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Chemistry questions

  • 29-05-2013 8:22pm
    #1
    Closed Accounts Posts: 1,696 ✭✭✭


    Hey guys,
    So does anyone know why the acid is placed in the burette rather than the base? I can't seem to recall it and It's not in the notes :)


Comments

  • Registered Users, Registered Users 2 Posts: 10 Hazardous Garden Of Eden


    A lot of bases (like NaOH) would attack the glass etc..
    and cause the tap to stick.

    Hells bells...


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    A lot of bases (like NaOH) would attack the glass etc..
    and cause the tap to stick.

    Hells bells...

    Okay. Thanks a lot! :D


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    2001 Hl
    Sodium carbonate is not a Primary standard but anhydrous sodium carbonate is. why is this the case?


  • Registered Users, Registered Users 2 Posts: 10 Hazardous Garden Of Eden


    2001 Hl
    Sodium carbonate is not a Primary standard but anhydrous sodium carbonate is. why is this the case?

    Sodium carbonate cannot be prepared in a 100% pure, stable and soluble solid form so that it can be weighed out and readily dissolved in water to provide a solution of accurately known concentration, but the anhydrous can.

    Or something to that effect.


  • Posts: 0 [Deleted User]


    2001 Hl
    Sodium carbonate is not a Primary standard but anhydrous sodium carbonate is. why is this the case?

    As sodium carbonate cannot be made up into a solution of known concentration as we don't know the degree of hydration which implies we can't know the Molarity of the solution we make.


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  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Thanks guys!
    another question: examinations.ie seems to be down so I can't look up the Marking but I'll post the q here.
    washing soda
    2.51g washing soda dissolved made up to 250cm^3. Molarity found by titrating 25 of this against 0.1 HCL. Mean titre is 20.
    okay so i calculated the concentration to be 0.05m/l
    the value of X wont work out for me?? Can ye try this?


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Sodium carbonate cannot be prepared in a 100% pure, stable and soluble solid form so that it can be weighed out and readily dissolved in water to provide a solution of accurately known concentration, but the anhydrous can.

    Or something to that effect.

    The exact wording was this: Na2CO3XH20 is not a ps but NA2CO3 may be used as a PS. why is this the case?
    Are they asking why is NA2CO3 A ps?


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Thanks guys!
    another question: examinations.ie seems to be down so I can't look up the Marking but I'll post the q here.
    washing soda
    2.51g washing soda dissolved made up to 250cm^3. Molarity found by titrating 25 of this against 0.1 HCL. Mean titre is 20.
    okay so i calculated the concentration to be 0.05m/l
    the value of X wont work out for me?? Can ye try this?

    Actually it's okay. I got it! Had the m/l wrong! :P
    I thought that the mass was always 286? no?
    also why am i quoting myself? :P


  • Posts: 0 [Deleted User]


    Thanks guys!
    another question: examinations.ie seems to be down so I can't look up the Marking but I'll post the q here.
    washing soda
    2.51g washing soda dissolved made up to 250cm^3. Molarity found by titrating 25 of this against 0.1 HCL. Mean titre is 20.
    okay so i calculated the concentration to be 0.05m/l
    the value of X wont work out for me?? Can ye try this?

    25x/1 = 20(0.1)/1
    x = 2/25 = 0.08M

    0.08 in 1L = 0.02 in 250cm^3

    2.51/0.02 = 125.5 - 106 (rmm of washing soda) = 19.5/18 = 1x?

    That doesn't sound right at all but I'm doing it all from memory sorry


  • Posts: 0 [Deleted User]


    Actually it's okay. I got it! Had the m/l wrong! :P
    I thought that the mass was always 286? no?
    also why am i quoting myself? :P

    Could you post your solution please?!


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  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Could you post your solution please?!

    m1v1/n1 = m2v2/n2
    ie. 20(0.1)/2 = 25m1/1 then cross multiply giving you M1 as 0.04m/l

    then you say 0.04m/l thus 0.01m/250
    so 0.01m liberates 2.51g
    1m liberated ?
    2.51/0.01 giving you 251 grams.
    NA2CO3XH20 = 251
    106 + 18X= 251
    X= 8.1


  • Closed Accounts Posts: 3,479 ✭✭✭ChemHickey


    m1v1/n1 = m2v2/n2
    ie. 20(0.1)/2 = 25m1/1 then cross multiply giving you M1 as 0.04m/l

    then you say 0.04m/l thus 0.01m/250
    so 0.01m liberates 2.51g
    1m liberated ?
    2.51/0.01 giving you 251 grams.
    NA2CO3XH20 = 251
    106 + 18X= 251
    X= 8.1

    Don't forget that the substance could be effloresced and have lost some water to the atmosphere. It's a trick the Chief Examiner could/probably will throw in sometime {again} just because everyone, yourself included, is so used to working with 10 and whole numbers like that which are used in every example. It was one thing our teacher made us look out for and had us ready to answer a question on.

    If it comes up on the paper as an answer like that (an answer not equal to 10 or the normal w.o.c) a follow-up question could easily be "Give a reason for your result in the previous part"

    Ans: The substance has lost some water (effloresced) to the air/atmosphere and therefore the water of crystallisation is lower than expected.


  • Posts: 0 [Deleted User]


    m1v1/n1 = m2v2/n2
    ie. 20(0.1)/2 = 25m1/1 then cross multiply giving you M1 as 0.04m/l

    then you say 0.04m/l thus 0.01m/250
    so 0.01m liberates 2.51g
    1m liberated ?
    2.51/0.01 giving you 251 grams.
    NA2CO3XH20 = 251
    106 + 18X= 251
    X= 8.1

    I knew I had the stoichiometry wrong!


