Check out some similar questions!

theevilbeing · Feb 23, 2007, 05:34 AM

hey, can someone please tell me the ph of coper sulphate, I can't seem to find out of the web =s

Capuchin · Feb 23, 2007, 06:32 AM

Copper sulphate doesn't have a pH on its own, because it has no H+ ions, however when you form copper sulphate solution in water, H+ ions will dissociate from the water. This would depend on the concentration, do you have any idea what concentration you are using?

I think it would be weakly acidic, but you need to know the concentration to give a proper pH

theevilbeing · Feb 23, 2007, 08:42 AM

Hey, cheers, yea I'm using concentrations from 0.01, 0.02, 0.03, 0.04, 0.05, 0.06, 0.07, 0.08, 0.09 molars. And then 0.1, 0.2, 0.3, 0.4, 0.5, 0.6, 0.7, 0.8, 0.9 and 1 molars. Cheers, I'm doing my As level biology coursework on copper as a polutant. Taz

Capuchin · Feb 23, 2007, 09:25 AM

Blimey, well for all those you might want to do the test yourse,f it's not that hard to get hold of or do :)

theevilbeing · Feb 26, 2007, 03:58 AM

cheers dude, I can't do the test because we only had like a week to do the tests in lol so I'll just have to reason my conclusion with logic. Oh dear =P Ideal soil for my seeds was between 6-8 so the copper sulphate must logically be above that to inhibit it. In theory =P I put down that it could be due to osmosis that my seeds did not germinate, because the lower osmotic potential of my copper sulphate solution prevented the seeds taking in the required 40-55% saturation required for germination. Should b all rate lol. Cheers, Taz

Capuchin · Feb 26, 2007, 04:06 AM

Copper sulphate will be quite acidic, I think that in the concentrations you were using, the pH would be below 6. But that's only an educated guess.

theevilbeing · Feb 26, 2007, 04:19 AM

Cheers =) I've just a few more pages to write now and I'm done. Haha the deadlines tomorrow. This is why they said don't go out in the holidays =P insidently: why Capuchin, as oppose to say marmoset? =) cheers again for all the help, Taz