an absolute legend , we have this practical on friday and i was so confused due to how the teacher was explaining it , and now i fully understand it thank you so much 🙏🏿💯
hii there, i really enjoyed this experiment. it is very useful, i will be making my lab practical soon. it is about types of titration with some other experiments.
Can you please help me with this ❓ A 1.2034grams sample was titrated with 0.5324M HCl, with phenolphthalein as indicator. The solution turned colorless after the addition of 25.6ml of the acid. Methyl orange was then added and a volume of 0.3ml more of the acid was required for the color to change to pink. Determine the identity of the sample and its percent purity.
In the final calculations at 8:16, there is a discrepancy between the results of Step 3 and Step 4. Step 3 says that 0.0135 mol of NaOH(aq) is required for the solution to reach the end-point. According to Step 4, mole ratio of NaOH to HCl is 1:1. Therefore, shouldn't Step 4's result also be '0.0135 mol' (same as Step 3) instead of "0.135 mol"?
Correct me if I'm wrong, but I don't think that this method works. The endpoint of the phenolphthalein indicator is over pH 8. So how are you determining the moles of NaOH that were necessary to neutralize the remaining HCl? That solution is basic, not neutral, so aren't the moles of NaOH in that solution higher than was necessary to neutralize the acid?
how can i calculate the concentration of the reagents with a known - concentration (HCl and NaOH)? is there a certain amount of concentration for them which is special for every back - titration setup?
Yes, firstly, you calculate the amount of HCl UNREACTED; then, using the initial amount of HCl added, you can calculate the amount of HCl REACTED. After that, by considering the mole ratio of Al(OH)3 : HCl, you can work out the amount of Al(OH)3 present in the tablet.
Why 0.135 is the number of the moles of HCL remain unreacted? Isn’t it should be 0.0135? I am sorry, I just not really good with chemistry. Preparing for my exam now.
![Lab: Back titration to determine the % CaCO3 in eggshell DATA COLLECTION [IB CHEMISTRY]](http://i.ytimg.com/vi/DjBXw7toD_0/mqdefault.jpg)
an absolute legend , we have this practical on friday and i was so confused due to how the teacher was explaining it , and now i fully understand it thank you so much 🙏🏿💯
so straight to the point and easy to understand. thank you
This video helped me so much!! Keep it up! I recommend writing down the experiment and uploading that with the video as it will be more helpful
This video is absolutely amazing! It helps me to understand back titration thoroughly. Thank you so much!
great video, very helpful to students revising and needing guide with reverse titration. also providing all the significant background information
That's a very superb experiment.... Great work 💞
hii there, i really enjoyed this experiment. it is very useful, i will be making my lab practical soon.
it is about types of titration with some other experiments.
this is part of my assignment and honestly had no clue as to how to start it but he explained it perfectly
Good work....I am solidly matching behind you....making chemisty interesting
Thank you so much!
Can you please help me with this ❓
A 1.2034grams sample was titrated with 0.5324M HCl, with phenolphthalein as indicator. The solution turned colorless after the addition of 25.6ml of the acid. Methyl orange was then added and a volume of 0.3ml more of the acid was required for the color to change to pink. Determine the identity of the sample and its percent purity.
It was #amAZING#
And good to watch ☺️
Thank you so much,😊😊😊
tysm u saved me
simple and easy to understand
In the final calculations at 8:16, there is a discrepancy between the results of Step 3 and Step 4.
Step 3 says that 0.0135 mol of NaOH(aq) is required for the solution to reach the end-point.
According to Step 4, mole ratio of NaOH to HCl is 1:1. Therefore, shouldn't Step 4's result also be '0.0135 mol' (same as Step 3) instead of "0.135 mol"?
you are right
Very nice 😃
👍 i have an exam for this lmao
But..... Please tell me the calculations process.. I can't understand by just seeing photo
Well taught 👌👌😀
Such an help in lockdown when we cant physically perform anything unfortunately
so coool
Correct me if I'm wrong, but I don't think that this method works. The endpoint of the phenolphthalein indicator is over pH 8. So how are you determining the moles of NaOH that were necessary to neutralize the remaining HCl? That solution is basic, not neutral, so aren't the moles of NaOH in that solution higher than was necessary to neutralize the acid?
how can i calculate the concentration of the reagents with a known - concentration (HCl and NaOH)? is there a certain amount of concentration for them which is special for every back - titration setup?
The concentrations and volumes are suggested by the laboratory manual.
how does the calculation work? Is the purpose of the calculation to work out how much there is excess of hcl?
Yes, firstly, you calculate the amount of HCl UNREACTED; then, using the initial amount of HCl added, you can calculate the amount of HCl REACTED. After that, by considering the mole ratio of Al(OH)3 : HCl, you can work out the amount of Al(OH)3 present in the tablet.
Why 0.135 is the number of the moles of HCL remain unreacted? Isn’t it should be 0.0135?
I am sorry, I just not really good with chemistry. Preparing for my exam now.
Hi Vera, it was a typo and yes it should be 0.0135, thanks for pointing that out. The final answer is correct tho.
Did you use 0.1M NaOH solution?
It was 0.451M NaOH, you can refer to the calculation part at the end of the video.
Experiment of double indicator titration