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posted by  The Joker on 6/29/2008 1:12:02 PM  |  status: Live  

General Chemistry...please help..will rate lifesaver and quickly

Course Textbook Chapter Problem
General Chemistry Chemistry (7th) by Chang 4 N/A
Question Details:
The concentration of an unknown barium hydroxide solution is determined by titration with 0.0555 M HNO3
A) Complete and Balance the equation for the reaction. BA(OH)2 (aq) + HNO3---->??.
Also...If I cant solve this one, If 15.72 of the nitric acide solution is needed to neutralize 50.00 mL of the Ba(OH)2 solution, what is the molarityof the solution?
"I think I can safely say that nobody understands Quantum Mechanics"
-Richard Feyman.
".....(Fe)male...male with iron
added, for greater strength, ductility, and magnetism".(unknown)
 
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posted by KyleK on 6/29/2008 1:32:41 PM  |  status: Live
Asker's Rating: Lifesaver   
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Response Details:
A.)  Ba(OH)2(aq) + 2HNO3(aq)  -->  Ba(NO3)2(aq) + 2H2O(l)
This is simply an acid-base reaction:  OH- + H+ --> H2O

For the second part, you calculate how many moles of HNO3 you used to titrate, then use the balanced equation to find the moles of Ba(OH)2 (2 moles HNO3 to 1 mole Ba(OH)2).  Finally, convert this to molarity:

15.72 ml HNO3 x 0.0555 mol/L = 0.000872 moles HNO3
This will react with 0.000872 / 2 = 0.000436 moles Ba(OH)2
0.000436 moles / 50.00 ml = 0.00872 moles/L = 0.00872 M Ba(OH)2
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