1. Ohio State Chemistry 1210 Lab Manual
2. Ohio State Chemistry 1210 Lab Manual Answers
3. Ohio State Chemistry 1210 Lab Manual Answer Key

Click to expand. Some students dream of receiving the email students in Robert Zellmer’s Chemistry 1250 class received roughly 25 minutes before their Fall Semester final that said the exam had been postponed.

Unfortunately for them, the email was a hoax. Zellmer, senior lecturer of chemistry and biochemistry at Ohio State, taught two sections of Chemistry 1250 during Fall Semester. Zellmer said for the final, he had students taking it in three different rooms at different times. Zellmer was getting ready to give one of the chemistry finals, which was set to start at 8 p.m.

Chemistry 1210, General Chemistry Laboratory Manual, Ohio State University Spiral-bound – 2014. Be the first to review this item. See all formats and editions Hide other formats and editions. Price New from Used from Spiral-bound 'Please retry'.

At about 7:35 p.m., students in Zellmer’s class received an email, allegedly from Zellmer, stating the Chemistry 1250 final would be postponed to the following day because of poor weather conditions. The email was brought to Zellmer’s attention, and once he saw it, he said he knew it was fraudulent.

He sent out follow-up messages to all of the students who had not yet taken the final when he saw it, about 11 minutes after the fraudulent email was sent, telling them the previous correspondence was not from him. Some students in the other classrooms who had seen the email, though, had left their respective exams. “I sent out two more emails, telling the students we would wait until 8:15 p.m. To start the final, since we were the last scheduled exam, and (then I sent) another telling them to come back to the exam,” Zellmer said in an email.

1. Lecture: MWF 8:00-8:55 am – 1000 McPherson Lab (MP) (5 credit hours). Online Homework: Sapling Learning – see Carmen for registration instructions.
2. CHEM 1210: General Chemistry I August 19, 2015 Prereq: One unit of high school chemistry, and Math Placement Level L or M; or a grade of C- or above in Math 1130.

He said he was able to get all of the students who had left the room after seeing the fake email to come back to take the final. Blake Gehret, a second-year in mechanical engineering, said he was in a different room than Zellmer where the final was about to be given when a student received the fake email and told the class that the final was postponed. “Initially after reading it, I started walking home,” Gehret said.

On the walk home, Gehret called his friend, who was also in the class. His friend told him Zellmer said the email was a fake and the exam was still set for that night.

“I then headed back to my exam. When I got back to the building, I noticed a lot of people had left and Zellmer was shouting that the exam was still on,” Gehret said. Jake Cordonnier, a second-year in mechanical engineering, was also in a different room than Zellmer where the final was set to be given when he received the fake email. Cordonnier said he got really excited when he first saw the email, thinking he would not have to take the final that night. Cordonnier said he happened to be standing by a teaching assistant who also saw the email. “If I wouldn’t have been standing by a teaching assistant when I saw it, I would have walked home and never checked my email again to see Dr.

Zellmer’s other emails that stated the final was still on,” Cordonnier said. To accommodate those students who arrived late, Zellmer said he stayed past the assigned finish time to allow them as much time to take the final as the other students. Zellmer said he still does not know who sent the email or why. “I feel it was a juvenile prank, which caused a lot of commotion and could have caused a lot of problems, including perhaps causing someone to have an accident, because they were sent home and then had to come back,” Zellmer said. Zellmer said the problem was sent to someone another staff member knows after the incident and was told it would be forwarded to the Office of the Chief Information Officer. So far, Zellmer has yet to hear anything regarding whether OCIO was able to identify who sent out the fraudulent email. According to OCIO, there is no record of the issue being reported.

If a student sent the email, OSU’s Code of Student Conduct states that any student found to have engaged in dishonest conduct, including “misuse or falsification of university or related documents by actions such as forgery, alteration or improper transfer,” is subject to disciplinary action by the university. Zellmer said he has already taken steps to attempt to ensure a similar incident won’t happen. “I told the students this semester I would never send an email canceling an exam, lab, recitation or lecture,” Zellmer said. “The only way anything will be canceled is if OSU does so and it’s officially posted on the OSU web page.” 2014-02-16.

“According to OCIO, there is no record of the issue being reported.” Of course there isn’t. OCIO and OSU Police remove reports all the time in order to make the campus seem safer and give the appearance that our administration has some semblance of control How else would the school be able to rope in more students? Want to test it? Try making a report with either agency. If it involves gross negligence, gross student misconduct, or assault, it will magically disappear – especially if an athlete is found to be involved.

