I need to make a stock solution of 0.1 M of AlNH4(SO4)2 · 24H2O but our lab only has a bottle of compound with the formula AlNH4(SO4)2 · 12H2O. How much of the compound do I need to make a stock solution of 500ml? Also, I have already made 500 ml stock solution of 0.1M AlNH4(SO4)2 · 12H2O. Can I add more water to it to convert it to 0.1M AlNH4(SO4)2 · 24H2O?
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when you say that you need to make a stock solution of 0.1 M of AlNH4(SO4)2 · 24H2O
the water of hydration is ejust xcess baggage needed to be weighed out to get
0.1 M of AlNH4(SO4)2
whether you have made a liter of a 0.1 molar solution using
0.1 mole of 0.1 M of AlNH4(SO4)2 · 24H2O
0.1 mole of 0.1 M of AlNH4(SO4)2 · 12H2O
0.1 mole of 0.1 M of AlNH4(SO4)2 · (anhydrous)
0.1 M of AlNH4(SO4)2
all three give the same result once dissolved inwater
do not alter the 500 ml stock solution of 0.1M AlNH4(SO4)2 · 12H2O.
it is just want you want
once dissolved...
there is no difference between it and 0.1M AlNH4(SO4)2 · 24H2O
the water of hydration is ejust xcess baggage needed to be weighed out to get
0.1 M of AlNH4(SO4)2
whether you have made a liter of a 0.1 molar solution using
0.1 mole of 0.1 M of AlNH4(SO4)2 · 24H2O
0.1 mole of 0.1 M of AlNH4(SO4)2 · 12H2O
0.1 mole of 0.1 M of AlNH4(SO4)2 · (anhydrous)
0.1 M of AlNH4(SO4)2
all three give the same result once dissolved inwater
do not alter the 500 ml stock solution of 0.1M AlNH4(SO4)2 · 12H2O.
it is just want you want
once dissolved...
there is no difference between it and 0.1M AlNH4(SO4)2 · 24H2O
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Steve O is correct Take 500 ml and that is it. You can not make a solution of a hydrate in water.
If you used the hydrous salts it would be a different problem because the molecular mass very greatly due to such high hydration.All the substances contain 236g of solute per mole.
If you used the hydrous salts it would be a different problem because the molecular mass very greatly due to such high hydration.All the substances contain 236g of solute per mole.