Acid-Base Titration

[@BebeZaharasBeignets]

Professor Dave, you’re a lifesaver. If I get accepted for transfer at my dream university, graduate, then have the life I’ve always wanted I want you to ordain my wedding.

[@TheNaikas]

Did you?

[@omarqacle]

@@TheNaikas its been a year how he finna do all that in this amount of time

[@jubileej1629]

@@omarqacle girl u neva know

[@marcus9441]

Update us

[@GrandTheftAut0]

u marry yet?

[@vanityromano3748]

I want to cry with joy at how easily you explained this, thank you for alleviating a huge frustration!!!

[@elizabethcolon3181]

If you were my real professor i'd have 105 in chem you explain so well give great examples and you make sure we understood what you showed us by making us do an exercise ourselves. What great way of teaching!

[@NoviProleterijat]

@Usern Last You are right! However this is not equal for children or I should rather say not for EVERY child. Guidance is important until a child matures and so the teacher can be a strong factor in the students success.

[@chemistrywithcoffee1381]

In my 13+ years of experience, I can tell you that some students need more support than the others. World is not fair! But we can make it work by publishing quality videos for the needed.

[@PunmasterSTP]

Hey I know it's been years, but I just came across your comment and was curious. How have your studies been going?

[@ivoryas1696]

@@chemistrywithcoffee1381 You know, that's pretty fair.

[@marcusayala6933]

@@chemistrywithcoffee1381 That's equity, not equality

[@hamzamalik8925]

Brilliant teaching. Really appreciate the thought and effort made into making these videos.

[@JasonChanMarioKartProPlayer]

Molarity times Volume (MV)before titration= MV after titration 75/1000 x 0.5 = 165/1000 x M M= 0.2272727... This also worked and my teacher told us to use this method

[@educationalaccount5963]

But only for monoprotic substances

[@blinkeverlast718]

i think this only works with niche acid-base titrations? along with dilution problems - c1v1=c2v2

[@cheddar6020]

Coincidence. Only true when the stoichiometric ratio is 1:1 In fact, his video mistakes this when H2SO4 reacts with NaOH

[@pasdpasse439]

@@cheddar6020 It is just an example dude, however I am curious, why wouldn't it react? If I remember correctly, they both are soluble

[@wamakamutale4123]

Assuming 1:1 molar ratio. If we balance the equation it's 1:2 giving us 2.784M

[@rokotrstenjak1895]

you forgot to do molar ratio for the first problem. you should've multiplied the moles of H2So4 by 2 due to the 1:2 ratio. Thank you

[@kamogelomokale9183]

I was also thinking the same thing

[@rucio1118]

agreed

[@yuiii1193]

Wait, did I just finally understand the topic in under 2 minutes and 40 seconds? Yes. Thank you so much prof Dave! You made it so much easier to understand!

[@beckya.9594]

Thank you for NOT over complicating your explanations. 🙏🏽

[@rohmanjakarta9732]

On the example, the mol of base should be two times the acid so the mol of base is 0.0696

[@meganxu5475]

i want the 5 hour version of the jingle

[@yukitai9063]

Imagine a yr12 chemistry class in Australia watching someone from the United States.

[@kburishkin]

Your videos are great...I recommend my students to view them quite often. However, in this case it may have been better to use a monoprotic acid in the example...

[@incognito7575]

Yes, this is my concern too.

[@lottajarvi476]

Thank you so much, your videos have been super helpful as I have been studying for my big chemistry exam!

[@ProfessorDaveExplains]

my pleasure! you can do it!

[@dragon.fromindia3235]

SELL GOLD AND SILVER BUY PLATINUM PRICE IS LOW NOW PROMOTE PLATINUM PRICE IS RISING LIKE GOLD....

[@AmanSharma-xz8nz]

Sir your video was very helpful I understood everything I wish that u were my chemistry teacher

[@rosieleaverton]

I was stressing really bad over my homework because the other resources my teacher gave weren't helping, but your video made it so incredibly clear. Thank you!!

[@kripashankarshukla4073]

Sir your theme song and your explanation both are the best.

[@aionioshagiazo]

Hi Prof. Dave, I have a question: Should we not consider the balanced equation of Sulfuric acid and Sodium Hydroxide when we do the calculation? The ratio of acid/base should be 1:2, then the mole of base should be 0.0348 x 2 = 0.0696...please advice thanks!

