An aqueous solution of barium hydroxide is
standardized by titration with a 0.199 M solution
of hydroiodic acid.
If 19.1 mL of base are required to neutralize
18.2 mL of the acid, what is the molarity of the
barium hydroxide solution?
______M barium hydroxide
Balanced chemical equation is:
2 HI + Ba(OH)2 ---> BaI2 + 2 H2O
Here:
M(HI)=0.199 M
V(HI)=18.2 mL
V(Ba(OH)2)=19.1 mL
According to balanced reaction:
1*number of mol of HI =2*number of mol of Ba(OH)2
1*M(HI)*V(HI) =2*M(Ba(OH)2)*V(Ba(OH)2)
1*0.199*18.2 = 2*M(Ba(OH)2)*19.1
M(Ba(OH)2) = 0.0948 M
Answer: 0.0948 M
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