Wow you have really taught titration to the fullest God bless you.i saw this particular question in another TH-camrs timeline it seems the question is going to come out .you really have the passion to teach you're a good teacher ❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰
I wrote my waec last year and mostly everything you explained during the pre practical came out.I wish you have an online tutorial for students like me who are interested in partaking in practicals
Great video again 👏. However, there is something that could confuse the viewers...when you use the formular, n =m/mm, you get your answer in mole, and not mol/dm^3. Since you divided 24.82 g by 248 g/mol, your answer must be 0.100 mol. I believe your question is incomplete. Had it been you wrote 24.82 g of thiosulphate dissolved in 1 dm^3, it would have resulted to 0.100 moldm^3 using the formula below; Molar conc= mass conc/molar mass Then you have; 24.82 g/dm^3/248 g/mol = 0.100 moldm^3. I hope this makes sense and helps viewers clarify their doubt about the calculations. In all, I must commend your confidence in teaching.
That’s an omission... The 24.82g is g/dm3 because 24.82g of Na2s2O3 was dissolved in water and made up to 1dm3.... Thanks for your comment 🙏🏻 I really appreciate
Yea it makes sense. I wanted to write 24.82g/dm3.... That’s why I said if not that you call my attention to that I didn’t even saw I omitted the dm3.... Thanks 🙏🏻 I appreciate
Please I see your videos helpful but however you must specify the type of titration so that we will know the right one to choose. For instance bank titration, redox titration, acid base etc🙏🙏
Well done sir. Your effort is appreciated. But I noticed that the mass concentration of iodine you got does not tally with the mass of the reacting iodine in the 25.4 g impure mixture in dm3 according to the calculations you did at the beginning of the video. Does this not matter?
You are doing a great job. But dont you think that its only the anhydrous part of the sodium trioxosulphate that reacted, and as such the molar mass should be 166gmol
The mass of the water is important too since it’s an hydrated salt.... You can’t leave the mass of water out... What if they ask them to calculate the amount of water of crystallization ? leaving the mass of water out will greatly affect the calculations
Thank you Sir. Sir, what if ur school provide iodine solution directly and not iodine crystals and potassium iodide to form the solution of iodine, will the experiment be accurate and if yes how can we measure the iodine solution for the titration.
If the question I predicted is same with the one given tommorow you can but please read the instructions tommorow to know if there is any slight change ✅
@@tazerdentertainment8601 Let’s wait to see if we would be asked to do that .... But when you acidify it will tend to increase the rate of the reaction
I followed this but unfortunately the titre value I got when thiosulfate is the burette is very small like 7cm3 Then with iodine in the burette I didn't get any reaction,I don't know where I missed it
Great job.... But don't you think the equation for the reaction should be with the hydrated thiosulphate and not the anhydrous...and that will be 4moles of Iodine and 1 mole of the hydrated thiosulphate
Pls can you check again, if a salt is impure, it means it has pure form of it with some impurities. So if what they gave in the question for impure is 12.2g and yiy calculated that of the pure to be 4.52, then tge impure should be 12.2- 4.52. Pls check it again
In as much as the funnel is removed before the titration starts at the initial was carefully checked before the titration... There is no problem about that
In redox titration there is nothing like acid or base... Kindly take your time to watch the video again to see how the practical and calculations was done ✔️
I don’t have the instructions sent to Ghana Teachers From Waec .... If You Can Get It Send to Me on +23408100059151.... I will Try and Come Up With Something
Actually I don't have that and getting it will be difficult because most of teacher here don't agree showing to students.So I think getting it will be difficult.Pls just try and do something for us
Job well done. Please Sir, if you use the specifications from Waec and you have the iodine solution in the burette, add starch solution to the thiosulphate and titrate, there will be color change from colourless to blue-black which is the end point. Though the end point is big.
@@askchemistryhangout Good morning sir pls Sir in your calculation of Cb you only calculated the mole pls is it also the same thing as your molar conc. because you used it in finding Ca
@@johnadam1214 I calculated my CB in mol/dm3 and also calculated in amount of moles.... Amount in moles and concentration in mol/dm3 are two different things
If the question indicates that the na2s203 should be in the burette and iodine solution in the conical flask✅ You Can Use that my end point💯 But wait and see what the question is like on that day before deciding on what to do📌
@@askchemistryhangout sir, it actually did oh. I did it, but it was exactly 50cm³. I crushed the iodine and poured into a hot KI solution a lot of it dissolved. I however don't think waec would request such procedure that gives such high end point value.
@@uchegodswill397 You Crushed And poured into a hot KI..... The reason why you got 50cm3 means that all the iodine dissolve which is practically impossible without you crushing and increasing the temperature..... I worked it out and got 50cm3 but that is practically not feasible for a titration that you use a 50cm3 burette..... I love your sincerity ✅ Any value lower than 50cm3 to me is not correct because that is the theoretical titre.... I doubt if waec will go that way.....