When I was assaulted last year on Ohio State’s campus, I made a report with OSU Police. Myford gearbox manual. They never showed up, but Columbus PD did at the dental school. Columbus PD then called to update OSU PD on the case. Two days later, OSU had “no record” of the assault ever happening, even though it occurred on campus during business hours and Columbus PD had record of contacting OSU multiple times.

Two students in an upper-division humanities course (which one of my colleagues teaches) were subjected to a disciplinary committee hearing after they were found to have plagiarized all assignments over a 16-week period. There is no record of this, and the instructor was told to “Grade the items as they are” because “these are two athletes on scholarship, and being dismissed would ruin their lives.” OSU is just plain underhanded in their enforecement (or lack thereof) of codes of conduct and campus safety.

CHEMISTRY 1210 - LAB: CORRECTIONS, SUGGESTIONS, PRELAB AND REPORT QUESTIONS CHEM 1210 - Sp16 LAB: CORRECTIONS, SUGGESTIONS, PRELAB & REPORT QUESTIONS Last Modified: This material is copyrighted. Any use or reproduction is not allowed except with the expressed written permission of Dr. If you are taking Chem 1210 you are allowed to print one copy for your own use during the semester you are taking Chem 1210 with Dr. You are not allowed to disseminate this material to anyone else during the semester or in the future. Always do INDIVIDUAL WORK (i.e. Work ALONE) both in the lab and on your reports. The only time you can work together in the lab is if your TA gives you permission.

You can discuss the lab with each other before and after lab but when it comes time to answer any questions it must be your own work. ALWAYS WEAR SAFETY GLASSES - failure to do so will result in:. First offense - loss of 1/10 points (10%) for that day's exp. Second offense - loss of additional 1/10 points (10%) for that day's exp. Third offense - loss of all points (100% pts.) for that day's exp. Continued violations may result in dismissal from the course. Wearing contact lenses is NOT recommended.

Reports are due BEFORE lab ONE week after the work is completed. Reports are submitted on-line in Carmen (directions are there). It is YOUR responsibility to make sure the report is submitted properly.

A Word file (docx) or PDF must be submitted. Any report submitted after the due date (even if on the same day) will be penalized 10% per day. NO credit will be given after 1 week (7 days) or past the due dates shown in the syllabus. If you must submit a late report you must notify your TA by e-mail within 1 day after submission. Lab reports should be graded by your lab instructor and returned one week after submission. Changes or corrections generally will be minimal and announced before the lab. Make sure your lab manual is the 2017-2018 printing.

I have most of these changes listed below for each experiment. Some may have already been fixed in this latest edition of the manual. 1 (Measurement and Use of Laboratory Glassware):. Report Questions: 1-3 on p. Answer these questions and include in the report. Corrections, changes or hints to the lab manual:.

Review the following parts of the Lab Manual before lab. Use of the Balance: Appendix E. Use of the Pipet and Buret: Appendix D. Use a buret reading card when trying to read volumes on a buret or even a graduated cylinder. Record ALL values to the correct number of sig.fig. And use UNITS. Record ALL data in the NOTEBOOK not the lab manual or another sheet of paper.

You will have points deducted if you record data in the manual or somewhere other than the notebook, even if you transfer it to the notebook later. Copy tables 1.1-1.4 from the manual (pages 12-13) into your notebook for recording your measurements and calculated values. In the Data Analysis for the report you can put both figures (1.1 and 1.2) on page 14 of the manual on a single piece of paper in the report. Normally there should be only one graph per page. In this report it is okay to have the 2 number lines on a single page.

Determining the significant figures for the density using the eqn. On page 8 are tricky so be careful.

2 (Separation of the Components of a Mixture):. Pre-lab 'quiz' on Carmen (takes you to an external link, which can also be reached at the following link).

Due before the lab period. Online Prelab: Online at. Corrections, changes or hints to the lab manual:. Use the 4-mL test tubes. These are the small test tubes in the drawer or the front of the room. Take only about 6 mL of the dichloromethane (CH 2Cl 2) in a small graduated cylinder from the cart and bring it back to your hood (place in hood). You can always get more if needed.

Use about 2 mL of dichloromethane at a time to wash the sample. That's about half-way up the 4-mL test tube. Use a micropipet to remove decantate (liquid above solid).

Be careful not to remove the solid. You may need to counter-balance the centrifuge with a test tube of H 2O. In Part C resting the crucible lid on the clay triangle can help to stablize it. You have to be really careful not to break the lid or you will have to start over. Collect organic waste in a beaker at your desk. Use about 5 mL of dichloromethane to wash the solid organic off the watch class into your beaker. You should rinse more than once so divide up the 5 mL of dichloromethane into small aliquots.

