My chem professor is literally no help these days. God bless you. Having no option but to do Chemistry online is difficult! I’m sure a lot of students are having a hard time during this quarantine.
A thank you from Australia!! I’ve got a chem personal project and I’m so glad I found this! Sometimes I’m afraid to ask questions in class so I’m glad I can learn and rewatch your vids until I understand without judgement!
Thank you so much for your help ❤❤youi just worked as an angel for me . Just loved the way of your explaination thank you so so much for Your help from the bottom of my heart ❤
Wish I watched this before my practical! It was on this experiment (chosen by prof. out of all the other experiments). Completely bombed the calculations. This was super helpful and I now understand it 100%. I still have my theory exam which will involve calculations, I hope this will be on it so I can prove what I've learned!!!! Thank you so much for your knowledge.
Holy moly thank you so much for this video! We had lab online and in person but still didn’t know how to solve all of this! You helped me and my girl friend so much! Thank you!
Hello! Great video is gonna be a great help for my final on this with the exact same chemicals, my question is how would I find avg number of NaOH used in the trials?
Thankyou from Australia, we have a prac on this exact titration coming up which goes towards our final score in Year 12 Chemistry, so this really helped :)
Thank you so much .This helped me so much. I am on 2 week break and I have a chemistry test 2nd day back and this has clarified so much. Just one question, when you put final and initial amounts into the table. Is the initial amount, the amount of titrant that was in the Burnett’s before you added any NaOH? As it says an amount less than 1 but the final amount is around 35? Thanks again
The initial amount is the buret reading before any NaOH was added to the vinegar in the flask. Some instructors would have you fill your buret exactly to zero, but that is t necessary unless you plan to make a titration curve using pH probes and a graphing program.
I have a question with the 2 decimal places when marking down the volume of the titrant(NAOH). Wouldn't it be one decimal place as you can not be more accurate than the measurement equipment(the burette) itself? Or maybe is your burette just more accurate than the one I have at school as the one I use during practicals only measure to 0.1 of a mL. This was a very informative video and has cleared up many things for me. Thanks!
hi! this video was super helpful! i just had a quick question. if for my lab, i had used 6.12 g of NaOH, which converted to moles would be 0.153 mol of NaOH, would i use that when calculating the molarity of the acetic vinegar? or would i use the molarity of the NaOH standard solution?
Since it is a 1:1 mole ratio if 6.12 grams was needed of NaOH to neutralize the Acetic Acid you would have 0.153 mol of acetic acid which you could then divide by the volume of the acetic acid used (vinegars volume).
Amazing. I can see that you used the stoichiometric mole ratio to calculate the concentration of the acid. I want to ask, what if I used the M1V1=M2V2, equation, cause this equation doesn't consider stoichiometric balance. What would be the effect
You can definitely use that equation because the mull ratio is one to one. There are titrations where the mole ratio is not one to one. I prefer to have my students use that instead of the dilution formula. Just builds better understanding using stoichiometry.
Your base NaOH will be diluted and you will use more volume of it Then you will calculate that you had more moles of acid present so the molarity would be larger than it actually is.
Hi Anne, are you able to tell me how you know you have reached equivalent point? If I understand this correctly, the end point is when the solution becomes pink after swirling the flask, but im struggling to understand the difference between these two points? Thank you!
Equivalence point is where mathematically the moles of acid are equal to the moles of base for this titration. The endpoint is a color change from the indicator that signals that that point has been reached. A specific indicator needs to be used for different acid and base titrations depending on if the acid or base are weak or strong.
As long as the mass of acid or volume of acid was taken at the start, the moles of acid doesn't change so adding water has no effect on the calculations.
Professor, I would like to ask you some questions. Why we need to add distilled water into vinegar? One more thing, when we calculate the C of vinegar, we use the original volume of vinegar or the volume of vinegar+distilled water?
You don’t need to add distilled water to the vinegar it just helps to carry out a good titration by washing down the inside of the flask. Use the original volume of vinegar.
