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pH calculation????
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will'o'wisp
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0.5g of a mixture of sodium hydrogencarbonate and anhydrous sodium carbonate was dissolved in water. The solution was titrated against 0.1M hydrochloric acid, requiring 15cm^3 using phenolphthalein as indicator. Calculate the percentage by mass of sodium hydrogencarbonate in the mixture.
I have no idea where to start, ,i don't even know what to do, someone set me in the right direction.
I have no idea where to start, ,i don't even know what to do, someone set me in the right direction.
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Pigster
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#2
Sodium carbonate has two end points, one of them is the same as the end point for the hydrogencarbonate end point.
Which one does the phenolphthalein indicator change colour on?
Which one does the phenolphthalein indicator change colour on?
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will'o'wisp
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#3
(Original post by Pigster)
Sodium carbonate has two end points, one of them is the same as the end point for the hydrogencarbonate end point.
Which one does the phenolphthalein indicator change colour on?
Sodium carbonate has two end points, one of them is the same as the end point for the hydrogencarbonate end point.
Which one does the phenolphthalein indicator change colour on?
I haven't done anything redox.
I recently found this was a redox titration which i know nothing about, how nice of my teacher to put a redox titration question on a pH calculations sheet
Well so far i found some stuff on past papers and some similar questions that's how i got 48g for that other question
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will'o'wisp
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#4
(Original post by Pigster)
Sodium carbonate has two end points, one of them is the same as the end point for the hydrogencarbonate end point.
Which one does the phenolphthalein indicator change colour on?
Sodium carbonate has two end points, one of them is the same as the end point for the hydrogencarbonate end point.
Which one does the phenolphthalein indicator change colour on?
I made
NaHCO3+Na2CO3+3HCl--->3NACl+2H2O+2CO2
found mol of HCl=1.5x10^-3
3 mol of HCl=1 mol of NaHCO3
didve by 3
mol of NaHCO3=5x10^-4
mass=molxMr
=5x10^-4 x 84=0.042g
0.042/0.5 all multiplied by 100 gives me 8.4%
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Pigster
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#5
It isn't a redox titration.
The phenolphthalein changes colour when all of the CO32- converts into HCO3-.
n(HCl) required to reach this endpoint = c v = 0.1 x 15/1000 = 0.0015 mol = n(Na2CO3)
m(Na2CO3) = n x Mr = 0.0015 x 106 = 0.159 g
The rest is NaHCO3, i.e. 0.341 = 68.2%
But I am sleepy.
The phenolphthalein changes colour when all of the CO32- converts into HCO3-.
n(HCl) required to reach this endpoint = c v = 0.1 x 15/1000 = 0.0015 mol = n(Na2CO3)
m(Na2CO3) = n x Mr = 0.0015 x 106 = 0.159 g
The rest is NaHCO3, i.e. 0.341 = 68.2%
But I am sleepy.
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will'o'wisp
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#6
(Original post by Pigster)
It isn't a redox titration.
The phenolphthalein changes colour when all of the CO32- converts into HCO3-.
n(HCl) required to reach this endpoint = c v = 0.1 x 15/1000 = 0.0015 mol = n(Na2CO3)
m(Na2CO3) = n x Mr = 0.0015 x 106 = 0.159 g
The rest is NaHCO3, i.e. 0.341 = 68.2%
But I am sleepy.
It isn't a redox titration.
The phenolphthalein changes colour when all of the CO32- converts into HCO3-.
n(HCl) required to reach this endpoint = c v = 0.1 x 15/1000 = 0.0015 mol = n(Na2CO3)
m(Na2CO3) = n x Mr = 0.0015 x 106 = 0.159 g
The rest is NaHCO3, i.e. 0.341 = 68.2%
But I am sleepy.
But surely i need a balanced equation for this? Or how would i know it's a 1:1 ratio?
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