NaOH + CuSO4

[NATT]

Bros i wanna know what will be the the result. I added NaOH with water and hope i made it saturated cuz i mixed em till nothing more dissolved in it. Then i put a piece of CuSO4 and they reacted very rapidly and the solution became blue and i saw a gas was emmited. Any Ideas?????

[Melvin]

Well, the copper(II) sulfate would react with sodium hydroxide in solution; this gives insoluble copper(II) hydroxide and leaves sodium sulfate in solution. I'm not really sure about the gas, though...

[NATT]

The blue solution is Na2SO4???

[DJBruce]

The blue solution is Na2SO4???

 

No the blue precipitate is [math]Cu(OH)_{2\ s}[/math]

 

The overall reaction is:

 

[math]CuSO_{4\ aq} + 2OH^{-}_{aq} \rightarrow Cu(OH)_{2\ s} + SO^{2-}_{4\ s} [/math]

 

The blue in the solution is caused by the unreacted [math]Cu^{2+}_{aq}[/math]

Edited August 12, 2009 by DJBruce

[NATT]

I saw some kinda solid particals dipsoted in the bottom.... Are they Na... something

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No the blue precipitate is [math]Cu(OH)_{2\ s}[/math]

 

The overall reaction is:

 

[math]CuSO_{4\ aq} + 2OH^{-}_{aq} \rightarrow Cu(OH)_{2\ s} + SO^{2-}_{4\ s} [/math]

 

The blue in the solution is caused by the unreacted [math]Cu^{2+}_{aq}[/math]

 

what do you think about the gas emitted?

Could u plz temme the whole reaction.......

 

what will happend to Na in NaOH

[DJBruce]

I saw some kinda solid particals dipsoted in the bottom.... Are they Na... something

 

As you said you saturated the solution with [math]NaOH_{s}[/math] it could be. If the temperature changed or you added slightly to much [math]NaOH_{s}[/math] then some of it would not dissolve and would simply collect on the bottom. Of course in the above mentioned situation the stuff on the bottom would be [math] NaOH_{s} [/math] not [math] Na [/math].

 

As a small side note their is actually no [math] Na [/math] in the solution their is [math] Na^{+}_{aq} [/math]. Although it seems trivial if there was actually [math] Na_{s} [/math] in the solution you would have a very violent reaction where [math]NaOH_{aq}[/math] is formed

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what do you think about the gas emitted?

Could u plz temme the whole reaction.......

 

what will happend to Na in NaOH

 

I left out the [math] Na^{+} [/math] in the reaction because it is a spectator ion, it simply stays in solution unreacted. If you want the reaction in it entirety here it is:

 

This is the dissociation of the sodium hydroxide.

[math] NaOH_{aq}\rightarrow Na^{+}_{aq} + OH^{-}_{aq}[/math]

 

This is the dissociation of the Copper (II) Sulfate.

[math] CuSO_{4} \rightarrow Cu^{2+}_{aq} + SO^{2-}_{aq} [/math]

 

When you mix them you get this overall reaction.

[math] 2Na^{+}_{aq} + 2OH^{-}_{aq} + Cu^{2+}_{aq} + SO^{2-}_{aq} \rightarrow Cu(OH)_{2 s} + SO^{2-}_{4 aq} + 2Na^{+}_{aq}[/math]

Edited August 12, 2009 by DJBruce
Consecutive posts merged.

[NATT]

As you said you saturated the solution with [math]NaOH_{s}[/math] it could be. If the temperature changed or you added slightly to much [math]NaOH_{s}[/math] then some of it would not dissolve and would simply collect on the bottom. Of course in the above mentioned situation the stuff on the bottom would be [math] NaOH_{s} [/math] not [math] Na [/math].

 

As a small side note their is actually no [math] Na [/math] in the solution their is [math] Na^{+}_{aq} [/math]. Although it seems trivial if there was actually [math] Na_{s} [/math] in the solution you would have a very violent reaction where [math]NaOH_{aq}[/math] is formed

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[math]\rightarrow[/math]

 

I left out the [math] Na^{+} [/math] in the reaction becuase it is a spectator ion. If you want the reaction in it entirity here it is:

 

This is the disasociation of the sodium hydoxide.

[math] NaOH_{aq}\rightarrow Na^{+}_{aq} + OH^{-}_{aq}[/math]

 

This is the disacstion of the Copper (II) Sulfate.

[math] CuSO_{4} \rightarrow Cu^{2+}_{aq} + SO^{2-}_{aq} [/math]

 

When you mix them you get this overall reaction.

[math] 2Na^{+}_{aq} + 2OH^{-}_{aq} + Cu^{2+}_{aq} + SO^{2-}_{aq} \rightarrow Cu(OH)_{2 s} + SO^{2-}_{4 aq} + 2Na^{+}_{aq}[/math]

 

Then cant Na2SO4 or kind of that thing will produce by reacting 2Na+ and SO4 2-

[Fuzzwood]

What part of the last equation don't you understand? On top of that, sodium sulphate is a fairly soluble salt, ergo it does not form a precipitate that quickly, considering copper sulphate is far less soluble and you will not have much sulphate in the first place.

[DJBruce]

Then cant Na2SO4 or kind of that thing will produce by reacting 2Na+ and SO4 2-

 

No because all group one metals are completely soluble in water, and thus dissociate. Also most sulfates are soluble in water meaning that the reaction you propose would not happen.

 

Solubility Rules

[NATT]

What part of the last equation don't you understand? On top of that, sodium sulphate is a very soluble salt, ergo it does not form a precipitate.

 

:confused:

[hannibal]

Dear NATT!

 

I can't give you an exact answer, but I wish I could join your experiment! We know so little about the concentrated solutions... Here pH is high, and CO2 dissolves easily: OH- + CO2 <-> HCO3- etc. So, it can be CO2, cause you disturbe the system. But it is more funny, if you put a smoldering stick where the gas leaves, and it begins to shining. The emitted gas can be oxygen! Copper is stable in Cu+ form in alkalines, cause the solution creates reductive environment. And the reaction between Cu2+ and some oxygen(II)-containing components can happen, by the reduction of the Cu2+ ion. And it would give you Cu+ and O2. Please examine the emitted gas! I'm curious... I will do it myself in 10 day's time...

 

happy new year, NATT!