calculate the number of milliliters of .200 M Ba(NO3)2 which would be required to just precipitate all o fthe sulfate as barium sulfate
2007-09-24 22:12:44 · 4 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
the molecular mass
of MgSO4,7H2O is 24+32+4*16+7*18 =246
so1.25g =1.25/246 =0.0051mole =5.1mMole
The reaction is MgSO4+Ba(NO3)2 ---> BaSO4+ Mg(NO3)2
So you see that for 1 mole of MgSO4 you need 1 mole of Ba(NO3)2
here you need 5.1 mMole. In 1 mL of your solution there is 0.2mM of Ba(NO3)2
tne number of milliliters required is 5.1/0.2 =25.5 mL
2007-09-24 22:50:10 · answer #1 · answered by maussy 7 · 1⤊ 1⤋
Epsom Salt Formula
2016-12-17 08:26:34 · answer #2 · answered by ? 4 · 0⤊ 0⤋
Epsom Salt Chemical Formula
2016-10-01 05:07:46 · answer #3 · answered by stelter 4 · 0⤊ 0⤋
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The formula for epsom salts is MgSO4*7H2O. IF there is 1.250 g of the compound is disolved in water...?
calculate the number of milliliters of .200 M Ba(NO3)2 which would be required to just precipitate all o fthe sulfate as barium sulfate
2015-08-18 06:15:39 · answer #4 · answered by Anonymous · 0⤊ 0⤋
calculate the eq of sulphate, and divide by the concentration of your barium nitrate, you have now the volume necessary to precipitate all the sulphate.
Answer is : 25.5 ml
but you should do your homework by yourself
2007-09-24 22:52:30 · answer #5 · answered by scientific_boy3434 5 · 2⤊ 3⤋