0
$\begingroup$

I was doing a chemistry project to see if the pH of a carbonated solution effects the time taken for it to settle after being disrupted, and I am trying to map out the reaction when the components are combined.

I was able to figure out a few, but I got stuck on carbonic acid and lemon juice. For some reason, I was getting ethane as a by product of the reaction, and I'm sure that's not right. Could someone explain what I'm doing wrong?

the formula is $\ce{H2CO3 + C6H8O7}$

Improve this question
$\endgroup$
4
  • 1
    $\begingroup$ I'm assuming $\ce{C6H8O7}$ is citric acid. Acid + acid does not necessarily do anything productive. $\endgroup$
    – Ben Norris
    Commented Jan 20, 2014 at 12:35
  • $\begingroup$ if you're getting ethane there is something wrong here. are you sure it is lemon juice? $\endgroup$
    – Xiaolei Zhu
    Commented Jan 20, 2014 at 17:08
  • $\begingroup$ You should show what have you done...In my opinion there are no reactions between these two acid. When you make a lemonade you mix lemon juice that has a bit of citric acid with sparkling water that has carbonic acid and you don't smell ethane. $\endgroup$
    – G M
    Commented Jan 20, 2014 at 17:12
  • 1
    $\begingroup$ Would you mind to explain how you determined that ethane was produced? $\endgroup$
    – Klaus-Dieter Warzecha
    Commented Jan 20, 2014 at 21:07

2 Answers 2

Reset to default
1
$\begingroup$

These two weak acids have similar disassociation constants in water. A low Ka indicates a relatively small number of acid molecules will form an anion stabilized by water. Two weak acids with similar disassociation constants will coexist in a solution without interacting. If two weak acids have very different Ka then there can be a reaction. In this case nothing would happen. For more generalized information search for mixture of weak acids.

Carbonic Acid

$$\ce{H2CO3 + H2O <=> HCO3- + H3O+}$$ $$K_a = 4.3 \times 10^{-7} = \frac{[\ce{H3O+}][\ce{HCO3^-}]}{[\ce{H2CO3}]}$$

Citric Acid

$$\ce{H3C6H5O7 + H2O <=> H2C6H5O7- + H3O+}$$ $$K_a = 1.8 \times 10^{-6} = \frac{[\ce{H3O+}][\ce{H2C6H5O7^-}]}{[\ce{H3C6H5O7}]}$$

Improve this answer
$\endgroup$
0
0
$\begingroup$

By Le Chatelier's principle ,a new equilibrium will be formed for the H3O+ concentration , since H2CO3 has the lower dissociation constant.H3O+ concentration and therefore the pH will lie somewhere between the two acids

Improve this answer
$\endgroup$

Not the answer you're looking for? Browse other questions tagged or ask your own question.