chemistry alert...
Assumptions:
Sodium sulphide (SS) formula = Na2S.9H2O, FW = 240
Each mole of SS can potentially produce 1 mole of H2S gas
Each litre of working strength solution of toner contains 5 g of SS or 5/240 = 0.021 moles so can produce 0.021 moles of H2S. (I'm assuming dilution is 1+9)
1 mole of any gas at STP (0 degrees C) occupies 22.4 litres.
0.021 moles of H2S = ~.47 litres at 0 degrees C, more at 20C.
So: Each litre of working strength toning solution could produce >0.47 litres of H2S at 20C, the recomended max concentraton is 10ppm, most safety conscious employers in my experience would aim for 10% of that if possible i.e. 1ppm, so if you estimate the litre volume of your facility you can estimate the possible max concentration and if it will be safe.
The above is definitely a worst case calculation (normally not all the H2S would be released at once and presumably there is some exhaust system in operation etc.) but for safety calculations the worst case is the one to consider. At least if you do the calculation you'll know how critical your exhaust ventilation system is.
For example a room 3 x 3 x 5 metres, 45,000 litres volume, 1 litre of working strength toner could (worst case) give you ~10ppm of H2S (0.47/45,000 litres).
I should note that while I have experience in industrial chemical safety matters and the above shouldn't be total BS you have to use your own judgement about how you use the info.
BTW SS will actually produce all its potential H2S at once in contact with acid (e.g. stop) so don't mix with acids.
Hi Dave and Jordon
thanks for your help.
But if I look at Ians formual
Part b the toner is a 1-9 dilution from the stock . sodium sulfide is 50grams for the stock to make 1litre which upon dilution makes 9 litres. therefore if I want to make 50 litres of working solution I think I would be mixing 550grams of sodium sulfide to 50 litres of water.
Am I still in possible problem areas for the issues you state?
thanks
Bob