1.028 g- mass of barium sulfate
2007-12-09 16:40:19 · 4 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
BaSO4
You don't even need the mass of BaSO4 to calculate the percentage of sulfate. We'll use a little principle called stoichiometry:
MW of BaSO4 = 233
MW of SO4 = 96
Therefore % SO4 = (96 / 233) x 100
= 41.2%
lhvinny has calculated the mass of sulfur only, not the percentage sulfate
2007-12-09 16:51:38 · answer #1 · answered by Anonymous · 1⤊ 0⤋
the formula for barium sulfate is BaSO4 with 1 mole of sulfate for every mole of barium sulfate. So to find the % of sulfate, divide the molar mass of sulfate by the molar mass of barium sulfate
96.976/233.3676=.4156
Since you want a %, multiply the answer by 100 to get 41.56%
2007-12-09 16:54:02 · answer #2 · answered by ms_farenheit1 3 · 1⤊ 1⤋
The chemical formula for Barium Sulfate is BaSO4. In order to find the mass percent, you take the mass from Sulfur and divide it by the total molar mass of the substance.
Molar Mass BaSO4 = 137 + 32 + 16*4 = 233 g/mol
Mass from Sulfur = 32 g/mol
32/233 = 13.7%
So, of your 1.028 g sample, 13.7% (or 0.137 x 1.028) is sulfur. 0.137 x 1.028 = 0.1412 g of sulfur in your sample.
2007-12-09 16:51:25 · answer #3 · answered by lhvinny 7 · 1⤊ 2⤋
Molar Mass Of Baso4
2016-10-18 00:19:08 · answer #4 · answered by ? 4 · 0⤊ 0⤋