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Topic: NaHS  (Read 5436 times)

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Offline wonghk

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NaHS
« on: April 20, 2010, 07:38:53 AM »
could NaHS be produced by the following equation with mole ratio HCl:Na2S = 1:1?
HCl + Na2S -->NaHS + NaCl

or

How can I produce a standardized HS- solution in lab?
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Offline Borek

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Re: NaHS
« Reply #1 on: April 20, 2010, 08:27:10 AM »
This is tricky, HS- is a relatively strong base so it will react further with water. You will have to control pH to be sure what you have in solution.

Why do you need HS-?
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Offline wonghk

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Re: NaHS
« Reply #2 on: April 21, 2010, 05:48:34 AM »
I am going to analyse the amount of hydrogen sulphide in river water by potentiometric titration with HS- with known concentration (at pH13) against the sample water (also at pH13) using the Ag/AgCl and Ag/Ag2S ISE but I don't know how to make a HS- solution with known concentration.
I don't know much about the experiment so i am afraid there will be some problems cropped up :-X :-X :-X
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Offline wonghk

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Re: NaHS
« Reply #3 on: April 22, 2010, 06:01:59 AM »
could anyone answer me in more detail???? thank you very much
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Offline Borek

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Re: NaHS
« Reply #4 on: April 24, 2010, 04:00:12 PM »
If you start with Na2S solution and you add enough base (NaOH) to keep it at pH 13, concentration of HS- can be calculated using equation 9.13:

http://www.chembuddy.com/?left=pH-calculation&right=pH-polyprotic-acid-base#eq9.13
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Offline wonghk

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Re: NaHS
« Reply #5 on: April 25, 2010, 02:34:56 AM »
Thank you very much. ;D ;D ;D
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