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    ChemHickey wrote: »
    Don't forget that the substance could be effloresced and have lost some water to the atmosphere. It's a trick the Chief Examiner could/probably will throw in sometime {again} just because everyone, yourself included, is so used to working with 10 and whole numbers like that which are used in every example. It was one thing our teacher made us look out for and had us ready to answer a question on.

    If it comes up on the paper as an answer like that (an answer not equal to 10 or the normal w.o.c) a follow-up question could easily be "Give a reason for your result in the previous part"

    Ans: The substance has lost some water (effloresced) to the air/atmosphere and therefore the water of crystallisation is lower than expected.
    Just seen it in my notes there haha.
    thanks for the tip on the follow up question! ;)


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    I knew I had the stoichiometry wrong!

    haha my explanation is diabolical


  • Posts: 0 [Deleted User]


    haha my explanation is diabolical

    I understood completely :)
    Just a quick question, does anyone remember doing redox titrations of group 7 elements? I don't and if they come up as q1 well then I'm ****ed for that q


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    I understood completely :)
    Just a quick question, does anyone remember doing redox titrations of group 7 elements? I don't and if they come up as q1 well then I'm ****ed for that q

    hm? what you on about? there's vinegar, washing soda, hardness ;), DO, ammo iron, iron tab, sodimum thio, bleach


  • Posts: 0 [Deleted User]


    hm? what you on about? there's vinegar, washing soda, hardness ;), DO, ammo iron, iron tab, sodimum thio, bleach

    Hm sorry, redox reaction, not titration.
    (a) Redox reactions of group VII elements (b) Displacement reactions of metals
    Still doesn't ring any bells :pac:


  • Closed Accounts Posts: 3,479 ✭✭✭ChemHickey


    I understood completely :)
    Just a quick question, does anyone remember doing redox titrations of group 7 elements? I don't and if they come up as q1 well then I'm ****ed for that q

    They aren't titrations, they're just a set of experiments to show reduction/oxidation and how good of oxidising agents the halogens are and to show how they become better oxidising agents as you go up the periodic table (F > Cl as an oxidising agent)


  • Posts: 0 [Deleted User]


    ChemHickey wrote: »
    They aren't titrations, they're just a set of experiments to show reduction/oxidation and how good of oxidising agents the halogens are and to show how they become better oxidising agents as you go up the periodic table (F > Cl as an oxidising agent)

    Yeah my friend read it wrong from his book and was talking to me on the phone sorry :P


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  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Hm sorry, redox reaction, not titration.
    (a) Redox reactions of group VII elements (b) Displacement reactions of metals
    Still doesn't ring any bells :pac:

    ah yeah get it now! oh i hate them! :/


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    I have another few questions on water of crystallisation.
    1 why would a standard solution of ethanoic acid not be suitable for this titration?
    2 suggest a suitable base for standardisnig H2SO4?
    3 why was the titration flask ONLY rinsed with deionised water and not with the sol. it is to contain?


  • Registered Users, Registered Users 2 Posts: 1,049 ✭✭✭CookieMonster.x


    I have another few questions on water of crystallisation.
    1 why would a standard solution of ethanoic acid not be suitable for this titration?
    2 suggest a suitable base for standardisnig H2SO4?
    3 why was the titration flask ONLY rinsed with deionised water and not with the sol. it is to contain?

    2. Na2co3 I think
    3. Because if you rinsed it with the soln you would have an unknown volume on the flask and there would be a change in the number of moles reacting.


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    2. Na2co3 I think
    3. Because if you rinsed it with the soln you would have an unknown volume on the flask and there would be a change in the number of moles reacting.
    Thanks! you don't kniw when amm fe+2 sulphate is used to standardise do u?
    also, yiu dont have the answer to 1 no? :)


  • Registered Users, Registered Users 2 Posts: 1,049 ✭✭✭CookieMonster.x


    Thanks! you don't kniw when amm fe+2 sulphate is used to standardise do u?
    also, yiu dont have the answer to 1 no? :)

    It's used to standardise potassium permanganate :)
    I'm not sure about q1 but I would guess that it could be because HCl is a strong acid whereas ethanoic acid is a weak acid and it wouldn't react properly? Not too sure so don't take my word for it! :P are these from exam papers?


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    It's used to standardise potassium permanganate :)
    I'm not sure about q1 but I would guess that it could be because HCl is a strong acid whereas ethanoic acid is a weak acid and it wouldn't react properly? Not too sure so don't take my word for it! :P are these from exam papers?
    okay brilliant thanks! :) they are from the 80's/70's :)


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Okay so I have a Water of crystalisation question from the 1995 paper. I think I have it but as there's no marking scheme, I need to be sure. so if anyone could do it and post the answer it would be brilliant!
    7.77g NA2CO3XH20 was made up to 500cm^3. 25cm was titrated agaainst 0.075 molar h2so4. average titre is 20. ratio is 1:1.
    a) conc of na2co3xh20 in g dm^-3
    b) in mol dm^-3.
    c) hence find the % water in sodium carbonate crystals and the value of X.
    My answers are: a) 15.54 g/l,,, b) 0.06 and c) 59% with x being 8.5. is this right? :(


  • Registered Users, Registered Users 2 Posts: 306 ✭✭chatterboxxx95


    Outnumbered , your q 1 is because ethanoic acid is a weak acid and no indicator would be suitable to show the endpoint :P


  • Closed Accounts Posts: 1,696 ✭✭✭outnumbered


    Outnumbered , your q 1 is because ethanoic acid is a weak acid and no indicator would be suitable to show the endpoint :P

    Why thank you Chatterboxxx95 ;)


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