Chem revision question (1 Viewer)

[spammy679]

ok the whole question is:

"0.30 moles of magnesium oxide is completely dissolved in nitric acid (HNO3) to form a solution of magnesium nitrate. Calculate the number of moles and masses of: a) nitric acid required and b) magnesium nitrate formed"

the thing i cant get around is what else is produced besides Mg(NO3)2. Is is H2O or OH? or anything else? if not, where does the hydrogen go?

thanks

P.S. yearlies are so demanding

 

[zaa]

I'm pretty sure magnesium oxide is a base, so this is a neutralisation reaction (acid + base - -> salt + water)
So the other product should be water
Hope this helps

 

[randomnessss]

MgO (s) + 2HNO3 (aq) ----> Mg(NO3)2 (aq) + H2O (l)

This is a neutralisation reaction, and hence, acid + base ----> salt + water, where MgO is a base (metallic oxides are generally bases) and HNO3 is an acid.
In regards to your question, the hydrogen is covalently bonded to oxygen to form water.

Theoretical mole ratio - n(Mg):n(HNO3):Mg(NO3)2:H2O = 1 : 2 : 1 : 1
Therefore 0.3 moles of Mg react with 0.6 moles of HNO3 form 0.3 moles MgO and 0.3 moles of water.

Mass of HNO3 = nM
= 0.6 x (1.008+14.01+3(16))
= 37.8108 g


Mass of MgO = nM
= 0.3 x (24.31+16)
= 12.093 g

 

[spammy679]

cool
thanks a lot

good luck in exams, or if you already had them, hope you all did well

 

[randomnessss]

cool
thanks a lot

good luck in exams, or if you already had them, hope you all did well

lol thx dude, good luck for your exams too =)