You will need to have the density of vinegar in grams/mL to convert the volume used to grams to total mass. Then you can use the moles of vinegar used and the molar mass to find the mass of the acetic acid molecules. Then divide the mass of the acetic acid by the total mass of the acetic acid solution used and x 100.
No it’s not. As long as you have the original volume of vinegar you will then find the “unknown” moles of acetic acid from the titration with your standard solution. Then you can find the experimental molarity by dividing moles by volume.
Hi Anne, just a quick question why did you do all the calculations separate and then average the Molarity. Would it not have been quicker if I just averaged the titre values and completed the calculation once?. I appreciate hearing from you soon , thanks for this video!
Possibly, but I used different volumes of base and many times you will have different volumes of acid. So averaging the Molarity is typical vs averaging volumes.
That would be double the typical percent of 5% acetic acid and has a M of around 0.83 M. This video I don’t discuss the calculations to change the moles of acetic acid into a mass percentage.
This video helped me thank you so much. And I want ask you that when calculate the average volume of NaOH should we get the .01 values? If yes, should we get the lowest numbers or numbers with .01 decimals?
Phenolphthalein will be no color in the vinegar (maybe cloudy due to the fact that it is dissolved in alcohol). It will turn pink when you have excess base ions because of its equilibrium reaction. I just used the vinegar I bought from the store. You could make "vinegar" from more concentrated acetic acid solution and dilute it to make about 0.8-0.9 M solution of acetic acid.
Adding distilled water helps wash the sides of the flask, gives more volume to mix, rinse the tip of the buret or help add that one drop of titrant. If you measured the mass of volume of your titrand (substance in the flask) you have the mass/moles/volume and the water doesn't alter that quantity, just dilutes it.
I made the solution of NaOH to be approximately 0.50 M NaoH, however you would need to standardize it using a separate titration with something like KHP to get the actual molarity of NaOH because solid NaOH pellets absorb water when exposed to air and will not be able to be massed correctly. I do have a video on how to standardize NaOH with KHP at least calculation wise.
Yes, however, there is a chance you may need more than 50.0 ml of the base. If that happens you will need to stop and record your final volume of base. Then refill the buret, taken a new initial and then final reading once it is neutralized. Then add the two volumes of base together to get the total base volume used.
I have one simple question, isn't the endpoint is the point where you have a slight excess of the titrant? I mean, at the equivalence point for the acid-base titration, wasn't that supposed to be neutral as they are in equilibrium? Otherwise, I enjoy watching your educative videos and thanks a bunch!
Thanks! Because this is a weak acid with a strong base the equivalence point, where the acid is neutralized and all that is left in solution is the conjugate base ion (acetate) with water, so the pH is around 9 when all the acid is neutralized. This is why phenolphthalein is used because it turns light pink around that pH.
My chem professor is literally no help these days. God bless you. Having no option but to do Chemistry online is difficult! I’m sure a lot of students are having a hard time during this quarantine.
Marisol Torres sorry to hear that, but glad to hear the video helped you during this tough time.
I agree, it’s so disappointing, it’s almost criminal. Thank you Ms.Schmidt
Same he doesn't even respond too my emails
@@Dbf1339 Same here. This is so helpful!
🎉 that is great😊
This video was beyond helpful, even 5 years later. You're a wonderful educator and explained this complex reaction is such a simple way!
Thank you so much! Comments like this help encourage me to keep making content.
thank you for helping me with online simulation during this COVID-19 outbreak.
citoh 00 glad the video helped you!
You're not the only one who needs this
The only 15-minute lecture video that I actually watched from beginning to end. This is so helpful. Thanm you so much!
Thanks Anjo!
A thank you from Australia!! I’ve got a chem personal project and I’m so glad I found this! Sometimes I’m afraid to ask questions in class so I’m glad I can learn and rewatch your vids until I understand without judgement!
Outstanding to hear! Best wishes ☺️
this is very helpful and straightforward, thanks for helping a fellow chemistry student who is barely surviving
Glad to hear the video helped you! Keep trying and you will succeed.
Thank you for the calculations, you make it make sense. I returned to college and taking a course without a textbook. Thank you again.