Well done sir. Your effort is appreciated. But I noticed that the mass concentration of iodine you got does not tally with the mass of the reacting iodine in the 25.4 g impure mixture in dm3 according to the calculations you did at the beginning of the video. Does this not matter?
It won’t tally cos all the iodine will neva dissolve in the KI... The mass of the KI given is too small to dissolve the iodine hence a small fraction of the iodine is what will dissolve ✅
This is great and unique, what a perfect teaching skill, God bless you sir.
You have done justice to this sir. God bless and honor you richly sir. Thank you sir.
Wow you have really taught titration to the fullest God bless you.i saw this particular question in another TH-camrs timeline it seems the question is going to come out .you really have the passion to teach you're a good teacher ❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰🥰
You're such a wonderful teacher..God bless you richly
Thanks a bunch for this awesome video. I owe you one!
Even though our teacher didn't explain ...I now understand this to the fullest sir .....thank you very much sir ....more grease to your elbows
Thanks so much
Every thing here comes out in this year waec
I appreciate ❤️❤️
If this kind of group dey for physics practical I won't have fuck up🤔🤔
I wrote my waec last year and mostly everything you explained during the pre practical came out.I wish you have an online tutorial for students like me who are interested in partaking in practicals
Am happy to hear this .... Chat me on 08100059151
Wow sir continue with this spirit I like the video
Splendid💯.
Thanks so much sir I pray God bless you
Thanks sir you are the best
We want more of this
Thank you sir,but which of the compound Is a base or acid.
may Almighty God take you higher than this sir😊So that we can be able to enjoy more of this sir, thank you very much for your relentless effort sir😍
Amen 🙏
Thanks alot. You made learning chemistry practical easy 😊
How can solutions be prepared ?
Thank you sir,I now understand every thing, God bless you.
Great video again 👏. However, there is something that could confuse the viewers...when you use the formular, n =m/mm, you get your answer in mole, and not mol/dm^3. Since you divided 24.82 g by 248 g/mol, your answer must be 0.100 mol.
I believe your question is incomplete. Had it been you wrote 24.82 g of thiosulphate dissolved in 1 dm^3, it would have resulted to 0.100 moldm^3 using the formula below;
Molar conc= mass conc/molar mass
Then you have; 24.82 g/dm^3/248 g/mol = 0.100 moldm^3.
I hope this makes sense and helps viewers clarify their doubt about the calculations.
In all, I must commend your confidence in teaching.
That’s an omission... The 24.82g is g/dm3 because 24.82g of Na2s2O3 was dissolved in water and made up to 1dm3.... Thanks for your comment 🙏🏻 I really appreciate
Yea it makes sense. I wanted to write 24.82g/dm3.... That’s why I said if not that you call my attention to that I didn’t even saw I omitted the dm3.... Thanks 🙏🏻 I appreciate
Thanks so much @Chemistry Hangout and thumb up @ Esther for the observation
Ok
Thanks for your information
It has been so so useful
God bless you sir
Sir please can you do double indicator titration experiment
It is suspected that it'll be dropping this year in the wassce fir Ghanaians
And most students are still not all that satisfied with their knowledge and understanding in it
You are really doing great my dear teacher I appreciate your afford to deliver for us the candidates 🙏🙏🙏🙏
Thanks for the kind words 🙏🏻
Thank you sir you are doing a great job
Thanks For Your Kind Words🙏🏻 Am honored
weldone teacher
I wrote my chemistry practical yesterday,and I have to say that this was super helpful.God bless 👍👍👍
Thanks 🙏🏻 Wish you Sucess ✅
Please I see your videos helpful but however you must specify the type of titration so that we will know the right one to choose. For instance bank titration, redox titration, acid base etc🙏🙏
Hello sir your videos are very interesting but i have a question. I needed to know why should we multiply the mass of a solution by 1000cm3 ?
Well done sir. Your effort is appreciated. But I noticed that the mass concentration of iodine you got does not tally with the mass of the reacting iodine in the 25.4 g impure mixture in dm3 according to the calculations you did at the beginning of the video. Does this not matter?
Well done. Great Chemistry teacher
My Co- educator and chemist.... Thanks for the word of encouragement 🙏🏻
Good day sir, please I love and understand your video but could you direct me to a good physics practical tutor for waec 2023. Thank you sir❤
Wow
Great work
Thanks 🙏🏻
Thanks teacher for teaching me
You are doing a great job. But dont you think that its only the anhydrous part of the sodium trioxosulphate that reacted, and as such the molar mass should be 166gmol
The mass of the water is important too since it’s an hydrated salt.... You can’t leave the mass of water out... What if they ask them to calculate the amount of water of crystallization ? leaving the mass of water out will greatly affect the calculations
Thank you Sir. May your efforts be well rewarded
Make Ona Dey ask of my bank account number 😂 Thanks for your kind words I appreciate 🙏🏻
Thank you Sir. Sir, what if ur school provide iodine solution directly and not iodine crystals and potassium iodide to form the solution of iodine, will the experiment be accurate and if yes how can we measure the iodine solution for the titration.
