1. One antacid contains 334 mg of active ingredient, NaAl(OH)2CO3. Calculate number of mmol of HCL that the table can neutralize. The Neutralization produces NaCl, AlCl3, and H2O.
2. sample of 70.5 of potassium is added to 15ml of .050M silver nitrate. Calculate the theoretical yield of the precipitate that formed.
3. What volume of .500M BaCl2 is required to completely react with 4.32g of Na2SO4?
For each of these i now that i will need to find the limiting reactant, but whats next?
2007-04-25 18:52:05 · 1 answers · asked by wqel12 1 in Science & Mathematics ➔ Chemistry
2. 70.5 mg of potassium phosphate
2007-04-26 04:15:52 · update #1
NaAl(OH)2CO3 + 4HCl -> NaCl + AlCl3 + 3H2O + CO2
Molar mass of the antacid = 144 g
millimol = 334/144 = 2.319
millimol of HCl = 4x2.319 = 9.276
2.) 70.5 ???
3) BaCl2 + Na2SO4 -> BaSO4 + 2NaCl
Molar mass of Na2SO4 = 142 g
moles of Na2SO4 = 4.32/142 = 0.03
Thus vol. = 0.03/.5 = 0.06 litres
2007-04-25 20:51:03 · answer #1 · answered by ag_iitkgp 7 · 0⤊ 0⤋