350 mL of 0.10 mol/L solution of magnesium bromide is mixed with a 245.5 mL of barium fluoride solution. Calculate the concentration of the barium fluoride.
is this the correct equation?
2MgBr2+ 2BaF2 --> 2BaBr2+ 2MgF2
thanks in advance!
2007-05-01 04:23:31 · 2 answers · asked by hey!!!! 1 in Science & Mathematics ➔ Chemistry
The correct equation is as you stated but without the 2s
MgBr2+ BaF2 --> BaBr2+ MgF2
from this one mole of magnesium bromide reacts with one mole of barium fluoride. The number of moles of magnesium bromide is 0.1*0.35= 0.035moles and hence this will react with 0.035moles of barium fluoride. Its concentration will be 0.035/0.2455 = 0.1426Molar or mol/L.
2007-05-01 04:31:26 · answer #1 · answered by The exclamation mark 6 · 0⤊ 0⤋
First, this isn't a redox. The equation is OK, but you can take all of the 2's out from in front of each compound, so that you have a 1:1:1:1 stoichiometry.
2007-05-01 11:27:25 · answer #2 · answered by hcbiochem 7 · 0⤊ 0⤋