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

Answer 1

moles acid=.175*75/98=.133 moles
you will need 3/2 *.133 moles Ba(OH)2 to neutralize...(write the balanced chem eq)
MolesBa(OH2)=Molarity*.215
Molarity=.133*1.5/.215=.93 check the math