wait for part c, i am confused. If we knew the moles of H+ was 0.0100 and the total volume is 40ml. Couldn't we do Molarity = moles/liter to get 0.0100moles/0.04liter = 0.25M which is the concentration of H+. Since pH is -log(H+) we would get -log(.25) = .60pH not a pH of 7.
No, because all acid moles are consumed by the addition of the base which means that no acid or base moles remain in the beaker/container of the titration leaving only water and neutral salt(since the reaction is between strong acid and strong base the result would be neutral salt and water), therefore, the pH=7
Because, from the question, we have 0.01 moles of HCl, in which will react with 0.01 of NaOH. We'll remain with 0.0001 moles of base. Out of this, you can calculate the pOH-. Remember the pH + pOH = 14
@@Putputnunu hi, wait for part c, i am confused. If we knew the moles of H+ was 0.0100 and the total volume is 40ml. Couldn't we do Molarity = moles/liter to get 0.0100moles/0.04liter = 0.25M which is the concentration of H+. Since pH is -log(H+) we would get -log(.25) = .60pH not a pH of 7.
![Noob To Max With DRAGON REWORK In Blox Fruits [FULL MOVIE]](http://i.ytimg.com/vi/LnBMOinoOvA/mqdefault.jpg)
wait for part c, i am confused. If we knew the moles of H+ was 0.0100 and the total volume is 40ml. Couldn't we do Molarity = moles/liter to get 0.0100moles/0.04liter = 0.25M which is the concentration of H+. Since pH is -log(H+) we would get -log(.25) = .60pH not a pH of 7.
i dont think this would work at the end bc we reacted all our H+ We have an excess at beyond the end point
No, because all acid moles are consumed by the addition of the base which means that no acid or base moles remain in the beaker/container of the titration leaving only water and neutral salt(since the reaction is between strong acid and strong base the result would be neutral salt and water), therefore, the pH=7
good videos thanks
If the solution was naturalised in the previous question, why is 0.0100M H3O being deducted from 0.0101OH-?
because you added in excess base to pass the equivalence point
Why we use 0.0001 mole of base to calculate For pH solution?
Because, from the question, we have 0.01 moles of HCl, in which will react with 0.01 of NaOH. We'll remain with 0.0001 moles of base. Out of this, you can calculate the pOH-. Remember the pH + pOH = 14
@@Putputnunu well i mean water also has ph too why they won't count them?
@@donuts2786 Because water is considered Neutral.
@@Putputnunu thanks
@@Putputnunu hi, wait for part c, i am confused. If we knew the moles of H+ was 0.0100 and the total volume is 40ml. Couldn't we do Molarity = moles/liter to get 0.0100moles/0.04liter = 0.25M which is the concentration of H+. Since pH is -log(H+) we would get -log(.25) = .60pH not a pH of 7.
can you put a link to the previous video on here?
ruclips.net/video/JoGQYSTlOKo/видео.html
at part c why isnt the OH- moles that are found subtracted from the moles of acid that was left from part b??
you made an error you should have subtracted the 20.2 from 20 to get the amount that you have over shot the equivalence point by
Akeem Snave that's not an error he chose to use the long method
Whereas your method is the shorter one
Lightning McQueen? Is that you?
why this mans sound like remy from ratatoullie
great vid tho super helpful