What was the molarity of BaCl2 in the original solution if 1.653g of Barium sulfate was collected after precip?
Q. A barium mineral was dissolved in HCl to give a solution of BaCl2. An excess of potassium sulfate was added to 50 mL of this solution to precipitate all of the barium as BaSO4
Asked by help17 - Sun Oct 12 12:12:46 2008 - - 1 Answers - 0 Comments

What reagents are used to test for BaCl2 and MgCl2?
Q. you have a compound that contains either BaCl2 or MgCl2 and you need to add some reagents and check and see which one do u have. Does anyone have any idea of what to add?! Notice if you are testing for chloride both have it so either the Ba oe the MG has to be about the testing.!
Asked by M - Tue Dec 1 20:01:36 2009 - - 2 Answers - 0 Comments

A. Any soluble sulfate will precipitate out Ba++ as BaSO4 (white solid) and leave any MgCl2 in solution. So if you get a precipitate by adding a soluble sulfate to your sample, you will know it contains Ba++ ions. No precipate would show you it contains the Mg++
Answered by Fred - Tue Dec 1 20:18:08 2009

what are the products when dihydrated BaCl2 is heated?and the description of the 2 products?
Q. a test tube is filled one quarter wid dihydrated BaCl2 crystals. We were supposed to heat it and wid the standard test to identify the gases we were to find out the two products after testing, but i guess we went worng somewhere and i don't know what the produsts are. it would be great if someone new the answer
Asked by maggi - Fri Mar 21 15:32:01 2008 - - 2 Answers - 0 Comments

A. BaCl2*2H2O(s) ===> BaCl2(s) + 2H2O(g) BaCl2 is white crystals that look a lot like the dihydrate. Water comes off as steam, maybe condenses on the upper inside surface of the test tube.
Answered by steve_geo1 - Fri Mar 21 15:38:02 2008