[@ProfessorDaveExplains]

it's only strongly acidic for the first proton

[@aionioshagiazo]

@@ProfessorDaveExplains Thanks! I am doing Cambridge Chemistry A/AS level review presently... from the other references I gathered, it's a general rule to consider the balanced equation. But I guess, it depends on the curriculum not sure.

[@icduay4957]

@@ProfessorDaveExplains Hi Dave, I love your videos because they're very easy to follow. I would just like to correct this one. It is true that sulfuric acid is strongly acidic for the first proton, but that is relative to water acting as a weak base. In this case, you have a strong base, NaOH, reacting with H2SO4. It is strong enough to ionize the second proton, so the ratio is 1 NaOH : 2 H2SO4. Another example would be titration of acetic acid, a weak acid, to a strong base. You can still remove the proton from the acetic acid even if it is weakly acidic.

[@fasc2298]

@@ProfessorDaveExplains At a glance it seems that the 3.0 M sulfuric acid also as 3.0 N sulfuric acid. but Sulfuric acid is easily deprotonated twice by NaOH, so it is 3.0 M but 6.0 N. Therefore the NaOH would actually be 1.39x2 M. pKas are -2.88 and 1.99. while the second proton is not strongly acidic, its still easily deprotonated by the strong base NaOH. Otherwise would be like saying Acetic acid pKa = 4.75 is not deprotonated by NaOH because its the first is a weak acid... Treating 1M H2SO4 as 1N H2SO4 can have catastrophic consequences :s I also second IC Duays comment.

[@raphaelschiess4283]

@@ProfessorDaveExplains The second proton (the one of Hydrogensulfate) will still react with the hydroxide anions in the solution. Thus, the stochimetric factor of 2 has to be taken into account.

[@tunistick8044]

breef, 1/a.n(titrator)=1/b.n(titratee), such that the formula of both the titrator and the titratee is a.titrator and b.titratee

[@lucasvdb981]

This is exactly what I was looking for, tysm!

[@hanyanhavall3984]

Thenk you professor you saved my life i was having a seminar and i got 10/10❤️

[@yanapat345]

thanks pookie i missed like a week of school and didn’t even understand this lab

[@TheSecretBuster]

You are my go-to channel for chemistry help! Keep making content they're really informative and helpful! In the future videos, can you please make some on organic chemistry? Such as naming and drawing hydrocarbons in functional groups, or anything related to organic chem. Thank you and keep doing what you do best!

[@ProfessorDaveExplains]

+TheSecretBuster my friend, i have an entire organic chemistry playlist! 38 clips. check it out.

[@TheSecretBuster]

Professor Dave Explains Oh haha just saw them, sorry for the confusion.

[@arihantjain2845]

50 ml of a solution which is 0.050 M in the acid HA (pka = 3.80) and 0.10 m in HB (pka = 8.20) is a titrated with 0.2 M NaOH. calculate the pH at the first equivalence point, and second equivalence point. Please explain such question including this!

[@nuhiyaather9552]

Thanq sir u make the concept very easy to understand with in short time

[@Maddie05007]

For real i couldnt get this concept this clearly anywhere else.🎉🎉

[@PunmasterSTP]

Acid-base titration? More like "This is amazing information!" Thanks for sharing another very high quality video.

[@andrewjustin256]

1:40 Mr. Dave, perhaps you missed the point on using the stoicheometrical ratios. Besides you did not even balance the equation. Have a look at this: 2NaOH + H2SO4 ---> 2H2O + Na2aSO4 That implies you had to multiply 0.0348mol with 2, then divide with its volume. Because we need 2 miles of the base to neutralize just 1 mole of the acid, suggesting the resilience of the acid. So, 0.0348mol×2= 0.0696mol Then 0.0696mol/0.025L = 2.784M

[@sekhar9479]

that was quite helpful,keep on making such videos

[@matthewgeistfeld4035]

How is that first math example a 1:1 mole ratio? Wouldn't balancing the equation between the acid and base result in a 1:2 ratio between sulfuric acid and sodium hydroxide? H2SO4 + 2 NaOH --> 2H2O + Na2SO4 Thus making the answer half of what you have listed...

[@ProfessorDaveExplains]

+Matthew Geistfeld it's true i maybe should have used a monoprotic acid, but the Ka for the second ionization for sulfuric acid is tremendously smaller than the first, so it's not at all the same as considering it to be twice the volume of acid.

