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ionic compounds
Posted: 15 Mar 2013, 14:27
by rell
Hi everyone, i have a teacher who wants to use Copper cloride solution 0.1M & Sodium sulfide solution 0.1M.
My problem is i dont have any Sodium Sulfide.
Can someone suggest a subsitute?
Thanks Rell
Re: ionic compounds
Posted: 18 Mar 2013, 08:47
by Jazz
any of these solutions will do
AgNO3(aq) + CaCl2(aq)
• BaCl2 + Na2SO4
• Na2CO3 + CaCl2
positive ion.
• Silver nitrate
• Barium nitrate
• Lead (II) nitrate
• Strontium nitrate
negative ion.
• Solutions of:
• Sodium carbonate
• Sodium nitrate
• Sodium iodide
• Sodium Phosphate
• Sodium hydroxide
• Sodium sulfate
Re: ionic compounds
Posted: 18 Mar 2013, 09:19
by rell
Thanks Jazz
rell
Re: ionic compounds
Posted: 25 Mar 2013, 08:40
by Robb
HI All,
Great to see everyone on the ball with things, the networking is absolutely priceless for those questions and queries that many people have. Both new and old....
Cheers,
Robb.....
Re: ionic compounds
Posted: 30 Oct 2013, 12:56
by nickykinz
Should barium chloride form a precipitate with sodium hydroxide? The prac we have says it shouldn't but ours is and I just googled it and it says that Barium hydroxide is slightly insoluble.
Re: ionic compounds
Posted: 30 Oct 2013, 13:56
by Graham Kemp
What concentrations are you using, and in what proportion?
At 3.89 g/dL (20 °C), barrium hydroxide is reasonably soluable, but much less so than either sodium hydroxide (109%) or barium chloride (35.8%).
Ba(OH)2: 3.89 g/dL / 171.3425g/mol = 0.23 M.
You will not get a precipitate if you are mixing dilute solutions (~0.1M), but you may if mixing concentrated (~2.0M).
Re: ionic compounds
Posted: 30 Oct 2013, 14:40
by nickykinz
0.1M BaCl with 0.5M NaOH.