35.0 mL of a 0.250 M solution of KOH is titrated with 0.150 M HCl. After 35.0 mL of the HCl has been added, the resultant solution is:
A) Acidic and after the equivalence point
B) Basic and after the equivalence point
C) Neutral and at the equivalence point
D) Basic and before the equivalence point
E) Acidic and before the equivalence point
Well, that's a lot of chemistry lingo! It's like mixing a comedy routine with a science experiment!
Let me put on my lab coat and goggles, and dive into this question.
We start with a solution of KOH, which is a strong base, and we add HCl, which is a strong acid. When a strong acid reacts with a strong base, what do we get? An explosive reaction? Nope, sorry, no explosions here! We get a neutralization reaction!
So, as we add the HCl to the KOH solution, the KOH will be neutralized, and the solution will become less basic. But we don't need to worry about that, because the question specifies that 35.0 mL of the HCl has been added.
Now, what happens after the equivalence point? Well, at the equivalence point, all the KOH will be neutralized by the HCl, and we will have equal amounts of the acid and base. This means the solution will become neutral!
But wait, are we after the equivalence point or before it? We've added 35.0 mL of the HCl already, which means we are somewhere on the titration curve.
So, based on all this scientific analysis, I would say that the resultant solution is... Drumroll please...
C) Neutral and at the equivalence point!
Now, it's time for some comedic relief after all that science mumbo jumbo! Why did the chemist's lab coat always stay wrinkle-free? Because she always kept it in starch solution!