It has to be iodine crystals so you prepare with the specifications instructed by waec
U calculated mole of Na2so3. 5h20 nd u wrote mol/dm3.... Isnt dat d unit of molar conc.? Abi eyes dey pain me ni
Thank you so much! This was such a big help!
Am happy it helps
You finally found someone better than Mrs.Amaka.A?😭😂
Sir do u have something about Gh wassce chemistry
Please don't you have video of double indicator titration?
Great job sir 🎉🎉🎉
Thank God you are from Nigeria, alest we now have God send.But sir ,you are going higher places in Jesus name Amen!!!!
Thanks so much nice
God bless you
You are welcome 🙏🏻
Thank u so much sir. Pls if ur final readings are below twenty something . Is it correct.
yh
Nice one sir. Keep it up
Thanks 🙏🏻
how come your mass is in g/dm3 sir... wouldnt we be marked down
Please Sir, I would like you to include alternative to practical chemistry for private candidates in your teaching Sir.
No problem ✅
Is nice
Please is it likely Ghana will have similar questions? My boss
No please
Sir pls why didn't u leave ur initial readings at 0.00. Am confused.
My initial reading was 0.00 so after the rough titration I decided not to refill the burette cos I still have much solution in the burette
I really appreciate your presentation. God bless you and richly. I share your views on the question
@@adekunleayodeleogungboye3532 Thanks so much sir for your kind words🙏🏻 God bless You Too🙏🏻
Good day sir. Can I use this as my end point.
If the question I predicted is same with the one given tommorow you can but please read the instructions tommorow to know if there is any slight change ✅
Is it possible we could be asked to add H2SO4 to the solution to acidity it? If yes what effect will it have in my work.
@@tazerdentertainment8601 Let’s wait to see if we would be asked to do that .... But when you acidify it will tend to increase the rate of the reaction
Sir can you pls do some videos for Ghanaian students?
We will be starting our exams in August
We need you help pls
I will need the instruction sent to schools from WAEC if I will be able to help out .
@@askchemistryhangout okay sir thanks
When you get it send to me on +2348100059151
Okay sir
Pls how do we make starch indicator. Is it the same way we prepared starch we use on our clothes?
You can use Same starch too.... Jus measure about 1g and dissolve in 100cm3 of boiling water
@@askchemistryhangout Thank out Sir.
Great
@@askchemistryhangout thumb up
Ok
I followed this but unfortunately the titre value I got when thiosulfate is the burette is very small like 7cm3
Then with iodine in the burette I didn't get any reaction,I don't know where I missed it
Chat me on 08100059151
pls are you Peter Obi's brother?
Thanks sir but I think the rough value should never be lower than 1st or 2nd
That’s what my practical gave me.... That’s why it’s better to perform the experiment and not assume
@@askchemistryhangout thanks sir
Great job....
But don't you think the equation for the reaction should be with the hydrated thiosulphate and not the anhydrous...and that will be 4moles of Iodine and 1 mole of the hydrated thiosulphate
It doesn't change anything. If you want to add the water, all you need to do is to add 10H2O at the product side of the equation.
Thanks for the reply 🙏🏻✅God bless You 🙏🏻
Pls can you check again, if a salt is impure, it means it has pure form of it with some impurities. So if what they gave in the question for impure is 12.2g and yiy calculated that of the pure to be 4.52, then tge impure should be 12.2- 4.52. Pls check it again
That’s for percentage impurity
why did you leave the funnel when you adjust the level of sodium thiosulfate?
In as much as the funnel is removed before the titration starts at the initial was carefully checked before the titration... There is no problem about that
You used the volume of the pipette as volume of acid instead of volume of base.
In redox titration there is nothing like acid or base... Kindly take your time to watch the video again to see how the practical and calculations was done ✔️
Pls sir it seems u what you did is for Nigeria students only.How about Ghana students?
I don’t have the instructions sent to Ghana Teachers From Waec .... If You Can Get It Send to Me on +23408100059151.... I will Try and Come Up With Something
Actually I don't have that and getting it will be difficult because most of teacher here don't agree showing to students.So I think getting it will be difficult.Pls just try and do something for us
The molar mass are we to calculate for Na2S2O3 or Na2S2O3.5ho
Na2S203.5H20
Job well done. Please Sir, if you use the specifications from Waec and you have the iodine solution in the burette, add starch solution to the thiosulphate and titrate, there will be color change from colourless to blue-black which is the end point. Though the end point is big.
