Answer to Question #148919 in General Chemistry for eeee

Question

1. A sample of 25.0 mL of 0.120 M Ba(OH)2 is titrated with 0.150 M HBr. What volume of hydrobromic acid is needed to completely neutralize barium hydroxide?

Answer 1

V(Ba(OH)₂)=25.0mL=0.0250L

n(Ba(OH)₂)= c*V = 0.0250L * 0.120mol/L = 0.003mol

Ba(OH)₂ + 2HBr = BaBr₂ + 2H₂O

n(HBr)=2n(Ba(OH)₂)=0.006mol

V(HBr)=n/c=0.006mol / 0.150mol/L = 0.040L = 40 mL