Pour your waste into the large beaker provided in the orgnaic waste hood (one with red solvent can). Rinse your beaker with a little dichloromethane. Record total volume on waste sheet and sign. Dispose the isolated water soluble inorganic compound down the sink.

Dispose the insoluble inorganic compound and your remaining sample in the metal salts hood. Throw empty plastic vials in trash cans.

Post-lab 'quiz' on Carmen (takes you to an external link, which can also be reached at the following link). Due before the next lab period when the report is due. Online Postlab: Online at. Exp. 3 (Development of an Equation):. Pre-lab quiz on Carmen.

Due before the lab period. Corrections, changes or hints to the lab manual:. Counter-balance the centrifuge with a test tube of H 2O as shown in the video. Save time by centrifuging multiple test tubes at once.

Part D: Count and accurately measure the drops of solutions. Record the appearance and relative amounts of precipitate after centrifuging. Rinse the dropping tube and stirring rod with distilled H 2O between each solution. Dichloroethane, C 2H 4Cl 2, will be supplied in several bottles with droppers. Use about 30 drops total. The dicholorethane may split into two layers above and below the aqueous layer. Centrifuge the test tube which tends to force it to form one layer.

The dicholorethane is more dense than water so it will be on the bottom. Collect waste solutions in a beaker at your desk.

Pour your solutions into large beakers provided in the metal salts waste hood and sign waste sheet. If you don't complete part D cap the test tubes with cork stoppers and give to your TA to store in their locker. You can complete the exp in the next lab period. You should have the table 3.1 (on page 34) in the notebook (filled in) before lab.

You need a lot of space for observations. Look at the report sheets starting on page 37. Reproduce the table for Part D on page 39 in your notebook. 32): Save the test tube for part C.

Part B steps 4 and 5 on p. 33: Do NOT heat anything in step 4.

Heating takes place in step 5. WARNING: In this part you will be generating H 2S.

It smells like rotten eggs. Make sure the tubes are in your hood. NO Post-lab.

4 (EQW - Determination of the Molar Mass of an Unknown Acid):. Pre-lab 'quiz' on Carmen (takes you to an external link, which can also be reached at the following link). Due before the lab period. Online Prelab: Online at. Corrections, changes or hints to the lab manual:. General Directions for Quantitative Analysis - Titrations:.

Technique is very important. You are graded on accuracy for this exp. Buret techniques are discussed in Appendix D of the laboratory manual. Refer to pages D-3 and D-4 about titration in the manual. Cleaning the buret - the solution should drain completely - no 'beading'. Filling of buret - NO air bubles in the buret tip. (Wire to clean out tip available in 231 CE.).

Reading the buret - estimate to the nearest 0.01 mL. Buret reading cards are available from the cart near 231 CE. Manipulation of the stopcock. Learn how to do this so you can get only 1/2 a drop. Thoroughly mix reagents. If you get anything on the side of the flask wash down the side flask with distilled H2O from a wash bottle. Avoid splashing in the reaction flask.

Appearance of the end point - stop adding NaOH when 1/2 drop or less causes the first faint pink color to appear (stays pink). Use the SAME balance for BOTH Parts A and B. SAVE the standardized NaOH solution from Part A for Part B. Prior to the first titration in Part A shake the NaOH solution to mix thoroughly. Do a 'dirty' titration. In a 'dirty' titration you set things up as if you are doing a real titration but you aren't going to be really careful.

Instead you add about 1 mL of your titrant (liquid in the buret) and swirl the flask to mix. If the pink color disappears you aren't at the equivalence point yet. Keep adding the titrant, about 1 mL at a time. Keep track each time whether the pink color disappears after swirling. Eventually the pink color will not disappear. This gives you a decent idea of how much titrant you can add in the real titration quickly before you need to start being careful and adding only 1 drop at a time (or even 1/2 a drop). If you add only a few drops at a time the first time through it will take you forever.

If you do things correctly you will have enough NaOH to do all necessary titrations. If you use less than 10 mL of the standardized NaOH solution in Parts A or B discuss this with your TA. You want to make sure the volume of NaOH used is more than 10.00 mL so you get 4 s.f.

For the volume. You use the NaOH from Part A in Part B so do NOT throw it out after you finish part A.

If you don't finish, stopper the Erlenmeyer flasks containing the standard NaOH soln. Tightly to avoid contamination by CO 2 from the air.

