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Topic: Will these reactions occur?  (Read 2811 times)

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Offline zeoblade

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Will these reactions occur?
« on: February 27, 2010, 01:51:46 AM »
I believe the following reactions will occur and will result in the following manner:

Magnesium carbonate and dilute sulfuric acid.
MgCO3(s) + H2SO4(aq) --> MgSO4(aq) + H2O(l) + CO2(g)


Nickel sulfate solution and hydrogen sulfide gas.
NiSO4(aq) + H2S(g) --> NiS(s) + H2SO4(aq)
Mainly because metal sulphides are insoluble


Aluminium chloride solution and aqueous ammonia solution.
AlCl3(aq) + 3NH3(aq) + 3H2O(l) --> Al(OH)3(s) + 3NH4Cl(aq)
or AlCl3(aq) + 3NH3(aq) + 3H2O(l) --> Al(OH)4(aq) + NH4Cl(aq)
But I don't know which one would occur and if there will be a precipitate produced.

Lithium chloride solution and potassium nitrate solution.
LiCl(aq) + KNO3(aq) --> LiNO3(aq) + KCl(aq)
I am not sure if this would proceed since they are both aqueous, how could you tell the difference?

Offline Borek

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Re: Will these reactions occur?
« Reply #1 on: February 27, 2010, 04:26:08 AM »
Aluminium chloride solution and aqueous ammonia solution.
AlCl3(aq) + 3NH3(aq) + 3H2O(l) --> Al(OH)3(s) + 3NH4Cl(aq)
or AlCl3(aq) + 3NH3(aq) + 3H2O(l) --> Al(OH)4(aq) + NH4Cl(aq)
But I don't know which one would occur and if there will be a precipitate produced.

No suh thing as Al(OH)4 - if anythng, it has to be charged.

This is tricky. I think result depends on the concentrations.

Quote
Lithium chloride solution and potassium nitrate solution.
LiCl(aq) + KNO3(aq) --> LiNO3(aq) + KCl(aq)
I am not sure if this would proceed since they are both aqueous, how could you tell the difference?

Good question - perhaps just nothing happens?
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info, pH-meter.info

Offline zeoblade

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Re: Will these reactions occur?
« Reply #2 on: February 27, 2010, 04:43:40 AM »
Sorry just a formatting error.

Would you be able to point me in the right direction to where to find information on both reactions? I want to learn more about it and especially since you said it is concentration dependent

the fourth reaction, I have a feeling now that the reaction won't occur because I have a feeling they both are highly soluble. Is that consistent in practical application?

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