[@incognito7575]

Thanks!

[@eddiekim2475]

Professor Dave Explains I understand this but googling other examples of this same problem they do a 1:2 ratio. Why is that?

[@faithjohnson6649]

How did you get the 11.6mL??

[@A-Silver]

hard carry after 8 years, thank you so much!

[@ishkil]

I thought the stoichiometric ratio of H2S04 to NaOH is 1:2. why is the moles of acid equal to the moles of base? I'm confused about the conversion part can you pls clarify. thanks!

[@nickolasspagnolo7304]

I think he just made a mistake, I found ratio is 1:2 also.

[@JakeArnet]

Very helpful. Thank you for the clear explanation Professor Dave!

[@dustindusterooni3601]

Thanks dave

[@missygarrett1338]

One more thing, maybe include the balanced chemical equation too as part of the solution to the proposed problem. :-)

[@lanomusambazi8654]

I think so too because the stoichiometrical mole ratio in the example for NaOH and H2SO4 is 2 to 1 when the equation is balanced. Therefore the solution should have been 2.784M and not 1.39M.

[@lesnerchai2186]

TRUE, the ans is wrong

[@chennnpai]

It’s so much clearer now that I have gotten your explanation, thank you!

[@FatimaHassan-mj8hr]

Thank you, it is really useful

[@archiesomaiya]

You are wrong. Conc of naoh is 2.784 since it's a 1:2 ratio

[@emlmm88]

Also, next semester I'm supposed to take Physical Chemistry. If possible, videos on that would be greatly appreciated.

[@bennettegaper4344]

Thank you

[@Shykai449]

W you just dropped the exact answer for what i'm gonna need to do for my lab

[@missygarrett1338]

Great video but would you please consider updating the graphics to show the proper glassware (change the beaker to an Erlenmeyer Flask) since you need to swirl to mix.

[@ProfessorDaveExplains]

you can do it with a beaker and a magnetic stir bar, actually that's the most common way since it allows for constant stirring

[@missygarrett1338]

@@ProfessorDaveExplains but even then the flask is preferred.

[@opufy]

I like that method, but I just used good ole c1v1=c2v2

[@chemistrywithcoffee1381]

I liked the all the video but especially the backgrounds!!!

[@alva9690]

FINALLY IVE FOUND CHEMISTRY JESUS!

[@mabiakamal9322]

Really good

[@SimplyyBravo]

its 2am and im on campus a day before the exam but im patting myself on the back for getting the comprehension problem right haha

[@xamaadashnuur1648]

Thank u prof u save my day

[@allieharuu7308]

Aside from indicators, how could we determine the endpoint of acid-base titrations?

[@mattkrier5856]

THANKS FOR HELPING ME MAKE BIODIESEL

[@qweboss8784]

Iam thinking that 1 mole of H2SO4 reacts with 2 mole of NAOH

[@sheepmasterrace]

Shouldn’t you times 2 because there are 2 moles of NaOH for every H3SO4? why isn’t this the case?

[@OriganalSEX]

professor shouldnt the first example oh H2SO4 + NaOH result with 2.784 M since the H2SO4 is diaprotic?

[@endjess4857]

Thank you for helping me understand this💕

[@syedahmed3136]

For NaoH concentration the volume should be (.0116+.025) L not .025L.

[@cheddar6020]

concentration before the titration.

[@ruisir1]

shouldn't it be 0.0696 mol base?

[@ProfessorDaveExplains]

even though its a diprotic acid, the second proton is nowhere near as acidic as the first, so we are just looking at neutralizing the results of the first deprotonation.

[@cheddar6020]

@@ProfessorDaveExplains It's 98% as acidic and a balanced reaction will consider both protons.

[@lanomusambazi8654]

Thank you professor Daves

[@IsaacAwad.04]

Why i don't understand the will neutralizer 1:58

[@Scr1ball]

professor dave i’m in love with you

[@diwakarpatel2051]

Sir You are the best teacher

[@crieliocriel]

i thought the ratio of naoh to h2so4 is 2:1.. from the equation..

[@eliashospers4184]

thank you master dave

[@rassimsimou1594]

Good

[@PartyRick25]

Thanks Professor Dave!

