How many mL of 0.250 M BaCl2 would you need to precipitate all the sulfate ion present in 38.1 mL of 0.197 M H2SO4 solution? What is the concentration (M) of the chloride ion remaining in the resulting solution?
first see we balance reaction ,and then see 1 mole of BaCl2 reacts with 1 mole of H2SO4 gives 1 mole of BaSO4 and 2 moles of HCl .
Then first claculte moles of H2SO4 by using molarity and given volume
Molarity = moles / volume (lit)
After this we get moles of H2SO4 ,as we know that 1 mole BaCl2 reacts with 1 mole H2SO4 . So calculated moles of H2So4 reacts with same moles of BaCl2 .
So that now we have moles of BaCl2 and molarity of BaCl2 ,so easily we can calculate volume .
How many mL of 0.250 M BaCl2 would you need to precipitate all the sulfate ion...
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A 40.0-ml solution contains 0.021 M barium chloride (BaCl2). What is the minimum concentration of sodium sulfate (Na2SO4) required in the solution to produce a barium sulfate (BaSO4) precipitate? The solubility product for barium sulfate is Ksp = 1.1x10-10 Supporting Materials Periodic Table Supplemental Data Constants and Factors
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