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how to work out molarity?? watch

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    say of ethanol, if you're given the volume and the concentration? u have to find density? say ethnoal mixed with water
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    (Original post by neverbeejail)
    say of ethanol, if you're given the volume and the concentration? u have to find density? say ethnoal mixed with water
    What exactly is your question? :fluffy:
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    (Original post by Neuth)
    What exactly is your question? :fluffy:
    say u have 5ml 50% ethanol and in a solution its 1.000ml mineral water and 0.500 ethanol plus 0.5ml yeast how the hell do u do it i know u need to find density of ethanol
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    Please can someone else double check my answer.

    (Original post by neverbeejail)
    say of ethanol, if you're given the volume and the concentration? u have to find density? say ethnoal mixed with water
    (Original post by neverbeejail)
    say u have 5ml 50% ethanol and in a solution its 1.000ml mineral water and 0.500 ethanol plus 0.5ml yeast how the hell do u do it i know u need to find density of ethanol
    moles = mass/molar mass or moles = concentration x volume (in dm3)
    Google says density = mass/volume (remember Google is your friend.)

    I presume volume would be 2.5ml because it's 50% of 5ml.
    As you divide 1cm by 1000 to get dm3, I guess to get dm3 for ml I'd have to divide by 100.
    So moles = concentration x volume (in dm3), so moles = 0.500mol dm-3 x 0.0025dm-3 = 0.00125 moles.

    Rearranging the moles = mass/molar mass equation gives us
    mass = moles x molar mass
    Ethanol is C2H6O
    mass = 0.00125 x (24 + 6 + 16)
    mass = 0.0575g

    So density = mass/volume (in cm3)
    So density = 0.0575g / 0.25cm3
    Spoiler:
    Show
    You probably don't need to know yet, presuming you're beginning AS.

    ethanol
    eth- denotes two carbons,
    -an- denotes only single bonds,
    -ol is the suffix for the -OH group.
    A carbon can only have 4 bonds and be stable.
    So structural formula is CH3CH2OH
    Molecular = C2H6O
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    someone please double check his answer
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    Havent checked the maths but the chemistry is solid ^^
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    (Original post by XcitingStuart)
    Please can someone else double check my answer.





    moles = mass/molar mass or moles = concentration x volume (in dm3)
    Google says density = mass/volume (remember Google is your friend.)

    I presume volume would be 2.5ml because it's 50% of 5ml.
    As you divide 1cm by 1000 to get dm3, I guess to get dm3 for ml I'd have to divide by 100.
    So moles = concentration x volume (in dm3), so moles = 0.500mol dm-3 x 0.0025dm-3 = 0.00125 moles.

    Rearranging the moles = mass/molar mass equation gives us
    mass = moles x molar mass
    Ethanol is C2H6O
    mass = 0.00125 x (24 + 6 + 16)
    mass = 0.0575g

    So density = mass/volume (in cm3)
    So density = 0.0575g / 0.25cm3
    Spoiler:
    Show
    You probably don't need to know yet, presuming you're beginning AS.

    ethanol
    eth- denotes two carbons,
    -an- denotes only single bonds,
    -ol is the suffix for the -OH group.
    A carbon can only have 4 bonds and be stable.
    So structural formula is CH3CH2OH
    Molecular = C2H6O
    mate i cant get standard deviation if i didnt do repeat tests of the experiment right?
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    (Original post by neverbeejail)
    mate i cant get standard deviation if i didnt do repeat tests of the experiment right?
    I'm pretty sure you can, as standard deviation just shows the variation in data about the mean (I think.)
    You can get a mean from just one set of data.
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    (Original post by XcitingStuart)
    I'm pretty sure you can, as standard deviation just shows the variation in data about the mean (I think.)
    You can get a mean from just one set of data.
    ur kidding me. how the hell do i add error bars onto it then
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    (Original post by XcitingStuart)
    Please can someone else double check my answer.





    moles = mass/molar mass or moles = concentration x volume (in dm3)
    Google says density = mass/volume (remember Google is your friend.)

