All right, so remember there's an inverse relationship. So that means a weak acid will have a relatively strong conjugate base. And in fact, the weaker the acid, the stronger the conjugate base. A stronger conjugate base has a high affinity for protons, so it has it wants some more readily accepted H.
Here we have HCM, which is a weak acid hydrocyanic acid. It reacts with water. Water accepts an H+ and becomes H3O+. As a result, HCM gave away an H+ analog C and minus. Here it's a weak acid, so that means it's going to be a stronger conjugate base. It's still weak, but it's stronger because it came from someplace else that's weak.
Now notice also that we have reversible arrows here. The arrow that points to the reactant is longer. That means reactants are more highly favored. This makes sense because remember, weak acids and weak bases don't completely ionize. We don't make 100% of these ions. A vast majority of it is still in the reactant form, which is why the arrows pointing towards the reactant, that side is more favored. There's more of it.
So we're going to say here, stronger the base, the weaker the conjugate acid. We conjugate acids less readily donate protons. The weaker the base then the stronger the conjugate acid. Stronger acids more readily donate protons or more easily donate protons to. Just remember this inverse relationship. If you're strong in one particular way, you're weaker in the opposite way. A strong acid would equate to a weaker conjugate base.