Asked by Biplob
A 75.0g sample of liquid contains 17.5% by mass of H3PO4 (molar mass = 98.0g/mol). If
215.0mL of Ba(OH)2 is needed to completely neutralize the acid, determine the concentration
of the Ba(OH)2 solution used
215.0mL of Ba(OH)2 is needed to completely neutralize the acid, determine the concentration
of the Ba(OH)2 solution used
Answers
Answered by
bobpursley
assuming no other acid is in the H3PO4 mix, then
a) the equation
2H3PO4 + 3Ba(OH)2>>3H2O+Ba3(PO3)2
titration equation:
nb*Ma*Va=na*Mb*Vb
nb*molesacid=na*molesbase
3*75*.175/98=2*Molaritybase*.215
solve for molarity of base
a) the equation
2H3PO4 + 3Ba(OH)2>>3H2O+Ba3(PO3)2
titration equation:
nb*Ma*Va=na*Mb*Vb
nb*molesacid=na*molesbase
3*75*.175/98=2*Molaritybase*.215
solve for molarity of base
Answered by
Wellwisher
0.00092mol/L
Answered by
Wellwisher
0.927 mol/L
Answered by
fuad
0.937
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