Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: biomed77 on February 04, 2006, 11:17:23 AM
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16.0g of an impure sample of potassium hydroxide was dissolved in water and made up to 1.0dm3 in a volumetric flask. if 25cm of this solution required 50cm3 of 0.5mol dm-3 sulphuric acid for neutralisation, calculate the percentage purity of the potassium hydroxide (assuming the impurities are natural substances.
what i did is 50 x 0.5 / 25 = 1
and then 16.0 / 56 = 0.286
so purity = 0.286 / 1 x 100 = 28.6%
is that possible?? can someone correct me if wrong????
thanks :))
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IMHO question doesn't make sense. Are you sure numbers you have copied are correct?
Calculated purity is about 700%.
Note that sulfuric acid is diprotic.
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I got the same purity as Borek so there is definitely an error there in the numbers you provided.
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16.0g of an impure sample of potassium hydroxide was dissolved in water and made up to 1.0dm^3 in a volumetric flask. if 25cm^3 of this solution required 50cm^3 of 0.5mol dm^-3 sulphuric acid for neutralisation, calculate the percentage purity of the potassium hydroxide (assuming the impurities are natural substances.)
this is the original question that i have to solve...why the question does nt make sense and which numbers are incorrect???
this is the exact copy of the question maybe my solution is wrong, can you please help me???
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maybe my solution is wrong
Your solution was wrong too, but it doesn't change the fact that if you do calculations properly you will end with purity of the KOH in the range of 700% - which doesn't make sense.
Start with the reaction equation (write it here!) and calculate number of moles of KOH in the 25 mL sample. Then calculate number of moles in the 1L, then convert it to mass of KOH. Show every step of your calculations.
Note that the question wording is incorrect at least for one more (besides wrong result) reason. Impurities are not natural substances, but neutral substances.
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2KOH + H2SO4 ----> K2 SO4 + 2H2O
25 / 56 =2.24mol
so in 1L 17.86
THEN WHAT????
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2KOH + H2SO4 ----> K2 SO4 + 2H2O
OK
25 / 56 =2.24mol
No idea what you did - are you dividing 25mL by 56g? Not to mention the fact that on my calculator 25/56=0.446 and not 2.24.
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sorry i have been lazy..
i ll try again
formulae mass = 56 16.0g in 56 = 0.286 in 10cm^3 therefore 2.86 in 100cm^3 or 28.6 in 1000cm^3 so molarity = 28.6
25 x 28.6 / 1000= 0.715
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formulae mass = 56
OK
16.0g in 56 = 0.286
Thats OK, although it has nothing to do with things I have asked you to calculate
in 10cm^3 therefore 2.86 in 100cm^3 or 28.6 in 1000cm^3 so molarity = 28.6
And here I am completely at loss.
Either start again - doing exactly what you were asked to do two posts earlier, or I will be not able to help.
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Start with the reaction equation (write it here!) and calculate number of moles of KOH in the 25 mL sample. Then calculate number of moles in the 1L, then convert it to mass of KOH. Show every step of your calculations.
2KOH + H2SO4 ------> K2 SO4 + 2H2O
first it was my tutor's mistake that he wrote in the paper 0.5 mol , it is actually 0.05mol.
so 0.05 x 50 / 1000 = 2.5 x 10^-3 = 0.0025
0.0025 / 0.0025 = 1M
what do i do next????
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first it was my tutor's mistake that he wrote in the paper 0.5 mol , it is actually 0.05mol.
Happens.
2KOH + H2SO4 ------> K2SO4 + 2H2O
OK
so 0.05 x 50 / 1000 = 2.5 x 10^-3 = 0.0025
0.0025 mole of H2SO4 was used. OK
0.0025 / 0.0025 = 1M
I can only guess what you are doing here - I assume you are trying to calculate concentration of KOH. First, you forgot that sulphuric acid is diprotic, second, 0.0025L is not the same as 25mL.
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Also remember that 1.0 dm^3 = 1000 cm^3.
The first thing you need to do is calculate how many moles of Sulfuric acid were used to neutralize the solution of your unknown concentration. (Remember that the H2SO4 will be donating two moles of H+ for every moles of H2SO4). The number of moles you come up with will be how many moles of OH- are in your 25 mL sample.
Once you've gotten the number of moles in your 25 mL sample, you will then need to figure out how many moles are in your 1000 mL sample. Again, when that is figured out you'll have the total number of moles of OH- in your unknown powder which will be equal to the number of moles of KOH in your powder. Now figure out the mass of KOH you have, divide it by the total mass of the sample and you have your percentage KOH.
Post your answer when you've got it done.
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so 2 x 0.025 = 0.05 moles
0.05 x 25 / 1000 =
0.05 x 0.025 = 1.25 x 10^-3 = 0.00125 mol
is it right so far, i am really struggling with it...
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i finally got it.....i think !
formulae mass: 56moles so 16.0g in 56 = 0.286mol
moles = volume x concentration
0.286 x 25 / 1000 = 7.15 x 10^-3 = 0.00715 for potassium hydroxide
0.05 x 50 / 1000 = 2.5 x 10 ^-3 = 0.0025 for sulphuric acid
0.0025 x 2 = 5 x 10 ^-3 = 0.005
so, 0.005 /0.00715 x 100 = 69.9 = 70%
hope it is correct, if yes thanks for the guideness.. :)
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OK :)