|
Post by shamrockpea on Jun 8, 2016 13:26:04 GMT
|
|
|
Post by Patter on Jun 8, 2016 13:40:50 GMT
Oh dear, my senior chemistry major is at work. Let me see if I can text her.
|
|
|
Post by shamrockpea on Jun 8, 2016 13:42:36 GMT
please!!! i am unable to help and she can really use help!
|
|
|
Post by Patter on Jun 8, 2016 13:44:18 GMT
please!!! i am unable to help and she can really use help! She is looking at it now for you.
|
|
|
Post by Patter on Jun 8, 2016 13:47:32 GMT
Okay, she said this is better to explain in person but she is going to e-mail me an explanation to give you. She is working on it now for you.
|
|
Deleted
Posts: 0
Oct 7, 2024 17:20:49 GMT
|
Post by Deleted on Jun 8, 2016 13:48:59 GMT
I'm not positive what you're asking, but that reaction that is written as the answer for (C) can go either direction - the ions break apart to form the equation on the right, or they are bound together to form the one on the left. They'd combine in ways that balance out the cations and anions - positive binds with negative to neutralize the charge. The pH question in (G) is more complicated - the pH of a solution is a known and then you account for water I believe, and I'm going to suggest for that one reading over the Q&A on the chemistry help boards, since it will involve logs and molarity. If she's right up against the final exam time, I'd skip the second one and focus on the first. Maybe someone else can explain the pH question quickly, I can't seem to do it with out drawing diagrams and using my hands. Also I need more coffee. I hope she does well. ETA I see Patter is going to hook you up with a chemist - yay! - and here's the link I mentioned about pH concentration: chemistry.stackexchange.com/questions/44150/how-to-calculate-the-concentration-h3o-in-a-solution-with-ph-6-99
|
|
|
Post by elaine on Jun 8, 2016 13:55:02 GMT
|
|
|
Post by Patter on Jun 8, 2016 14:26:46 GMT
Oh man, she typed up a long e-mail, and it's lost in cyberspace and she is now in a meeting. She will resend in a bit. I am SO sorry. How many hours until her exam? I will post as soon as she gets it to me again. Man, I hate the internet sometimes.
|
|
|
Post by Mary_K on Jun 8, 2016 14:57:51 GMT
OMG - I know nothing about chemistry but i'm on pins & needles hoping the help comes in time!
Mary K
|
|
|
Post by shamrockpea on Jun 8, 2016 15:04:52 GMT
It is at 2:30 but she has 2 finals before do help will be appreciated!!!
|
|
|
Post by Darcy Collins on Jun 8, 2016 15:39:18 GMT
I can't open your link on my phone. Obviously not today, but after this term is over, I highly recommend you help your daughter figure out the resources available to her at her university. If the actual professor doesn't have office hours, they usually have TAs that do. Understanding how to get the help you need before the day of the final will be a whole lot less stressful. Good luck.
|
|
|
Post by Patter on Jun 8, 2016 15:53:12 GMT
Okay, here you go. I pray it helps her in some way! And sorry if there are typos. She was typing fast and trying to get back to work. 8c: When molecules react, they separate and reform according got cations and anions. In reactants side of the equation you have CaCO3 which disassociates into Ca 2+ and CO32- is the carbonate anion it will never disassociate unto the individual atoms, then you have H2O which readily dissociates into H and OH-. Now, you need to think of how these cations and anions would go together, OH- is stable on its own most of the time, so you do not need to add a cation to it. The most important thing to look at it balancing the charge. Ca2+ is also stable in the equation so we can leave it be, bicarbonate, (HCO3-) readily forms with water. Next, you check to be sure the carges balance on both sides. This problem is mainly knowing what cations and anions are stable and which ones will form more readily than others. 8g: You know from the previous problem that the pH is 11.71; therefore, the definition of pH is the concentration of H+ in the solution. Using this information and the pH equation gives the formula [H+] = 10-ph; therefore, solving this equation gives the concentration of H+ in the solution.
|
|
|
Post by shamrockpea on Jun 8, 2016 18:40:50 GMT
If I could visit just one website for the rest of my life it would be the peas! It is a group of people coming together to help others. I can't thank you all enough! Professor just posted this practice test on Sunday night and she went to school Monday and worked on stuff for all 3 finals all day Monday and Tuesday and went to the tutoring session for chem Monday. She said the tutor was great but their were too many students to help and no one else could help her.
|
|
|
Post by Patter on Jun 8, 2016 19:12:36 GMT
My daughter is a tutor but she also studies with Chemistry students in her classes. They work on the homework and things together. Sometimes 3 or 4 brains is better than your own. Those professors can be toots sometimes. My daughter had one post the practice test the night before, and it was for Organic Chemistry. Ick! I pray she does amazing on her exams.
|
|