Asked by NSU
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. WITH FULL EXPLANATION PLEASE!
215.0mL of Ba(OH)2 is needed to completely neutralize the acid, determine the concentration
of the Ba(OH)2 solution used. WITH FULL EXPLANATION PLEASE!
Answers
Answered by
bobpursley
a. determine moles of acid
75*.175/98
Heq*molesacid=Heqbase*Molaritybase*.215
3*75*.175/98=2*M*.215
solve for molarity of the base.
75*.175/98
Heq*molesacid=Heqbase*Molaritybase*.215
3*75*.175/98=2*M*.215
solve for molarity of the base.
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