<p>Lets get a nice list down. :D</p>
<p>Or… let’s not.</p>
<p>lol the other thread was deleted by CC for violating terms and conditions.</p>
<p>It was up long enough for a lot of people to post in it.</p>
<p>when will collegeboard post the frq on the website???!</p>
<p>^i second that question</p>
<p>FRQ is up… we are allowed to talk about free response</p>
<p>I know all the answers. My teacher solved every problem and I got a 60. :D. Hoping for a 5. I am talking about the FRQs. lol</p>
<p>What are the answers?</p>
<p>Can someone post a link to the AP Chem FRQ?</p>
<p><a href=“Supporting Students from Day One to Exam Day – AP Central | College Board”>Supporting Students from Day One to Exam Day – AP Central | College Board.
So you want me to tell you all the answers? lol. Ask a specific one.</p>
<p>^lol no thanks. What do you think we’ll need to get a 5?</p>
<p>Don’t the answers go on there too…</p>
<p>Number 1? Im pretty sure I got .01 moles and 122 g per mole but what about the rest</p>
<p>Does anyone have a compiled list of all the answers?</p>
<p>For number 1. .01 moles and 122g/mol is correct. Then the net ionic equation is like
HA + OH- —> A- + H2O . ph was like 2.45. F was tricky. It is a buffer solution, so you had to use the Henderson Hasselbalch equation. 2.85 is wrong, which is what I got when I bluntly used the ice box after considering NaOH as the limiting reagent. The answer is like
4.8ish. Plug in the values and you can see. When you find the molarity, the liters should be .080L.
A five would be around a 100. So if you made a 60 on the frq, you have to get at least a 40 on the MC.</p>
<p>Looks like I’m getting a 4 on that question</p>
<p>What was the evidence that it’s a weak acid</p>
<p>It’s a weak acid because you know it’s being titrated with a strong base so if it were a strong acid the equivalence point would be at 7. However since it is basic at the equivalence point: Weak acid + strong base = basic equivalence. (I hope lol)</p>
<p>I think I said something along those lines.</p>