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
ionic compounds
Re: ionic compounds
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
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
Cheers Jazz
Re: ionic compounds
Thanks Jazz
rell
rell
Re: ionic compounds
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.....
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.....
Dr Robert Crosdale. MRACI. NSS. NSSA. NASA.
Ph.D (Chem), Post Grad Ph.D (Physics), M.Ed, B.Sc (Hons), Dip. Appl. Sc. (Chem)
Lake Munmorah High School.
University of New England.
University of New South Wales.
University of Newcastle.
To understand the Universe from our perspective, we need to look towards our own backyard first for answers.
** AD ASTRA PER ASPERA - SEMPER EXPLORO **
Ph.D (Chem), Post Grad Ph.D (Physics), M.Ed, B.Sc (Hons), Dip. Appl. Sc. (Chem)
Lake Munmorah High School.
University of New England.
University of New South Wales.
University of Newcastle.
To understand the Universe from our perspective, we need to look towards our own backyard first for answers.
** AD ASTRA PER ASPERA - SEMPER EXPLORO **
- nickykinz
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Re: ionic compounds
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.
Nicky
St Augustine's College
Augustine Heights, QLD 4300
St Augustine's College
Augustine Heights, QLD 4300
- Graham Kemp
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Re: ionic compounds
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).
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).
- nickykinz
- Posts: 271
- Joined: 02 Feb 2009, 12:53
- Job Title: Lab Assistant
- School: St Augustine's College
- Suburb: Augustine Heights
- State/Location: QLD
Re: ionic compounds
0.1M BaCl with 0.5M NaOH.
Nicky
St Augustine's College
Augustine Heights, QLD 4300
St Augustine's College
Augustine Heights, QLD 4300