crystal grower
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Nickel(II) something-nate sludge
I needed to make some Ni(NO3)2 so I reacted HNO3 with Ni (Nickel was in a slight excess). Beside green solution I got this weird precipitate after
filtration. I have no idea what it is. (The solution is dilute enough to Dissolve all the salt).
Can anyone help?
 
[Edited on 18-5-2018 by crystal grower]
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DraconicAcid
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Looks like nickel(II) hydroxide from not adding enough acid?
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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crystal grower
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It looks like that. I did not realize it will form hydroxide, I thought excess Ni will simply stay unreacted. I'll try adding more HNO3
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LearnedAmateur
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How could a nickel hydroxide ppt. form without some sort of base in those quantities? I thought you would need at least a small amount of ammonia or
alkali hydroxide to do so. Haven’t really had a play around with nickel compounds so I’m curious.
In chemistry, sometimes the solution is the problem.
It’s been a while, but I’m not dead! Updated 7/1/2020. Shout out to Aga, we got along well.
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DraconicAcid
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I'd guess Ni(II) hydrolyzes to give nickel hydroxide and hydronium ion, and the hydronium ion reacts with more nickel to give Ni(II) and hydrogen.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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fusso
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Quote: Originally posted by DraconicAcid  | | I'd guess Ni(II) hydrolyzes to give nickel hydroxide and hydronium ion, and the hydronium ion reacts with more nickel to give Ni(II) and hydrogen.
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Shouldn't Ni reduce HNO3 to NOx instead of H2?
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DraconicAcid
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Depends on how much nitrate ion is left in solution.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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