The Unit exam

This exam felt a lot like the quiz before. My only real problem with the test was that it took place after we had a whole week to forget about it cause of labs. Moving on. This test was centered around all the previous notes we have done before. the only confusing part of the test for me was finding the ka with the ph and molarity of the solution. To study for this test i went over the big packet with mostly the ph square thingy, and the tests on schoology. Even thought the answer to study guide relationship was a little bit off. this helped with the ice box and titration problems the most. Overall for being the hardest test of the year it didn't feel like it. Which means i probably got a 50%

The unknown acid lab

So lets say you have an unknown acid (solid) and you want to know how to find it. First off you throw away all the data from the previous day and start fresh. This limits your time so you work harder. Next you take a base and acid combo that you already know and use this to find the molarity of the base because that information was somehow forgotten in the making of the base. then take the base you just used and titrate it with the unknown acid. this allows you to find the molar mass of the unknown acid and find out what it is. This is all just hypothetical..... I swear....

Acid and vinegar lab

The process is complete for the acid and vinegar lab. To start out we had to titrate the acid KHP (which is not just K, H, and P). To do this we had to set up the lab by clearing out the burett and filing it with NaOH (base). Taking .5ish grams of KHP and dissolving it in a about 75 ml of water with a couple drops of phenolphaline. Taking the KHP in a flask and put it under the burett to get titrated (make the phenolphaline turn the liquid light pink). Then you take the flask and fill ti with 10 ml of vinegar and then titrate it with the leftover base in the burett. After doing all of this we can find a large amount of different numbers and items. Such as the molarity of the base or the atomic mass of vinegar.

That last test though

So the test was not was what i was expecting it to be. The last part of it with the ice box problems was not my favorite. just in case anyone else had this problem here is the method to do them. Take the Equation X squared over the molarity minus X and set that equal to ka (unless it is less than kw). multiply the equation out to equal zero. Then Find the zeros of the equation on a graph or use the quadratic equation. Finally take this final number and use it as the [H+] to find ph.

Recent notes

Arrhenius reminds me of diarrhea. Just saying. So the first thing we went over this week was the difference between Arrhenius and Bronstead-lowry acids and bases. Arrhenius acids/bases are all the ones we have been using so far. Bronstead-lowry ones have generally not been used by us and have much more specific uses in a Bronstead-lowry equation. The general definition of the acids is that they donate an electron and the bases receive an electron. Our class also learned how to do ice box equations. Which generically evolve into X squared divided by the molarity minus X set equal to Ka. These equations are used to find the ph of weak acids. The last thing we went over is the H+ to OH- to pH to pOH square. this square tells how you can get any htree things from the square when you only start with one.

Vitamin C lab

So first off i have to apologize to all the groups because of the fact that Gannon ruined everything. He was only supposed to use one tablet of vitamin c concentration but he used two. Besides that the lab seemed to go off without a hitch. We started the lab by getting samples of 5 different liquids with varying vitamin C concentration. Putting 20 drops of each liquid in a test tube with starch readied them for testing. The testing was conducted by dropping iodine concentration into the test tubes and counting the amount of drops it took to turn fully blue. Then doing some plug and chug equations we were able to find the vitamin c concentration.