Have you done the practical or you jus guessing ?
Please what about Ghanaian candidates
I don’t have the instructions that will be sent to your various schools by WAEC.... If You can Get it send it to me on +2348100059151....
Sir it was very helpful what about qualitative analysis
Thanks
This is the link to the qualitative analysis
th-cam.com/video/et2cLiu0540/w-d-xo.html
You are doing well, sir.
Thanks sir🙏🏻 I appreciate your kind words sir
@@askchemistryhangout Good morning sir pls Sir in your calculation of Cb you only calculated the mole pls is it also the same thing as your molar conc. because you used it in finding Ca
@@johnadam1214 I calculated my CB in mol/dm3 and also calculated in amount of moles.... Amount in moles and concentration in mol/dm3 are two different things
@@askchemistryhangout Thank you sir
Sir why did you not calculate the 3 tital value
I confused on how to fill the teacher's report form.
Chat me up on 08100059151
@@askchemistryhangout how do will fill the form
@@adetolakey4229 chat me on 08100059151
Can I use this endpoint in my school because I Don't have the chemicals
If the question indicates that the na2s203 should be in the burette and iodine solution in the conical flask✅ You Can Use that my end point💯 But wait and see what the question is like on that day before deciding on what to do📌
Good
@@askchemistryhangout ok
@@askchemistryhangout Good
@@askchemistryhangout oooi
Is this 2022
Thank you very much sir
God bless u sir
U are very right I used iodine in burrete no results
Some set of people said they used iodine in the burette and changed to blue black 😂 I laugh chemically
@@askchemistryhangout sir, it actually did oh. I did it, but it was exactly 50cm³. I crushed the iodine and poured into a hot KI solution a lot of it dissolved. I however don't think waec would request such procedure that gives such high end point value.
@@uchegodswill397 You Crushed And poured into a hot KI..... The reason why you got 50cm3 means that all the iodine dissolve which is practically impossible without you crushing and increasing the temperature..... I worked it out and got 50cm3 but that is practically not feasible for a titration that you use a 50cm3 burette..... I love your sincerity ✅ Any value lower than 50cm3 to me is not correct because that is the theoretical titre.... I doubt if waec will go that way.....
God bless you so much sir
Abundant knowledge 🙏
Thanks sir , the one I titrated gave me 10.20 can use it for the students
You can since you are sure of your titration ✅
Also sir pls my teachers said that our concordant values should be near 0.20. But yours is exactly 0.20.
Yes he is right .. The one I did was exact because it was done by an experience chemist.... A student might not get exactly
Thank you sir 😊
Is this for 2022????
Yes
But sir, I can't see your writing very well on the board
Am Sorry For That Sir... The camera will be brought more closer in the subsequent ones 🙏🏻
@@askchemistryhangout you can also type it sir
@@pleasantchemistry5962 I will try to do that in my subsequent videos🙏🏻 Thanks sir
Its Ghana part.. Are Ghanaians going to answer the same question bro
Reply me sir
Ghanaian student reached out to me that their waec is September 🤷♂️ I don’t know how true that is ❓
Yes
of are we going to do same titration?
@@askchemistryhangout ooooooo
God bless you
please check on your camera
Noted☑️ Thanks
@@askchemistryhangout please when will you drop another video
@@dailyprayers2001 Next Month By Gods Grace 🙏🏻
@@askchemistryhangout ok thanks
@@askchemistryhangout will you do some before the wassce
start a patron account
Don’t know about this.... Pls kindly chat me up on 08100059151 so we talk better. Thanks 🙏🏻
You have tried so much. Kudos
your writing is not clear
Try to take a close look at it.... It was the camera that was a bit far. Sorry for that
Does one need to boil the starch to prepare it?
How do one prepare starch solution indicator?
@@blessingesther2598 You Boil the water then you poured the starch you have measured inside the boiling water ✅
I wish I had you number sir you are the best teacher I've seen so far
Thanks 🙏🏻 My number is 08100059151
Thank you for this wonderful teaching sir. I'm really greatful.
Sir, pls. Send me your contact
Thanks for your Kind Words🙏🏻 I Appreciate
08100059151
Well done sir pls I need your contact
08100059151
Well done sir. Your effort is appreciated. But I noticed that the mass concentration of iodine you got does not tally with the mass of the reacting iodine in the 25.4 g impure mixture in dm3 according to the calculations you did at the beginning of the video. Does this not matter?
It won’t tally cos all the iodine will neva dissolve in the KI... The mass of the KI given is too small to dissolve the iodine hence a small fraction of the iodine is what will dissolve ✅
@@askchemistryhangout thanks for the reply sir
@@askchemistryhangout thanks for the reply sir