2.0 M H2SO4 solution. calculate the pH​

-.30

Explanation:

H2SO4/sulfuric acid/dihydrogen sulfate is a strong acid, meaning that it easily releases an H+. You have to be careful with this problem, however, as H2SO4 is really only a strong acid for one of its hydrogens. In other words, after it becomes HSO4- upon releasing an H+, it is no longer a strong acid and therefore should not be factored into our calculation.

Now, moving onto the calculation, there are two key things we need to carry it out. First is the pH equation. pH = -log [H+]. And second is the concentration of H2SO4, which is equivalent to the concentration of that H+ released: 2.0 M.  Simply plug in your values.

pH = -log [2.0].

pH = -.30

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.