 x 10^-6 M Ba(OH)2 solution is approximately -3.95 x 10^-5 M.