[Jake]

Hello everyone, I'm new here and I've done my homework and still am not confident with my results, so I'd figure I'd come here for some 3rd party results.

I'm in Quantitative Analysis and I'm doing a titration lab.  Essentially, we standardized our titrant (using Hydrochloric Acid) and used it to titrate an unknown powder to find the concentration of the carbonate ions.

This is the picture of my math, and I'm hoping I did it all right.  I was wondering if people could point me in the right direction or verify I'm doing it right?  Thank you.

If you can't read my work, I'll be happy to explain it.

[Borek]

It is barely readable, but at first sight I don't see anything crying out loud "I AM WRONG!".

What was the indicator used? Are you aware of the fact that indicator choice can mean you titrated to HCO₃^- or H₂CO₃ endpoint?

[Jake]

It is barely readable, but at first sight I don't see anything crying out loud "I AM WRONG!".

What was the indicator used? Are you aware of the fact that indicator choice can mean you titrated to HCO₃^- or H₂CO₃ endpoint?

I used 4 drops of Methyl Red.  I'm aware this is a diprotic base.  I calculated the amount of HCl used at the 2nd equivalence point which was at the pH of 4.3-4.4

Essentially, I titrated it until the analyte turned a light pink (salmon?), boiled the excess carbon dioxide gas away until the solution turned yellow again and added a bit more titrant until it turned back to the salmon color.

[Borek]

OK, that's 2:1 stoichiometry then.

[Jake]

OK, that's 2:1 stoichiometry then.

So I'm doing it all right essentially other than my chicken scratch/doctor's handwriting? 

Thank you.

[Borek]

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