Write your name on it and give it to the TA. Part A: The molarity of the NaOH for the two trials should be w/in 1% of each other, maximum of 4 titrations. The molarity should be given to 4 sig. Part A: KHP stands for potassium hydrogen phthalate, KHC 8H 4O 4. This does NOT contain phosphorus and the molar mass is greater than 200 g/mol.

Part B: Repeat the titration until the molar mass of your unknow acid agrees w/in 1% (calculate the molar mass assuming it's a monoprotic acid). Maximum of 4 titrations. Collect excess solid unknown acid in a weighing dish and dispose in the inorganic waste beaker in the hood. Label 'organic acids - Expt. Return excess KHP to TA. All solutions can go down the drain (rinse with water). ALL SOLUTIONS DOWN DRAIN.

Empty plastic vials in trash cans. Data-entry link on Carmen (takes you to an external link, which can also be reached at the following link). Due before the next lab period when the report is due. Online Postlab: Online at. Exp.

5 (CAL - Calorimetry and Hess's Law):. Pre-lab quiz on Carmen. Due before the lab period. Corrections, changes or hints to the lab manual:. You will obtain a digital thermometer dispaly unit and probe from Room 231 or 331. An OSU picture ID or driver's license must be traded for them. See Appendix E.

Ohio State Chemistry 1210 Lab Manual

Do NOT use your mouth for pipetting. Instead, use a blue pipetting bulb from the locker. Refer to Appendix D in the Laboratory Manual for a discussion of pipetting technique. The bulb should NOT be forced onto the pipette. It 'sits' on top.

Each Styrofoam cup should have a lid. Punch a hole in it for the thermister probe.

Keep the tea cup calorimeter away from boiling water. Place the cup in a 400-mL beaker to stabilize it. Do NOT use a negative value for the heat capacity of the Styrofoam cup. If the correctly calculated value turns out negative (due to experimental error) then assume the heat capacity of the Styrofoam cup is zero and use that for parts B and C. See for a discussion of graphing. An example of a good graph was also passed out in lab.

The graph on page 59 is just a rough example of what to do. All the graphs look essentially the same. You can use Excel for manipulating your data, doing calculations and graphing.

If you don't know how to use Excel take a look at my example for exp 14. You can always come to me for help. If you do use Excel for doing calculations you must still show the required sample calculations.

If you are supposed to obtain a slope from a graph use the slope from Excel but show how you would get a slope using points from your graph (and that you used the slope Excel determined). For this exp.

You can plot the points (scatter graph) and then draw your required lines in by hand. Make sure you have Excel draw lots of grid lines on the graph so you can get more accurate results for your time and temperatures from the graph. You could have Excel plot your straight lines but this would be a little trickier. Again, if you want help come see me.

If the temperature does not rise at least 5 degrees, check the probe. The easiest way to do this is to place it in boiling water.

Defective display units or probes should be given to Room 231 or 331 when you get another one. Return thermometers to storerooms. All solutions can be poured down the drains. Waste disposal: Reacted and excess sample may be disposed down the drain while running water.

Throw out empty plastic vials in the trash cans. Help with Exp 5 Graphing. See Appendices B and F for a discussion of graphing. An example of a good graph was also passed out in lab. All three graphs look essentially the same. Also, take a look at the help link just above this section.

You can use Excel for manipulating your data, doing calculations and graphing. If you don't know how to use Excel take a look at my example for exp 14. You don't have to use Excel (you can draw your graphs by hand) but I highly encourage it. You can always come to me for help. If you do use Excel for doing calculations you must still show the required sample calculations.

If you are supposed to obtain a slope from a graph use the slope from Excel but show how you would get a slope using points from your graph (and that you used the slope Excel determined). For this exp. You can plot the points (scatter graph, points only) and use the drawing function in Excel to draw the required lines (time-of-addition and best-fit lines for determining T i and T f) or draw them by hand. Make sure you have Excel draw lots of grid lines on the graph so you can get more accurate results for your time and temperatures from the graph. You could have Excel plot your best-fit straight lines but this would be a lot trickier. If you can't figure out how to draw the lines in Excel and get text boxes for T i and T f I suggest you print the graph using Excel and draw in the T i, T f and time-of-additon lines by hand and then scan the graphs for inclusion in your report.

Again, if you want help come see me. The following is an example of a pretty good graph using Excel for Exp 5 (part A).

The intial temperature readings are not very good but overall the graph is good. It has a good title and axis labels.

It has the proper sig. On the axes (the s.f. For the time axis may differ depending on how careful you were keeping track of your time but in the end most likely can't be very accurately reported past a tenth of a minute). There are a lot of gridlines. This is the only set of graphs this semester that will require to you have Excel print the grid lines.