@@Priscilla-L33 Thank you for this wonderful comment! Happy to help and great to hear my explanation of the calculations were helpful to you.
You have no idea how much you helped me.
Super to hear the video was helpful! Best wishes
this was super helpful for my lab tonight! Thank you for how clearly you showed all the steps!
Thanks 😊
Thank you, You are my COVID19 online lab hero... I'm your fan #1 !
Thank you! Hopefully, more labs to be loaded besides the ones already on my channel.
God bless you woman. I have seen some senseless videos our school sent us. But this really helped
Glad to hear the video was helpful!
Literally the best video on titration! Thank you so much
Thank you David! Outstanding to hear it helped you.
Your explanation is very easy to understand! Thanks!
Thank you Ralph!
I noticed this video was Post for few years now, and it's going to help me today. Thank you
That’s outstanding!
There's a spot in heaven waiting for you! You're amazing:)
Aww 🥰 thank you Ciara❣️
Thank you, I have this experiment in HOL and I had no idea what I was suppose until I saw this video. This cleared things up so well!
Wonderful!
You just saved my chem lab grade. Very helpful. Thank you so much!!
Yay! Outstanding 😁 and you are very welcome.
I can finally complete my chemistry assignment thanks to you! great video :)
That’s great to hear Coral! Thank you and best wishes.
Thank You!!
Now I actually understand what to do in my Chemistry depth study.
prpawar You’re Welcome 😊 Glad to hear the video helped you be more successful with Titrations!
Have to do this titration alone for a final today and you really helped with my calculations bless you!
It’s wonderful to hear that my video helped you with your final today. Thanks for the wonderful comment. Best wishes in your studies.
Ma'am you are such a great teacher and this channel deserves millions of subscribers , stay blessed ma'am 💚
Thank you Abhishek!
Thank you so much for your help ❤❤youi just worked as an angel for me . Just loved the way of your explaination thank you so so much for Your help from the bottom of my heart ❤
You are so welcome❣️Comments like these brighten my day and make me feel like I’m paying it forward as well as making a difference.
Wish I watched this before my practical! It was on this experiment (chosen by prof. out of all the other experiments). Completely bombed the calculations. This was super helpful and I now understand it 100%. I still have my theory exam which will involve calculations, I hope this will be on it so I can prove what I've learned!!!! Thank you so much for your knowledge.
Happy to help and best wishes Kiran on the theory exam!
@@AnneSchmidt thank you!! :)
@@kiransomal3525 you are so very welcome! Best wishes 😃
This is lovely I haven't seen any teaching practical chemistry as you do
Thank you!
Thank you for your help, lots of love from a Brazilian student who doesn’t have lab classes yet because of covid here :(
Thank you Camila ❤️ Wishing for lab experience soon for you.
this video is very informative and i think this video will help a lot in my upcoming IGCSE Chemistry exam next week
thank you so much
Thank you Mohamed!
Holy moly thank you so much for this video! We had lab online and in person but still didn’t know how to solve all of this! You helped me and my girl friend so much! Thank you!
That’s great to hear! So glad the video was helpful 😃
Thank you so much this is the best titration video I have seen
Thank You! This is outstanding to hear. Best wishes 🧪
This is an excellent explanation! Next week I will have chem exam, I think it can help me a lot! Thank u for your video😊
Thank you 😊
It’s nice to hear the video was helpful!
Best wishes on your Chem exam.
Anne, your video came up when I was searching for titrations! Great work :)
Very Cool. Thanks Katy!
Super job. I understand it now because you explained all steps clearly.
Lee Oliver yeah! That is so great 😃 to hear.
This was really helpful! Thank you so much for the additional information as well!
Simply brilliant and informative 🇯🇲
Thank you very much. Both content and clarity of your video are excellent
I appreciate the wonderful comment! Great to hear the video so efficient and helpful.
bless you. you are really helping me understand what to do for my chem lab.
Jada Smith yay! That’s super great 😀 Glad to help 👍🏻
Thank you that was very helpful. I was lost as to how to fill out the lab manual. Do you think you can do a video on stoichiometry? Thanks again.