    I presume volume would be 2.5ml because it's 50% of 5ml.
    As you divide 1cm by 1000 to get dm3, I guess to get dm3 for ml I'd have to divide by 100.
    So moles = concentration x volume (in dm3), so moles = 0.500mol dm-3 x 0.0025dm-3 = 0.00125 moles.

    Rearranging the moles = mass/molar mass equation gives us
    mass = moles x molar mass
    Ethanol is C2H6O
    mass = 0.00125 x (24 + 6 + 16)
    mass = 0.0575g

    So density = mass/volume (in cm3)
    So density = 0.0575g / 0.25cm3
    Spoiler:
    Show
    You probably don't need to know yet, presuming you're beginning AS.

    ethanol
    eth- denotes two carbons,
    -an- denotes only single bonds,
    -ol is the suffix for the -OH group.
    A carbon can only have 4 bonds and be stable.
    So structural formula is CH3CH2OH
    Molecular = C2H6O
    0.0025 or 0.025
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    I'll give you an example.

    10, 30, 50, 70, 90

    44, 47, 50, 53, 56

    The mean of both is 50, yet in the first example, the standard deviation is much larger because the values used to calculate the mean are spread out much further.

    That is my understanding of it, though there's always the possibility that I'm wrong, so get someone else to confer with.
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    (Original post by neverbeejail)
    0.0025 or 0.025
    oops, I forgot to finish the last calculation off.

    So density = mass/volume (in cm3)
    So density = 0.0575g / 0.25cm3
    So density = 0.23g cm-3 I suppose
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    (Original post by neverbeejail)
    ur kidding me. how the hell do i add error bars onto it then
    I have no idea about the error bars. I can interpret those, but not make them.
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    (Original post by The Wavefunction)
    Havent checked the maths but the chemistry is solid ^^
    Ty. :)
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    Count them.

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    (Original post by XcitingStuart)
    I'll give you an example.

    10, 30, 50, 70, 90

    44, 47, 50, 53, 56

    The mean of both is 50, yet in the first example, the standard deviation is much larger because the values used to calculate the mean are spread out much further.

    That is my understanding of it, though there's always the possibility that I'm wrong, so get someone else to confer with.
    yes i understand that but in your example you have repeats e.g 10,30,50 ETC
    what if i literally just have one number??

    so at time 0 i get 20 yeast cells, at time 30 i get 40 yeast cells, how can i do a standard deviation if i dont have repeats for an average??
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    (Original post by neverbeejail)
    yes i understand that but in your example you have repeats e.g 10,30,50 ETC
    what if i literally just have one number??

    so at time 0 i get 20 yeast cells, at time 30 i get 40 yeast cells, how can i do a standard deviation if i dont have repeats for an average??
    They're not repeats of a test, they're just values in the data for one test.
    But I think I get where you're coming from.
    I suppose then I'd be no variation about the mean, so SD low/non-existant.
    I don't see where that'd happen though.
    I'm not sure here.

    Is it possible for you to post the entire question?
    Edit: Perhaps you can't do a standard deviation here.
    I'm really not sure here, so I might very well be wrong with the answer in this post.
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    im ****ed
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    (Original post by XcitingStuart)
    They're not repeats of a test, they're just values in the data for one test.
    But I think I get where you're coming from.
    I suppose then I'd be no variation about the mean, so SD low/non-existant.
    I don't see where that'd happen though.
    I'm not sure here.

    Is it possible for you to post the entire question?
    Edit: Perhaps you can't do a standard deviation here.
    I'm really not sure here, so I might very well be wrong with the answer in this post.
    sir, say i have 0.550ml ethanol and 0.950 water ALSO have 0.5 ml YEAST and i want the molarity, how does the yeast affect the calculation?
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    (Original post by neverbeejail)
    sir, say i have 0.550ml ethanol and 0.950 water ALSO have 0.5 ml YEAST and i want the molarity, how does the yeast affect the calculation?
    The molarity of what? The ethanol?
 
 
 
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