[tiny101]

Hi there,

I've been trying to utilize the information given in this problem but to no avail. Any help would be much appreciated.

Problem: How many milliliters of 3.00M H2SO4 are required to react with 4.35g of solid containing 23.2% Ba(NO3)2 if the reaction is Ba2+ + SO4^2- --> BaSO4(s)?

I've tried incorporating the density of solid Barium Nitrate in my dimensional analysis for an answer, but that didn't seem to lead anywhere? I figure I should get the number of moles contained in the amount of Ba(NO3)2 given, but I cannot figure out how.

Thanks in advance.

[AWK]

Just calculate mass of pure Ba(NO3)3, then moles and do stoichiometry of precipitation reaction (balance it) using moles of salt and molar concentration of acid (from which moles of acid are easily calculated)

[tiny101]

How would you calculate the mass of pure Ba(NO3)2?

Thanks again.

[AWK]

http://en.wikipedia.org/wiki/Percent