Glad the video helped. Stoichiometry is on my list of videos I need to make very soon!
Hello
How can I get the summary of the experiment?!
Please help me I have to write a summary about that😫and I have to work on a project for design.
I'm doing this experiment tomorrow, so thanks for the heads up video
Hope the video was helpful!
Really thank thee for helping me in Chemistry course!
Outstanding 😃 Happy to help!
Watched your video before my practical exam on titration. Coming back to thanks for the A🥰
Congratulations 🎉 and thanks for the thank you! Always wonderful to hear my videos are helpful.
Thanks a lot, ma'am......this video helped me at the last moment
Outstanding! Glad it was helpful 😁
Hello! Great video is gonna be a great help for my final on this with the exact same chemicals, my question is how would I find avg number of NaOH used in the trials?
Nice! Good luck and thank you 😊
That was outstanding
Thanks for the clear explanations
Thank you! Great to hear the video was helpful and clear.
Thank you!! I feel so prepared now for lab
@@nataliegaskill3 yay! 😀 that’s outstanding to hear.
Thankyou from Australia, we have a prac on this exact titration coming up which goes towards our final score in Year 12 Chemistry, so this really helped :)
Great to hear the video helped! Best wishes on your lab prac on titrations.
Thank you so much .This helped me so much. I am on 2 week break and I have a chemistry test 2nd day back and this has clarified so much. Just one question, when you put final and initial amounts into the table. Is the initial amount, the amount of titrant that was in the Burnett’s before you added any NaOH? As it says an amount less than 1 but the final amount is around 35?
Thanks again
The initial amount is the buret reading before any NaOH was added to the vinegar in the flask. Some instructors would have you fill your buret exactly to zero, but that is t necessary unless you plan to make a titration curve using pH probes and a graphing program.
Really thank thee for helping me in Chemistry course
You are very welcome.
@@AnneSchmidt THANKS
This video is very helpful. Can I know what brand of vinegar you used?
Thanks. I don’t remember the brand!
Thank you so much for this video. Is there any way you can teach to calculate ph and poh without using the calculator
Glad the video helped you! I like the idea 💡 of showing how to calculate or estimate the pH and pOH without a calculator.
thank you for helping with online simulation of this important chemistry topic during this COVID-19 pandemic and online classes.
It’s wonderful to hear that the video was helpful for such an important chemistry topic. Thanks Pedro 😅
I have a question with the 2 decimal places when marking down the volume of the titrant(NAOH). Wouldn't it be one decimal place as you can not be more accurate than the measurement equipment(the burette) itself? Or maybe is your burette just more accurate than the one I have at school as the one I use during practicals only measure to 0.1 of a mL.
This was a very informative video and has cleared up many things for me.
Thanks!
Burets read an estimated hundredths place because there are markings ever tenths place.
hi! this video was super helpful! i just had a quick question. if for my lab, i had used 6.12 g of NaOH, which converted to moles would be 0.153 mol of NaOH, would i use that when calculating the molarity of the acetic vinegar? or would i use the molarity of the NaOH standard solution?
Since it is a 1:1 mole ratio if 6.12 grams was needed of NaOH to neutralize the Acetic Acid you would have 0.153 mol of acetic acid which you could then divide by the volume of the acetic acid used (vinegars volume).
I love this ..
Such a Great moment WITH U
Thank you 😊
Thank you so much kween!
😁
Can i ask where did you get the 0.50m of NaOH? Is it in given or you just right it? Please help me
That was the given standardized solution that was able to reach an equivalence point for vinegar in under 30 ml.
What is the inital and final reading of the buret? I can not zoom in on the video
It’s in the data table in the second half of the video
Amazing. I can see that you used the stoichiometric mole ratio to calculate the concentration of the acid. I want to ask, what if I used the M1V1=M2V2, equation, cause this equation doesn't consider stoichiometric balance. What would be the effect
You can definitely use that equation because the mull ratio is one to one. There are titrations where the mole ratio is not one to one. I prefer to have my students use that instead of the dilution formula. Just builds better understanding using stoichiometry.
@@AnneSchmidt Thank you. 🙏
How the calculated molarity of vinegar could be affected if I forgot to rinse the burette with the titrant solution in the beginning?
Your base NaOH will be diluted and you will use more volume of it Then you will calculate that you had more moles of acid present so the molarity would be larger than it actually is.
Do I need to add water to the flask if i am measuring the concentration of acetic acid. will not adding water produce diffrent/wrong result?
this video is a god send
Aww ☺️ thanks! Happy to help.
What was the initial and final reading of the acid? I know the volume of vinegar was 20.00 mL.
Both are in the video and in the first calculation halfway through the video.
Thank you! I appreciate you uploading this!
Whitney, I am happy to hear the video helped you!
Hi Anne, are you able to tell me how you know you have reached equivalent point? If I understand this correctly, the end point is when the solution becomes pink after swirling the flask, but im struggling to understand the difference between these two points? Thank you!
Equivalence point is where mathematically the moles of acid are equal to the moles of base for this titration. The endpoint is a color change from the indicator that signals that that point has been reached. A specific indicator needs to be used for different acid and base titrations depending on if the acid or base are weak or strong.
Does the added water to add the suspended drop not effect the endpoint?
As long as the mass of acid or volume of acid was taken at the start, the moles of acid doesn't change so adding water has no effect on the calculations.
Professor, I would like to ask you some questions. Why we need to add distilled water into vinegar? One more thing, when we calculate the C of vinegar, we use the original volume of vinegar or the volume of vinegar+distilled water?
You don’t need to add distilled water to the vinegar it just helps to carry out a good titration by washing down the inside of the flask. Use the original volume of vinegar.
@@AnneSchmidt Thank you so much.💚
@@sasase3303 you are so very welcome!
Hello Anne,
Thanks a ton for the video. I need one more help if you can. Can you please explain how do we convert molarity to mass percentage?
You will need to have the density of vinegar in grams/mL to convert the volume used to grams to total mass. Then you can use the moles of vinegar used and the molar mass to find the mass of the acetic acid molecules. Then divide the mass of the acetic acid by the total mass of the acetic acid solution used and x 100.
You are a lifesaver! Thank u so much!
Happy to help!
can i ask how many drops of indicator were used for each trial?
Two-three
Thank you very much for this video, I now feel confident in my results!
Whohoo! That is great to hear Rosa.
@@AnneSchmidt Can we use your video at our lab lesson
İsmail Emin Kula absolutely!
Is the HOH accepted instead of H2O.
Yes
What a video mam,,
Wow ⚗️⚗️
Keep making video
Your big fan from India ,Mam
Ashutosh Patel thank you! Glad the video helped 👍🏻
Hi ms, I have heard that you have to dilute the vinegar first before the titration. Is this necessary?
No it’s not. As long as you have the original volume of vinegar you will then find the “unknown” moles of acetic acid from the titration with your standard solution. Then you can find the experimental molarity by dividing moles by volume.
@@AnneSchmidt I see thank you!
Can you tell me what factor affects the rate of this reaction and how?
How did you get 0.5mol of NaOH? Just wondering
I made that NaOH solution and standardized it.
@@AnneSchmidt How did you make and standardized it?
Is bioenzyme acidic or alkaline in nature?
Hi . I have a question. Was that a 5% vinegar from supermarket? Thank you
Yes it was!
Hi Anne, just a quick question why did you do all the calculations separate and then average the Molarity. Would it not have been quicker if I just averaged the titre values and completed the calculation once?. I appreciate hearing from you soon , thanks for this video!
Possibly, but I used different volumes of base and many times you will have different volumes of acid. So averaging the Molarity is typical vs averaging volumes.
@@AnneSchmidt Oh makes sense, thanks for letting me know!
Was the phenolphthalein add to the burette or in the flask?
The flask!
how do you know how much vinegar to put inside the Erlenmeyer flask?
Any volume that doesn’t need more than 50 mL of your titrant
I used a vinegar solution that contained 10% vinegar and 90% distilled water, when do I factor this into my calculations?
