Homework Help: chemistry

Posted by Michael on Wednesday, September 29, 2010 at 2:16am.

A sample of 0.6760 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.1405 g, what is the percent by mass of Ba in the original unknown compound?

chemistry - DrBob222, Wednesday, September 29, 2010 at 11:31am
Ba^+2 + SO4^= -->BaSO4.

moles BaSO4 = g/molar mass = ??
moles Ba is the same as moles BaSO4.
g Ba = moles Ba x atomic mass Ba.
%Ba = (g Ba/mass original sample)*100 =??

Answer this Question

Related Questions

ap chem - A 1.42 g. sample of a pure compound, with formula M2SO4, was ...
Chemistry - you add excess sodium sulfate to a solution of a soluble barium ...
Chemistry - you add excess sodium sulfate to a solution of a soluble barium ...
College Chem - When a0.269g sample of a barium compound was treated with excess ...
Chemistry - A 1.42-g sample of a pure compound, with formula M2SO4, was ...
AP Chem - A chemist added an excess of sodium sulfate to a solution of a soluble...
physiscs - A 10g sample of an unknown ionic compound is dissolved, and the ...
chemistry - To analyze for barium in an unknown white powder, an excess of ...
CHEMISTRY - My chem class just finished a lab in which the objective was to find...
science - Calculating A sample of barium nitrate is placed into a jar containing...

For Further Reading

First Name:
School Subject:
Answer: