0
$\begingroup$

As an exercise in chemistry, I decided to observe the kinetics of the decay of thiosulfate ions in an acidic medium. As far as I am aware, it is a very well known exercise among chemists.

I found a paper in which the author uses a sodium thiosulfate solution with a concentration of 0.25 mol/L and sulfuric acid with a concentration of 0.25 mol/L. I would like to know if it is okay to use hydrochloric acid with a concentration of 0.50 mol/L, instead of sulfuric acid? In other words, can I expect the same turbidity time of the aqueous solution as the author?

$\endgroup$
3
  • $\begingroup$ Not exactly, 2nd proton isn't as acidic in H2SO4, and there's a bigger issue - it an be reduced. $\endgroup$ Commented Apr 17, 2025 at 11:35
  • $\begingroup$ Considering different ionic power and just partial dissociation of HSO4^-, leading to different H+(aq) activity, the time values will be just similar/comparable. $\endgroup$ Commented Apr 17, 2025 at 11:35
  • $\begingroup$ related chemistry.stackexchange.com/questions/66141/… chemistry.stackexchange.com/questions/74021/… $\endgroup$ Commented Apr 17, 2025 at 15:45

0

Reset to default

You must log in to answer this question.

Start asking to get answers

Find the answer to your question by asking.

Ask question

Explore related questions

See similar questions with these tags.