.Sam.
  • .Sam.
I'm missing something :p
Chemistry
katieb
  • katieb
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.Sam.
  • .Sam.
A sample of ethyl propanoate is hydrolysed by heating under reflux with aqueous sodium hydroxide. The two organic products of the hydrolysis are separated, purified and weighed. Out of the total mass of products obtained, what is the percentage by mass of each product? \(\color{blue}{Ans:}32.4% and 67.6 \)% and \(67.6\)%
.Sam.
  • .Sam.
\[M_r(CH_3CH_2COOCH_2CH_3)=102g/mol\] Separated compounds should be carbox and alcohol right \[M_r(CH_3CH_2COOH)=74g/mol\] \[M_r(HOCH_2CH_3)=46g/mol\] What I've found was 38.3% and 61.7%
mathslover
  • mathslover
You are correct @.Sam.

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.Sam.
  • .Sam.
But the answer is 32.4% and 67.6% :(
mathslover
  • mathslover
The answer (from wherever it has been taken) is wrong.
mathslover
  • mathslover
The products of the hydrolysis are correct; the molecular masses are also correct then there is nothing left which could be wrong.
.Sam.
  • .Sam.
Hmm I still can't trust my answer, we'll wait for more opinions from others okay :)
mathslover
  • mathslover
Best choice. :)
anonymous
  • anonymous
You did a mistake in there. The base hydrolysis of esters results in a sodium salt rather than carboxylic acid itself. So, here you'll get sodium propanoate i.e CH3CH2COONa So your Mr will be 96. Now, your percentage by mass of each product will be: (96/142) x 100= 67.6% (46/142) x 100= 32.4%
.Sam.
  • .Sam.
Oh yeah we're not using \(H_2O\) to hydrolyse that ester, derp... Okay got it, thanks @emcrazy14 :)
anonymous
  • anonymous
yw! :)
mathslover
  • mathslover
Oh, I did 96 + 46 = 162 :D , good work @emcrazy14
anonymous
  • anonymous
First of all thanks A LOT for posting this question Sam and No wonder, I was thinking that why is he writing a product of esterification?? instead of a sodium salt?? either way thanks you all! ;D
anonymous
  • anonymous
and @emcrazy14 you too!! thanks!!! :D
anonymous
  • anonymous
:)

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