Ohio State Chemistry 1210 Lab Manual Answers

Note, the T i, T f and time-of-additon lines were not drawn in by Excel. Print the graph and draw in those lines by hand (it's the easiest thing to do). There are actually two graphs of the same data. The first one doesn't have the best-fit lines drawn in. The second one has the lines drawn in.

Note, for the best-fit line for T i I only fit the line to last 4 data points since the first few readings were rather erratic. You don't have to use 'bad' data points when producing a best-fit line. Note the graph occupies pretty much the whole page with minimal page margins (I used margins of 0.10 inches). I told Excel to draw major grid lines on the y-axis every 1 degree (major unit of 1) and minor grid lines every 0.1 degrees (minor unit of 0.1). On the x-axis I had Excel draw major grid lines every 1 minute and minor grid lines every 0.2 minutes (only 5 grid lines between each major grid line marking 1 minute intervals).

This made it a little more presentable on line and considering you are only estimating your actual time of addition (unless you explicitly recorded it) it's probably good enough. Finally, the graph (whether by hand or using Excel) should be set up in portrait mode with the temperature values on the long side of the paper and the time values on the short side of the paper. The default in Excel is Landscape so you will have to set it to portrait mode (using 'Page Setup' or 'Page Layout'). 10 (IGL - Investigation of a Real Gas: Determination of Molar Mass and van der Waals' Constant):. Pre-lab quiz on Carmen. Due before the lab period. Corrections, changes or hints to the lab manual:.

TAKE ALL BROKEN MODIFIED FLASKS TO ROOM 231/331 CE. The modified flasks must be returned at the end of the session. Do NOT place them in your lab drawers. Pressure units of atm must be used in the IGL. The volume should be in liters. Evenly distribute tygon tubing on glass tip and flask.

Remove tubing as you would a champagne cork (gradually - a little on each side). A buret clamp should be used to hold the flask in the hot water. You should carry the flask in your hand. The modified flasks are to be IMMERSED IN, not floated on, the hot water contained in a trough. Keep the trough FULL! The vapors from the unknowns are flammable so flames are not to be used near the troughs.

Each trough is heated with an electric hot plate. Both the mass of the EMPTY flask and that of the flask containing the condensed liquid should be determined with the same analytical balance. However, if the mass is greater than 110 g, use the PE 600. Use a PE 600 balance to determine the mass of the flask when filled with water. The mass of the empty flask must be obtained when the flask is dry (both inside and outside). The flask with condensed liquid must be cool.

(Cold water may be used on the outside of the flask after it's cooled somewhat.) Dry the outside before weighing. Don't let it cool too much. While still slightly warm to the touch start taking the mass. When weighing the flask after cooling it take the initial reading after placing the flask on the balance and write that in your notebook. If the reading steadily decreases use the initial reading as the mass of the reliquefied unknown.

If the mass starts increasing you can't use the initial reading. You need to further cool the flask. Then reweigh it and record the mass and wait to see if it decreases or increases. If it still increases cool it further. If it decreases use the mass you recorded.

Ohio State Chemistry 1210 Lab Manual Answer Key

You must wait until you see the mass first start to decrease. When this occurs take that reading and use that as your mass for the reliquefied unknown.

Be careful not to cool it too much. What's going on? When you vaporize the 5 mL of your compound you are also forcing the air which was in the flask out. Once all of your compound has vaporized essentially all the air has been forced out. What happens when you cool the flask? As the flask cools the air starts to come back in. You sample starts to liquefy but it also vaporizes (goes back to the gas phase).

As the flask is cooling so much air is coming back in the vapor of your sample can't get out very easily (and escape into the room). As this is occuring the mass of your flask will actually go up as the air flows in (remember, when you first weighed it there was air in the flask). Once all the air which is going to flow into the flask as it cools has come back into the flask your sample can now escape (leave) more easily as it vaporizes (evaporates).

As this happens the mass of the flask decreases because the reliquefied unknown is vaporizing and leaving the flask (evaporating into the room). If you left it on the scale for several hours your entire sample would eventually evaporate and pretty much leave the flask. The mass would keep decreasing. You don't want this to happen. You're trying to 'catch it' just as the air stops coming back in at a rapid rate as it cools and before your reliquefied sample has a chance to evaporate and escape.

This is why you want to weigh it several times as it cools. Check that the barometric pressure is reasonable (above 735 mm Hg). If not, speak to the TA. Record the barometric pressure to 1 decimal place. Use a medicine dropper attached to a water aspirator for evaporating acetone in the flask (Fig. 10.3), and for removing water (Fig.