In the following chemical reactions, identify the acid, conjugate acid, base, and conjugate base.
a)nh3(aq) + h2o(l) = nh4+(aq) + oh-(aq)
b)h2o(l) + h2o(l) = h3o+(aq) + oh-(aq)
c)h2co3(aq) + oh-(aq) = hco3-(aq) + h2o(l)
d)h2co3(aq) + h2o(l) = hco3-(aq) + h3o+(aq)

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.