That would be double the typical percent of 5% acetic acid and has a M of around 0.83 M. This video I don’t discuss the calculations to change the moles of acetic acid into a mass percentage.
This video helped me thank you so much. And I want ask you that when calculate the average volume of NaOH should we get the .01 values? If yes, should we get the lowest numbers or numbers with .01 decimals?
If you average the volumes keep the average to two decimal places.
@@AnneSchmidt okay. Thank you so much
Thank you very much for this video..
😄
Great to hear the video was helpful! 😃
Very very very helpful ❤️❤️
@@juliyabiju5382 outstanding!
Thank you soo much mam, can u please put the reference for this method??
Hi did u make an aliquot of the vinegar? Since once I tried it in school the phenolphthalein indicator did not show at all. Thank you
Phenolphthalein will be no color in the vinegar (maybe cloudy due to the fact that it is dissolved in alcohol). It will turn pink when you have excess base ions because of its equilibrium reaction. I just used the vinegar I bought from the store. You could make "vinegar" from more concentrated acetic acid solution and dilute it to make about 0.8-0.9 M solution of acetic acid.
Thankkk youuu!!!!!!❤
@@ankitdas8709 you are very welcome! Great to hear the lab video was helpful.
Keep it up 🌹 love from Ukraine
Thanks and sending you love back. Stay safe
Hi Ann, are you still there. Please can you tell me how to make white vinegar
I didn't make the vinegar, I bought it!
Why do you add distilled water. And why won't it affect the the values?
Adding distilled water helps wash the sides of the flask, gives more volume to mix, rinse the tip of the buret or help add that one drop of titrant. If you measured the mass of volume of your titrand (substance in the flask) you have the mass/moles/volume and the water doesn't alter that quantity, just dilutes it.
Beautiful and smart Chemist
Thank you 😊
How do you get .50 for the NaOH standardized mole?
I made the solution of NaOH to be approximately 0.50 M NaoH, however you would need to standardize it using a separate titration with something like KHP to get the actual molarity of NaOH because solid NaOH pellets absorb water when exposed to air and will not be able to be massed correctly. I do have a video on how to standardize NaOH with KHP at least calculation wise.
May I know where did you get the accepted value?
Many reputable chemistry Websites give the accepted value.
Oh god thank u for helping me w the calculations
Happy to hear the video helped you!
Can I change the initial volume of vinegar to 15cm^3 instead of 25cm^3 and use the 0.1M?
Yes, however, there is a chance you may need more than 50.0 ml of the base. If that happens you will need to stop and record your final volume of base. Then refill the buret, taken a new initial and then final reading once it is neutralized. Then add the two volumes of base together to get the total base volume used.
this is so helpful thank you!
😊
thx for the help 2 but you had a miscalculation for volume of NaOH used for second trial! Still helped
Hello, can I ask what was the equivalence point on the experiment? How can we identified it
The equivalence point is when the indicator changes color. If a pH meter was used you could see the equivalence point graphically.
I have one simple question, isn't the endpoint is the point where you have a slight excess of the titrant? I mean, at the equivalence point for the acid-base titration, wasn't that supposed to be neutral as they are in equilibrium? Otherwise, I enjoy watching your educative videos and thanks a bunch!
Thanks! Because this is a weak acid with a strong base the equivalence point, where the acid is neutralized and all that is left in solution is the conjugate base ion (acetate) with water, so the pH is around 9 when all the acid is neutralized. This is why phenolphthalein is used because it turns light pink around that pH.
Can you please tell me how did you get 0.60 as the initial volume of NaOH..
That’s the buret reading after filled.
Thank you so much. You help me a lot, I appreciate 🌹
Yay! It is fantastic to hear the video helped you 😁
Thanks ❤️❤️❤️❤️Really for helping
Mayar Potter so happy to hear the video helped you! Pass on the help others💜
Would you be able to share the mass of the empty vial and the mass of the vinegar so I'm able to find density? Thanks!
I do not have that data. Sorry