[@rainsmush]

pls make on Arrhenius,Bronstein and lewis concept literally need it

[@ProfessorDaveExplains]

check my video on acids and bases

[@estelamino6356]

THANKS

[@pagodnako]

Thank you papa susej🙌🏻

[@salvy2896]

Why 11.6ml ???

[@sicilianotoronto]

I did M1V1 = M2V2, solved for M2, got the same answer.

[@vatsalyatiwarii]

Thanks for the formula

[@TheHHPodcast]

should it not be 4 significant figures? the 165.0 had 4

[@rylietaylor8208]

You're my literal lord and savior thank you so much

[@user-hu1gy2de2u]

I want to knowWhat are three attributes of a successful titrimetric analysis?

[@boashoe]

This man is saving my degree 😭

[@atharyalajmi670]

you're a lifesaver​

[@omaralslamen]

Thank you But can u talk about neutralization titration Pls

[@ZeonGenesis]

I still can't fathom how we know when we reach an equivalence point with an indicator, all I get is we just make it change color.. ach.

[@Antweezy]

Agh, the prof wants us to answer concentration of .1M NaOH (which is being titrated INTO KHP soln), how can we do this? It doesn't make sense to figure out M of NaOH instead of M of KHP.

[@amnaataha]

1:35 why is the mol ratio for stoichemetry 1 to 1? Isn't it supposed to be 1:2

[@jacipope8289]

I'm not an expert by any means, so don't listen to closely to me, but I THINK it depends from substance to substance. The different solutes and solutions have different ratios. (Not 100% sure though, don't @ me if I'm wrong pls)

[@willm3027]

You don’t worry about coefficients in molarity. As long as you do Molarity = moles/ liters. If you solve molarity by m1v1= m2v2 then you do worry about coefficients. Don’t use the second method. You’ll be wrong.

[@roxyta182]

Thank you!

[@user-by9xx2rz5z]

watching before my chemistry exam

[@tushhaardesai]

Excellent

[@harishbaghel7263]

Sir I would like to ask as to why the graph of volume of base vs pH is a curve not a straight line??

[@ProfessorDaveExplains]

logarithmic relationship!

[@4m0d]

EPIC VID PROFESSOR

[@joelsksksk7500]

Whats the different between acid-base titration and acidimetry?

[@hrishirachchh1947]

Sir you are like ranbir kapoor.

[@HargunKaurSandhuHargun]

Bro what where did animal come from? 😂

[@emlmm88]

How many tags do you put on your videos? The quality of them is so often exceptional that something seems amiss.

[@nawalzahra3612]

You are so good 😊 thanku

[@vicgervemarlang5181]

is the 3.0m H2SO4 the indicator?

[@michaelmancano]

Brilliant

[@imosdefinite]

On a titration curve, is base always on the x axis?

[@MerlinsFury]

Brother, the stoichiometric ratio is not 1:1 for NaOH and H2SO4...

[@elianeshantalliendoenciso8572]

hi teacher , why 11.6??? please

[@hephaestus5521]

Why is the conversion factor mol/1L why isnt it 22.4? Pls help

[@ProfessorDaveExplains]

That's for ideal gases.

[@pullagurlayoganandreddy7683]

wait.....how acid and base can be together they just react right!

[@captaininsane1893]

What topic are the calculations from that confused me slightly

[@cloudwalker2730]

When you try to find the point of inflection of the graph......

[@chocolatestrawberry5491]

yes!!!! calculus>chemistry

[@earthtoaquila]

I get it but why is it that sometimes you change the volume of the acid to liters and sometimes you leave it as mLs? I googled a few of my practice questions and the way you do it here gives me a different answers than what I find online. Can M also be equal to mol/mL or only mol/L

[@ProfessorDaveExplains]

M is mol/L, it's just that for certain calculations volumes in mL are ok

[@shalomagutierrez5710]

wow you look just like Nicholas Megalis

[@mow7da7777]

Easy and perfect - kuwait

[@nhenry621]

Professor Dave, Do you have videos for biochemistry?

[@ProfessorDaveExplains]

+Nicole Henry those will be coming soon! probably over the summer.

[@nhenry621]

omgg yes please!!! i finish organic this semester and I am scared for biochem

[@handsomemonkeyking5299]

Wow.. So my university just stretched this simple concept out to a 45 minute explanation AND made it unnecessarily confusing.

[@huangyipeng1108]

Gigachad teacher